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RACE # 01
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
2.
3.
Select the correct option for decreasing order of number of atoms.
(I) 2 gm of hydrogen
(II) 16 gm of sulphur
(III) 4 gm of oxygen
(IV) 31 gm of phosphorus
(A) II > III > IV > I
(B) IV > II > III > I
(C) I > IV > II > III
(D) I = IV > II > III
Find the correct option for 36 gm C6H12O6.
(A) 4.8 NA molecules of C6H12O6
(B) 19.2 NA electrons
(C) 0.8 moles
(D) 0.6 gm-molecules of oxygen.
Number of electrons in 36mg of
(A) 1.2 × 1021
4.
18
8
O -2 ions are (Take NA = 6 × 1023)
(B) 9.6 × 1021
(D) 1.9 × 1022
Molar mass of electron is nearly (NA = 6 × 1023, mass of electron = 9.1 × 10–31 kg)
(A) 9.1 × 10–31 kg mol–1
(C) 54.6 × 10–8 gm mol–1
5.
(C) 1.2 × 1022
(B) 9.1 × 10–31 gm mol–1
(D) 54.6 × 10–8 kg mol–1
What is the specific gravity of a liquid if 260 mL of the liquid has the same mass as 390 mL of
water ?
6.
(A) 0.66
(B) 0.5
(C) 1.5
(D) 1.8
A sample of oxygen gas ( only O2 molecules) contains O16 and O17 oxygen atoms only in
9 : 1 atomic ratio. The average molecular mass of O2, this sample, is :
(A) 32.00
(B) 16.30
(C) 32.20
(D) 33.80
Multipl correct :
7.
The number of oxygen atoms present in 24.5 gm of H3PO4 is equal to (P = 31)
(A) Number of electrons present in 1.6 gm methane (CH4)
(B) Number of molecule of CO2 present in 22 gm CO2.
(C) Number of moles of proton present in NA gm-atom of Hydrogen.
(D) Number of total atoms present in
8.
4
mol of CO2.
3
An elements has three isotopes X20 , X21 and X22. Percentage abundance (mole %) of X20 is
90 and average atomic mass of X is 20.18. Select correct option(s) (A) Percent abudance of X21 = 8%
(B) Percent abudance of X21 = 2%
(C) Percent abudance of X22 = 8%
(D) Percent abudance of X22 = 2%
Subjective :
9.
Find the volume (in ml) of monoatomic gas that contain 0.005 NA atoms at 0°C & 760 torr.
10.
Calculate the number of Na+ ion present in 142 amu of Na2SO4 in aqueous solution.
PHYSICAL /R # 01
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RACE # 02
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
A pure sample of CaCO3 contain 100 moles of total atoms. What is the mass of sample (A) 1 kg
2.
6
(B) 16 gm
(C) 8 gm
(D) 32 gm
One atom of an element X weighs 6 × 10–23 gm. Number of moles of atoms in 3.6 kg of sample of X will
be : (NA = 6 × 1023)
(B) 0.04
(C) 100
(D) 1000
0.36 gm of a triatomic gas, X3, occupies 168 ml at 1 atm & 273 K. The atomic weight of X is
(A) 48
5
(D) 1.66 kg
16
gm and it form X2 type gas. How many grams of X2 is required to fill
NA
up the gas vessel with volume 350 mL at 0°C and to obtain the pressure 2 atm -
(A) 40
4
(C) 2.0 kg
If the weight of one atom is
(A) 1 gm
3.
(B) 2.5 kg
(B) 16
(C) 24
(D) 12
Which of the following will occupy greater volume under the similar conditions of pressure and
temperature?
(A) 6 gm oxygen
(B) 0.98 gm hydrogen
(C) 5.25 gm nitrogen
(D) 1.32 gm helium
The number of electron in 3.1 mg NO3¯ is (A) 32
(B) 1.6 × 10–3
(C) 9.6 × 1020
(D) 9.6 × 1023
Multiple correct :
7.
One gm of each 1H1 , 8O16 , 6C14, 92U238 have (A) same atoms
8.
9.
(C) same nucleons
(D) Same electrons
The number of oxygen atoms present in 20.4 g of Al2O3 are equal to the number of :
(A) Oxygen atoms in 3.6 g of water
(B) Oxygen atoms in 5.4 g of water
(C) Hydrogen atoms in 5.4 g of water
(D) Hydrogen atoms in 10.8 g of water
1 mol of 147N–3 ions contains :
(A) 7 NA electrons
10.
(B) same protons
(B) 7NA protons
(C) 7 NA neutrons
(D) 14 NA protrons
1.61 gm of Na2SO4.10H2O contains same number of oxygen atoms as present in
(A) 0.98 gm H2SO4
(B) 0.08 gm SO3
(C) 1.78 gm H2S2O7
(D) 0.05 gm CaCO3
PHYSICAL /R # 02
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RACE # 03
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
Which is heaviest ?
(A) 25 g of Hg
2.
5.
(C) 6 × 6.02 × 1023
(D) 7/4 × 6.02 × 1023
(B) 1 : 2
(C) 1 : 1
(D) 2 : 1
1
mol of carbon dioxide
2
(A) it occupies always 11.2 L of volume
(B) it corresponds to
(C) it contains one g-atom of oxygen
(D) it contains 6.0 g of carbon
The ratio of the mass of C-12 atom to that of an atom of element X (whose atomicity is four) is
1 : 9. The molecular mass of element X is :(B) 432 g mol–1
(C) 36 g mol–1
(D) 84 g mol–1
Number of electrons present in 3.6 mg of NH4+ are : (NA = 6 × 1023)
(A) 1.2 × 1021
7.
(B) 5 × 6.02 × 1023
What is not correct regarding 22 g of CO2 ?
(A) 480 g mol–1
6.
(D) 4 g atoms of oxygen
A certain gaseous mixture contains methane and sulphur dioxide in ratio of 1 : 8 by mass. The ratio
of the number of molecules is :(A) 1 : 8
4.
(C) 2 moles of CO2
How many atoms are present in 1/4 mole of H2SO4 ?
(A) 3 × 6.02 × 1023
3.
(B) 2 moles of H2O
(B) 1.2 × 1020
(C) 1.2 × 1022
(D) 2 × 10–3
Which one of the following contains largest number of atoms :(A) 50 g of N2O
(B) 17 g of NH3
(C) 150 cm3 of pyridine (C5H5N), density of pyridine = 0.983 g cm–3
(D) 1 mol of N2
8.
A sample of MgSO4 contains 8 × 1020 'O' atoms what is the mass of 'S' in the sample ?
(A) 32 g
9.
(C) 3.33 × 10–2 g
(D) 50 × 10–2 g
6 × 1024 atoms of an element weight 200g. If this element forms homodiatomic gas (X2) then calculate
gram molecular mass of X2(NA= 6 × 1023)
(A) 10
10.
(B) 1.06 × 10–2 g
(B) 20
(C) 30
(D) 40
4.4 g of CO2 and 2.24L of H2 at 0ºC & 1atm are mixed in a container. Find total number of molecules
present in the container ?
(A) 6.022 × 1023
PHYSICAL /R # 03
(B) 1.2044 × 1023
(C) 2 mol
(D) 6.022 × 1024
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RACE # 04
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
Which of the following has the smallest no. of molecules :–
(A) 22.4 mL of CO2 gas at 0ºC, 1 atm
(B) 22 g of CO2 gas
(C) 11.2 L of CO2 gas at 0ºC, 1 atm
2.
3.
How many moles are there in 1m of any gas at 0ºC and 1atm :(A) 44.6 moles
(B) 44.6 × 10–3 moles
(C) 4.46 moles
(D) 44.6 × 103 mole
Calculate the total number of atoms in 5.6L of SO2 gas at 0ºC and 1 atm :–
(A)
4.
NA
4
(B)
3
N
4 A
(C) NA
(D)
3
4
Number of neutrons present in 1.7 grams of ammonia is (A) NA
5.
(D) 0.1 moles of CO2 gas
3
(B) 0.4 NA
(C) 0.7 NA
(D) 70 NA
The volume of a gas in discharge tube is 1.12 × 10–7 ml. at 0ºC and 1 atm. The number of
molecule of gas in the tube is (A) 3.01 × 104
6.
(B) 3.01 × 1015
(C) 3.01 × 1012
(D) 3.01 × 1016
If 1kg of common salt costs Rs. 7 and 1 kg of sugar costs Rs. 14. What would be the cost of
1 mole of salt and sugar (A) Both will have the same cost
(B) The cost of sugar will be half the cost of salt
(C) The cost of sugar will be more than that of the salt
(D) The cost of sugar will be twice the cost of salt
7.
A person adds 1.71 gram of sugar (C12H22O11) in order to sweeten his tea. The number of
carbon atoms added are
(A) 3.6 × 1022
8.
(B) 7.2 × 1021
(B) 30.6
(C) 28.8
(D) 29.2
Find vapour density of mixture having 64% by mass of CH4 , 32% by mass of O2 and remaining
H2 (Vapour density =
(A) 10.28
10.
(D) 6.6 × 1022
Average molecular weight of a gaseous mixture which contains 80% by mole N2 & rest O2 gas
is(A) 28
9.
(C) 0.05
mol.wt.
)
2
(B) 20.56
(C) 14.28
(D) 7.14
–
The number of F ions in 4.2 gm AlF3 is (Al = 27, F = 19)
(A) 0.05
PHYSICAL /R # 04
(B) 9.03 × 1022
(C) 3.01 × 1022
(D) 0.15
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RACE # 05
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
Balanced chemical equation is given as following :
C2H5OH (l) + 3O2(g) ¾® 2CO2(g) + 3H2O(l)
What value of the volume in litre of CO2 (g) measured at 200 K and 1 atm, produced from the
combustion of 0.25 mole of C2H5OH (l) ?
[Use R = 0.08 L atm mol–1 K–1]
(A) 5
2.
(B) 8
(C) 10
(D) 15
12 moles of each A & B are allowed to react as given : 3A + 2B ® C +
1
D . If 60 g of D is
2
produced then calculate the atomic mass of D.
(A) 30
3.
4.
(B) 45
(C) 60
(D) 15
A cylinder of compressed gas contains nitrogen and oxygen gas in the mol ratio 3: 1, if the
cylinder is known to contain 2.40 gm of oxygen. What is the total mass of gas mixture
(A) 8.7 g
(B) 7.2 g
(C) 6.8 g
(D) 6.3 g
If 0.5 mol of BaCl2 is mixed with 0.1 mole of Na 3PO4, the maximum number of mole of
Ba3(PO4)2 that can be formed is:(A) 0.7
(B) 0.05
(C) 0.30
(D) 0.10
Multiple correct :
5.
Select the correct statement(s) about chemical reaction in a closed container (A) total mass remains conserved
(B) total moles of molecules remains conserved
(C) total moles of atoms remains conserved
(D) total moles of molecules may change
6.
7.
In 2.6 kg of FeSO4 . 6H2O (At. wt. of Fe = 56)
(A) Number of atoms of O are 100 × NA
(B) Moles of H-atoms are 120 × NA
(C) Molecules of water are 60 × NA
(D) Moles of e– present in SO4 are 500
2–
5 moles of VO & 6 mole of Fe2O3 are allowed to react completely according to reaction
VO + Fe2O3 ® FeO + V2O5
The number of moles of V2O5 formed is (A) 6
(B) 2
(C) 3
(D) 5
Match the list :
8.
List-I
List-II
(Amount of substance)
(No. of moles of particular atoms in
the given substance)
24
(P) 6.022 × 10 formula units of Al2(SO4)3.3H2O
(1) 15 mole O-atoms
(Q) 90 gm C6H12O6
(2) 3 mole O-atoms
(R) 112 litre SO3(g) at 1 atm and 0°C.
(3) 2.5 mole O-atoms
(S) 54 gram N2O5 (g)
(4) 150 mole O-atoms
PHYSICAL /R # 05
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Code :
(A)
(B)
(C)
(P)
4
4
4
(Q)
2
2
1
(R)
1
3
2
(S)
3
1
3
(D)
2
1
4
3
Subjective :
9.
Based on following reaction, give minimum possible value of 'x' for 1 mol AF6.
AF6 + H2O ® AOx
10.
+ HF
A sample of NaHCO3(s) on heating undergoes 1.845 gm loss of mass. Approximate mass of
NaHCO3 (in nearest integer) in gm is
PHYSICAL /R # 05
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RACE # 06
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
12
gm / cm3 ,
p
1.
A plant virus contains spherical particles of diameter 4Å. If the density of virus is
2.
the molar mass of virus is (A) 76.8 gm/mol
(B) 9.6 gm/mol
(C) 614.4 gm/mol
(D) 128 gm/ mol
Certain mass of starch, (C6H10O5)n, is burnt completely. If 26.4 kg CO2 is produced, the mass
of water produced simultaneously is (A) 9.0 gm
(B) 18.0 kg
(C) 9.0 kg
(D) 27.0 kg
3.
Each molecules of a compound contains 5 carbon atoms, 8 hydrogen atoms and 4 × 10–23
gm of other elements. The molecular mass of compounds is (NA = 6 × 10 23)
4.
(A) 92
(B) 68
(C) 308
(D) 108
Calculate the mass of HCl (in gm) produced if 2gm H2 is mixed with 71 gm Cl2.
® 2HCl
H2 + Cl2 ¾¾
5.
(A) 35.5
(B) 72
(C) 36.5
For the reaction:
7A + 13B + 15C ¾¾
® 17P
(D) 73
If 15 moles of A, 26 moles of B & 30.5 moles of C are taken initially then liniting reactant is–
(A) A
(B) B
(C) C
(D) None of these
Matrix type :
6.
Match the column :
Column-I (Reaction)
Column-II (At the end)
(A)
(B)
50% yield
2A + 2B ¾¾¾¾¾
® 3C
4 mol
1
2
80%yield
A + 2B ¾¾¾¾¾
®C
4 mol
(C)
(D)
6 mol
15 mol
5 mol
3 moles C formed
(Q)
3.2 moles C formed
(R)
A is limiting reagent
(S)
B is limiting reagent
(T)
1.6 moles C formed
8 mol
60%yield
3A + 2B ¾¾¾¾¾
®C
A
(P)
20 mol
+ 3B
12 mol
20%yield
¾¾¾¾¾
® 2C
Subjective :
7.
A person produce 2.5 L gastric juice per day, which contains 3.65 gm HCl per litre. The
minimum integer number of antacid tablets, each containing 870 mg Mg(OH)2, which should
be taken by that person to neutralise all HCl produce in one day, is : [Mg = 24]
8.
P & Q are two elements which form P2Q3 and PQ2 molecules. If 0.15 mole each of P2Q3 and
PQ2 weighs 15.9 gm and 9.3 gm respectively. Calculate the atomic weights of P and Q.
9.
An element X is found to combine with oxygen to form X4O6. If 8.4 gm of this element combines
with 6.4 gm of oxygen, then calculate the atomic weight of X.
10.
Moles of glucose, which produce a total of 744 gm CO2 and water on complete combustion,
is :
PHYSICAL /R # 06
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RACE # 07
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
Mass ratio of NH3 and CO2 for maximum product formation as per reaction :
2NH3 + CO2 ® NH2COONH4
(A)
2.
17
22
(A)
17
40
22
17
(D)
44
17
(B)
4
7
(C)
17
56
(D) None of these
A given initial mass of KClO3 on 50% decomposition produces 67.2 litre oxygen at 0ºC and
1 atm. The other product of decomposition is KCl. The initial mass of KClO 3 (in gm) taken
is.
(B) 122.5
(C) 490
(D) 735
A mixture containing 3 moles each of C4H8 and C6H6 undergoes complete combustion with
O2 to form CO2 and H2O. Calculate total mass of CO2 produced
(A) 1320 gm
5.
(C)
7
O ¾¾
® 2NO2 + 3H2O
2 2
(A) 245
4.
17
44
To obtain maximum mass of NO2 from a given mass of a mixture of NH3 and O2, the ratio of
mass of NH3 to O2 should be
2NH3 +
3.
(B)
(B) 610 gm
(C) 528 gm
(D) 792 gm
Calculate % yield of the reaction if 1 Kg KHCO3 produces 110 g of CO2 upon strong heating.
(A) 25
(B) 75
(C) 50
(D) 80
Multiple correct :
6.
For reaction :
2Fe2S3 + 6H2O + 3O2 ¾¾
® 4 Fe(OH)3 + 6S
If 4 moles of Fe2S3 react completely with 2 mole of H2O and 3 moles of O2, then which of the
following statement (s) is/are correct(A) H2O is limiting reagent
(B) Moles of Fe(OH)3 formed is 4/3
(C) Moles of Fe2S3 remaining is 10/3
(D) Mass of O2 remaining is 32 gm
PHYSICAL /R # 07
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7.
For reaction
MnO2 + 4HCl ¾¾
® MnCl2 + 2H2O + Cl2(g)
261 gm MnO2 mixed with 448 litre of HCl gas at 273°C & 1 atm pressure to produce product.
[NA = 6 × 1023; Atomic mass of Mn = 55, Cl = 35.5]
Select correct statement(s).
(A) MnO2 is limiting reagent
(B) Chlorine gas produced contains 15 × 10 23 molecules.
(C) Moles of excess reactant left is 0.5 moles
(D) If % yield of reaction is 50%, then mass of MnCl2 obtained will be 315.
Subjective :
8.
42 gm of a mixture of propyne (C3H4) and oxygen gas is collected in a vessel and fired. The
maximum possible mass ( in gm) of water formed is-
9.
27 gm of Al react with excess of oxygen to give 4.59 gm of Al2O3. Calculate percentage yield
of reaction.
10.
If 5g H2 is mixed with 14g of nitrogen gas for the following reaction
N2 + 3H2 ® 2NH3
At the end , mass (in gm) of H2 left unreacted is
PHYSICAL /R # 07
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RACE # 08
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
2 moles of KClO3 is completely decomposed to produce O2. How many moles of butane can be
completely burnt by the O2 gas produced
(A) 0.5 mole
2.
(B) 1 mole
(C) 2 mole
(D) 3 mole
20 gm pyrolusite ore exactly requires 29.2 gm HCl for complete reaction :
MnO2 + 4HCl ® MnCl2 + Cl2 + 2H2O
The mass percent of pure MnO2 in the pyrolusite ore is ( Mn = 55)
(A) 17.4 %
3.
(B) 87 %
(C) 43.5 %
(D) 14.6 %
How many gram glucose should be burnt completely to produce sufficient CO2 which may
convert 12 gm NaOH into Na2CO3 ?
(A) 4.5 gm
4.
(B) 9.0 gm
(C) 2.25 gm
(D) 13.5 gm
10 gm NaOH and 9.8 gm H2SO4 are allowed to react by which 8.52 gm Na2SO4 is formed.
The percentage yield of products is (A) 60 %
5.
(B) 48 %
(C) 100 %
(D) 75 %
20 gm of a chalk sample is dissolved completely in excess of dilute HCl solution. If 3.36 L CO2
gas is produced at 273K and 1atm, the percentage of pure CaCO3 in chalk is (assume that
the impurities are inert to HCl and CO 2 is completely insoluble in water)
(A) 25 %
6.
(B) 50 %
(C) 75 %
(D) 80 %
When a solid mixture of NaHCO3 and Na2CO3 is strongly heated to 500K in an open vessel,
the mass of sample decreases. The decrease is (A) Only due to CO 2(g) formed by decomposition of Na 2CO3
(B) Only due to CO 2(g) formed by decomposition of NaHCO3
(C) Only due to CO2(g) formed by decomposition of both, Na 2CO3 and NaHCO3
(D) Due to CO2(g) and water vapour formed by decomposition of NaHCO 3
7.
1.5 gm mixture of SiO2 and Fe2O3 on very strong heating leave a residue weighing 1.46 gm. The
reaction responsible for loss of weight is
Fe2O3 (s) ¾® Fe3O4 (s) + O2(g)
What is the percentage by mass of Fe2O3 in original sample.
(A) 80%
(B) 20%
(C) 40%
(D) 60%
8.
An organic compound contains 40% carbon atom 6.67% hydrogen atoms and remaining oxygen atoms
by mass. The empirical formula will be (A) CH 2
PHYSICAL /R # 08
(B) CH2O
(C) C2H4O2
(D) CH3O
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Matrix type :
9.
Match the column :
Column-I (compund)
Column-II (Relative amounts of products
on complete combustion)
(A)
CH 4
(P)
Moles of CO2 < Moles of H2O
(B)
C2 H 4
(Q)
Moles of CO2 = Moles of H2O
(C)
C2 H 2
(R)
Moles of CO2 > Moles of H2O
(D)
C3 H 8
(S) Mass of CO2 > Mass of H2O
Subjective:
10.
62.5 gm of a mixture of CaCO3 and SiO2 are treated with excess of HCl and 1.1 gm of CO2 is
produced. What is mass % CaCO3 in the mixture.
PHYSICAL /R # 08
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RACE # 09
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PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
A monobasic acid contains : N = 22.22%, H = 1.59% and rest oxygen atoms. The number of oxygen
atoms in the molecular formula of acid is (A) 1
(B) 3
(C) 4
(D) 2
2.
A metal sulphate is isomorphous with CaSO4. 2H2O and contains 10%S. What is atomic weight of metal
(Given : Ca = 40, S = 32)
(A) 108
(B) 94
(C) 188
(D) 208
3.
What is % H2O in CuSO4.5H2O (Cu = 64, S = 32)
(A) 36%
(B) 7.2%
(C) 20%
(D) 25%
4.
2.8 gram of an organic compound treated according Kjeldahl's method and evolved NH3 was absorbed
in aqueous sulphuric acid solution having 0.01 mole of sulphuric acid. Find % of N in organic
compound
(A) 14%
(B) 5%
(C) 20%
(D) 10%
5.
Which compound, contain equal percentage of all elements in its compound (A) CO2
(B) HCOOH
(C) SO2
(D) CH 3COOH
6.
A hydrocarbon (containing only carbon, hydrogen) on complete combustion gave 4.4 gm CO2 and
1.8 gm H2O. What is it's empirical formula
(A) CH2
(B) CH
(C) CH3
(D) C2H5
7.
An oxide of iron contains 70% iron by mass, simplest formula of oxide is [Fe = 56]
(A) FeO
(B) Fe2O3
(C) Fe2O
(D) Fe3O4
Subjective :
8.
Calculate the amount of ZnO produce (in gram) when 390 gram of ZnS reacts with 179.2 litre O2 at
1 atm and 273 K [Zn = 65.5]
ZnS + O2 ® ZnO + SO2
9.
90 g of a silver coin was dissolved in strong nitric acid, and excess of sodium chloride solution was
added. The silver chloride precipitate was dried and weighed 71.75 g. Calculate the percentage of silver
in the coin (Atomic mass of Ag = 108)
Ag + 2HNO3 ¾® AgNO3 + NO2 + H2O
AgNO3 + NaCl ¾® AgCl + NaNO3
10.
Prepration of Na2SnO2 involves the following set of reaction.
(i) Sn + 2HCl ¾® SnCl2 + H2
(ii) SnCl2 + 2NaOH ¾® Sn(OH)2 + 2NaCl
(iii) Sn(OH)2 + 2NaOH ¾® Na2SnO2 + 2H2O
(a) Mass of Sn (in kg ) required to produce 19.7kg Na2SnO2, assuming 100% yield of each reaction.
(b) If % yield of reaction (i), (ii), (iii) 25%, 50% , 40% respectively. Calculate the mass of Sn (in kg)
required to produce 19.7kg of Na2SnO2. [Sn = 119]
PHYSICAL /R # 09
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RACE # 10
PHYSICA L CHEMISTRY
MAX. TIME : 20 Min.
Single correct :
1.
Find % (w/v) of 20% (w/w) H2SO4 solution, if density of solution is 1.2 gram / ml.
(A) 24%
(B) 12%
(C) 20%
(D) 16.6%
2.
Molality of pure liquid benzene (C6H6) if its density d = 2 gram/ml is (A) 2m
(B) 0.78 m
(C) 12.8 m
(D) 50 m
3.
30 ml , 50% (v/v) HCl added into 70 ml, 20% (v/v) HCl solution. Find % (v/v) of resultant soluiton
(A) 14
(B) 29
(C) 15
(D) 70
4.
A deci-molar solution of urea is diluted 100 times. It's final molarity is (A) 10–2
(B) 10–3
(C) 10
(D) 100
5.
Mole fraction of aqueous solution of CH3COOH is 0.1. Select incorrect statement (A) % (w/w) = 27
6
(B) Molality = 6.17 m (C)
M solute
× 100
(M solute + M solvent)
W
HO
= 27
(D) W
CH COOH
2
3
(B) 50%
M solute
× 100
M solvent
Decreasing order (first having highest & then others following it) of mass of pure NaOH in each of the
aqueous solution
(i) 50 gm of 40% (w/w) NaOH
(ii) 50 gm of 50% (w/v) NaOH [dsoln. = 1.2 gm/ml]
(iii) 50 gm of 20 M NaOH [dsoln. = 1 gm/ml]
(A) (i), (ii), (iii)
(B) (iii), (ii), (i)
(C) (ii), (iii), (i)
(D) All contain same wt. of NaOH
(C) 66.67 %
8.
N CH3COOH
=9
If ratio of mole fraction of solute to solvent is unity, what would be % by wt. (concentration of solute)
(M solute = molecular mass of solute, M solvent = M molecular mass of solvent)
(A)
7
N H2O
(D)
100 ml. aqueous solution (density =
5
gm/ml) contain 40 % by weight NaOH. The number of molecules
3
of NaOH dissolved in the above solution is :
(Use NA = 6 × 1023)
(A) 2 × 1022
(B) 3.33 × 1022
(C) 1024
(D) 3.33 × 1023
Multiple correct :
9.
90 gm glucose is dissolved in 800 gm water to get a solution of density
concentration of solution is /are (A)
90
% (w/w)
8
(B)
90
% (w/v)
8
(C) 0.625 m
89
gm / ml. The correct
80
(D) 0.625 M
SUBJECTIVE:
10 Calculate molarity of NaOH in a solution made by mixing 2 lit. of 1.5 M NaOH, 3 lit. of 2M NaOH and
1 lit. water.
PHYSICAL /R # 10
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RACE # 11
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
Single correct
1.
What volume of 95% H2SO4 by weight (dsolution = 1.85 g/ml) must be taken to prepare 100 ml of 15%
æwö
ç ÷ solution of H2SO4 (dsolution = 1.1 g/ml)
èwø
(A) 9.4 ml
2.
3.
(B) 18.8 ml
(C) 28.2 ml
(D) 56.4 ml
How many gram of KCl is required to make it's 500 ml solution of molarity 0.1M. (K = 39, Cl = 35.5)
(A) 3.725
(B) 1.8625
(C) 0.745
(D) 7.45
æwö
500mL, 0.2M Na2SO4 solution is mixed with 100 mL , 17.1% ç ÷ Al2(SO4)3 solution and resulting
èVø
–2
solution is diluted to 5 times. Find the molarity of SO4 ions in the final solution
[Mw of Al= 27, s = 32, Na = 23]
(A)
1
M
12
(B)
5
M
12
(C)
7
M
5
(D)
12
M
5
Multiple correct :
4.
Select the correct statement(s) :
(A) Ratio of gm/litre & % w/v of a solution is independent of solute substance.
(B) Ratio of % w/v and molarity of a solution depends on solute substance.
(C) Ratio of % w/v and molarity of a solution depends on solvent substance
(D) Ratio of % w/v & ppm for any solution is same
5.
400 ml 0.1 M BaCl2 is mixed with 600 ml 0.1 M H2SO4 to form product according to following reaction
BaCl2 + H2SO4 ¾¾
® BaSO4 + 2HCl
Select the correct option(s), after reaction is completed
(A) Molarity of Ba+2 ions in final solution is 0.04 M
(B) Molarity of SO42– ions in solution is 0.02 M
(C) Molarity of H+ ions do not change on mixing
(D) Final molarity of H+ ion in soluiton is 0.12 M
6.
Aqueous solution containing 30gm CH3COOH are (A) 250 ml of 2M CH3COOH solution
(B) 600 gm of 5% (by wt.) CH3COOH solution
(C) 111gm of solution in which mole fraction of CH3COOH is 0.1
(D) 500 gm of 7m CH3COOH solution
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Molarity of solute A (mol.wt. = 60) and B (mol.wt. = 40) in an aqueous solution are 2M each.
(Density of aqueous solution is 1.2 gm/ml.)
(A) Molality of A in the solution is 2m
(B) Molality of B in the solution is 2m
(C) wt% of B in the solution is 10%
(D) wt % of A in the solution is 10 %
Subjective :
8.
1000 ml solution of CaBr2 contain 200 gm CaBr2. If density of solution is 1200 kg/m3 , calculate molarity
of solution
9.
What volume (in litres) of 0.4 M HCl completely reacts with 0.5 M , 4 litre of NaOH solution
10.
What is Cl– concentration (in M) in 2.5 M BaCl2 solution which is 80% dissociated ?
PHYSICAL /R # 10
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RACE # 12
JEE (Main + Advanced) 2022
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NURTURE COURSE
NURTURE COURSE
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
Single correct :
1.
200 ml of an aqueous solution of glucose (C6H12O6) has molarity of 0.01M. Which of the following
operations can be done to this solution so as to increase molarity to 0.015 M ?
(A) Evaporate 50 ml water from this solution
(B) Add 0.18 g glucose to solution without changing its volume
(C) Add 50 ml water to this solution
(D) None of these
2.
3.
4.
5.
6.
7.
A gaseous mixture of C3H8 and CH4 exerts a pressure of 320 mm Hg at temperature TK in a V litre
flask. On complete combustion of mixture, flask containing only CO2 exerts a pressure of 448 mm Hg
under identical condition. The mole fraction of C3H8 in the given mixture is
(A) 0.35
(B) 0.5
(C) 0.2
(D) 0.4
50 ml Toluene [C6H5CH3(g)] undergoes combustion with excess of oxygen. Calculate the volume
contraction.
(A) 50 ml
(B) 150 ml
(C) 75 ml
(D) 100 ml
The questions below to consist of an Assertion and the Reason. Mark appropriate option using the
given directions.
Assertion : Molarity & molality for very dilute aqueous solution is approximately same
Reason : For all aqueous solution total mass of solvent is approximately equal to total volume of
solution.
(A) If both Assertion and Reason are CORRECT, and Reason is the CORRECT explanation of
the Assertion.
(B) If both Assertion and Reason are CORRECT, but Reason is not the CORRECT explanation of
the Assertion.
(C) If Assertion if CORRECT but Reason is INCORRECT.
(D) If Assertion is INCORRECT Reason is CORRECT.
An alkane on complete combustion with O2 shows 50% of volume contraction. Molecular formula of
alkane is (A) C4H10 (g)
(B) CH4 (g)
(3) C2H6 (g)
(D) C3H8 (g)
A sample of H2SO4 solution having density 1.96g/ml. If 50 ml of this solution is completely neutralize
by 2M, 100ml NaOH solution. Wt % of H2SO4 in the solution is.
(A) 6 %
(B) 12.5 %
(C) 10 %
(D) 2 %
Which of the following is incorrect for 17g/L of H2O2 solution ?
(A) Volume strength is 5.6
(B) Molarity of solution is 0.5M
(C) 1 ml of this solution gives 2.8 ml O2 at 273K and 2 atm
(D) The molarity of solution is 2M
PHYSICAL /R # 12
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8.
Match the column :
(P)
Column-I
Column-II
20% (w/w) solution of KOH
(A) 8.64 M
(density of solution = 1.02 gm/mL)
(Q) Solution containing 864 gm
(B) 3.64 M
of CaCO3 in a 1 L.
(R)
Volume of 1.204 × 1024
(C) 5 mL
molecules of water at 4°C
(S)
Volume of 0.2 M NaOH solution
(D) 36 mL
containing 40 mg of NaOH
Code :
P
(A) 4
(B) 2
(C) 4
(D) 2
9.
R
2
3
3
4
S
3
4
2
3
5 ml of 1.2 M- NaOH solution is diluted till the concentration becomes 2% (w/v). Assuming volume
to be additive, the volume of water added for dilution is (A) 12 ml
10.
Q
1
1
1
1
(B) 7 ml
(C) 19 ml
(D) 5ml
An aqueous glucose solution of density 1.71 gm /ml has mole-fraction of solute equal to 0.10. The molarity
of solution is (A) 0.5 M
PHYSICAL /R # 12
(B) 5.0 M
(C) 2.5 M
(D) 1.5 M
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RACE # 13
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
Single correct :
1.
The air contains 78% N2 & 22% O2 by volume. The volume occupied by 40 gm air at 20°C &
745 mm Hg pressure approximately.
(A) 34 lit.
(B) 34 ml
(C) 3.4 K. lit.
(D) 3.4 lit.
2.
Human lungs can absorb 8 gm O2 per hour by respiration. If all oxygen atoms are converted to
carbohydrates (C6H12O6) how long will it take to produce 180 gm C6H12O6
(A) 8 hour
(B) 12 hour
(C) 10 hour
(D) 6 hour
Paragraph type :
Pagraph for Q.3 to Q.5
Labelled as '% oleum' , it means maximum amount of H2SO4 that can be obtained from 100 gm of such
oleum (mixture of H2SO4 and SO3) by adding sufficient water. For ex. 109 % oleum sample means,
with the addition of sufficient water to 100 gm oleum sample 109 gm H2SO4 is obtained.
% labelling of oleum sample = (100 + x)%
x = mass of H2O required for the complete conversion of SO3 in H2SO4
3.
50 gm of 109 % oleum is mixed with 50gm of another 118% oleum. Calculate the maximum weight of
H2SO4 which can be obtained from the resulting mixture.
(A) 100 gm
(B) 113.5 gm
(C) 127 gm
(D) 118 gm
4.
What is the maximum mass of H2SO4 that can be obtained from a 100 gm oleum sample labelled as
110%
(A) 110 gm
(B) 120 gm
(C) 90 gm
(D) 115 gm
5.
25 gm of an oleum sample contains 15 gm H2SO4. What is % labellling of this oleum sample (A) 104.5
(B) 109
(C) 118
(D) 115
Subjective :
6.
An alkene upon combustion produces CO2(g) and H2O(g). In this combustion process, if there is no
volume change then the no. of C atoms per molecule of alkene, is.
7.
The % by volume of C4H10 in a mixture of C4H10, CH4 and CO is 41, then calculate volume of
CO2 (in ml) produced when 100 ml of mixture is burnt in excess of O2.
8.
What volume (in ml) of 0.8 M - Ca(NO3)2 solution should be mixed with 40 ml of 0.6M - Al(NO3)3
solution to get a solution having NO3– ion concentration equal to 1.70 M ?
9.
80 ml of 0.5 M - Na2SO4 solution is mixed with 100 ml of 0.4 M - BaCl2 solution. The molarity of Na+
ion in the resulting solution is.
10.
H2O2 decomposes as :
2H2O2(aq.) ® 2H2O(l) + O2(g)
If 50% of H2O2 present in 400 ml of 0.4M - H2O2 solution decomposed as above, the volume ( in L) of
O2(g) produced at 27ºC and 608 torr is (R = 0.08 L-atm/K-mol)
PHYSICAL /R # 13
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RACE # 14
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
1.
Calculate the O.N. of all atoms in following compounds:-
(i)
Fe3O4
(ii)
Na2S4O6
(iii)
C2H 5OH
(iv)
FeSO 4.(NH4)2SO4.6H2O
(v)
FeS2
(vi)
CrO5
(vii)
(N2H5)2SO4
(viii)
N2 O 5
(ix)
HCN
(x)
HNC
(xi)
Ba[H2PO2]2
(xii)
OsO4
(xiii)
H 2S 2O 3
(xiv)
CH3 SO3 H
(xv)
Ba2XeO6
(xvi)
Ba(SCN)2
Single correct :
2.
3.
Which of the following is correctly matched :Compound
Oxidation number
(a) AlF3
(P) +2.5
(b) P4O10
(Q) +7
(c) HClO4
(R) +5
2–
(S) +3
(d) S4O6
(a)
(b)
(c)
(d)
(A) P
Q
R
S
(B) S
R
Q
P
(C) S
R
P
Q
(D) P
Q
S
R
The oxidation number of oxygen in KO3 and Na2O2 is respectively :(A) 3, 2
4
6.
(C) 0, 1
(D) –0.33, –1
In which of the following compound, the oxidation state of sulphur is +7 ?
(A) Na2S2O8
5.
(B) 1, 0
(B) H2S2O7
(C) H2SO5
(D) None of these
In the sulphur molecule, S8
(A) Valency of S is 0
(B) Valency of S is –2
(C) Oxidation state of S is 0
(D) Oxidation state of S is +2
Of the following elements, which one has the same oxidation state in all of its compounds ?
(A) Hydrogen
(B) Fluorine
(C) Carbon
(D) Oxygen
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7.
Oxidation number of Fe in Fe3O4 are :
(A) +2 and +3
8.
9.
(C) +1 and +3
(D) None
Which of the following compounds are arranged in increasing oxidation number of S :–
(A) H2SO3, H2S, H2SO4, H2S2O3
(B) H2S2O3, H2SO3, H2S, H2SO4
(C) H2S, H2SO3, H2SO4, H2S2O3
(D) H2S, H2S2O3, H2SO3, H2SO4
Oxidation number of sodium in sodium amalgam is
(A) +1
10.
(B) +1 and +2
(B) 0
(C) –1
(D) +2
A compound contains atoms A, B and C. The oxidation number of A is +2, of B is +5 and of
C is –2. The possible formula of the compound is :
(A) ABC2
PHYSICAL /R # 14
(B) B2(AC3)2
(C) A3(BC4)2
(D) A3(B4C)2
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RACE # 15
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
Single Correct :
1.
The reaction H2S + H2O2 ® S + 2H2O manifests :
(A) Oxidising action of H2O2
(B) Reducing nature of H2O2
(C) Acidic nature of H2O2
(D) Alkaline nature of H2O2
2.
If an element is in its lowest oxidation state, under proper conditions it can act as :
(A) Reducing agent
(B) An oxidising agent
(C) Oxidising as well as reducing agent
(D) Neither oxidising nor reducing agent
3.
Reaction
(A) S–2 + 4 H2O2 ® SO42– + 4 H2O
(B) Cl2 + H2O2 ® 2HCl + O2
The true statement regarding the above reactions is :
(A) H2O2 acts as reductant in both the reactions.
(B) H2O2 acts as oxidant in reaction (A) and reductant in reaction (B).
(C) H2O2 acts as an oxidant in both the reactions.
(D) H2O2 acts as reductant in reaction (A) and oxidant in reaction(B)
4.
5.
In the reactions:C + 4HNO3 ® CO2 + 2H2O + 4NO2
HNO3 acts as :–
(A) An oxidising agent (B) An acid
(C) A reducing agent
(D) A base
Which species are oxidized and reduced in the reaction ?
FeC2O4 + KMnO4 ¾® Fe3+ + CO2 + Mn2+
(A) Oxidised : Fe, C ; Reduced : Mn
(B) Oxidised : Fe ; Reduced : Mn
(C) Reduced : Fe, Mn ; Oxidised : C
(D) Reduced : C ; Oxidised : Mn, Fe
Multiple Correct :
6.
Which of the following can only acts as oxidising agent?
(A) KMnO4
(B) K2MnO4
(C) H2O2
(C) SO2
7.
The compound that can work both as an oxidising as well as reducing agent is :
(A) KMnO4
(B) H2O2
(C) Fe2(SO4)3
(D) K2Cr2O7
8
Which of the following process is neither oxidation nor reduction ?
(A) SO42– ® SO3
(B) Cr2O72– ® CrO42–
(C) PO43– ® P2O74–
(D) C2O42– ® CO2
PHYSICAL /R # 15
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9
Which of the following compound(s) can not decolurise acidified KMnO4 solution
(A) SO2
10.
11.
12.
(B) FeCl3
(C) H2O2
(D) FeSO4
Find out the oxidation number per atom of the underlined elements :
(a)
K2Cr2O7
(b)
K4Sb2O7
(c)
MnO4–
(d)
MnO2
(e)
ClO
–
(f)
Ni(CO)4
(g)
MnO
(h)
K2MnO4
(i)
Cr2O3
(j)
NaBH 4
(k)
MgSO4
(l)
SiCl4
(m) P4O10
(n)
HClO4
(o)
HAuCl4
(p)
CuI
(q)
CuO
(r)
Tl2O
(s)
Cu 2O
(t)
CaCO 3
(u)
V2O 5
(v)
KClO3
(w) NO 3–
(x)
SO32–
(y)
NaHSO4
(z)
NaH2PO 4
Classify each of the following unbalanced half–reactions as either an oxidation or a reduction :
(a)
Cl2(g) ¾¾® Cl–(aq.)
(b)
S2O32–(aq.) ¾¾® S4O62–(aq.)
(c)
NH3(g) ¾¾® NO(g)
(d)
C2O42–(aq.) ¾¾® CO2(g)
(e)
Hg22+(aq.) ¾¾® Hg2+(aq.)
(f)
Pb3O4(s) ¾¾® PbCl2(aq.)
Identify the oxidant and reductant in the following reactions :
(a)
Cr2O72–(aq.) + 3SO32–(aq.) + 8H+(aq.) ¾¾® 2Cr3+(aq.) + 3SO42– (aq.) + 4H2O(l)
(b)
2AgBr(s) + C6H6O2(aq.) ¾¾® 2Ag(s) + 2HBr(aq.) + C6H4O2(l)
(c)
N2H4(l) + 2H2O2 (l) ¾¾® N2(g) + 4H2O(l)
(d)
Pb(s) + PbO2(s) + 2H2SO4(aq.) ¾¾® 2PbSO4(s) + 2H2O(l)
(e)
C6H5CHO(l) + 2[Ag(NH3)2]+(aq.) + 3OH– ¾¾® C6H5COO– (aq.) + 2Ag(s) + 4NH3(aq.)
+ 2H2O(l)
¾¾
® NaI(aq.) + Na2S4O6(aq.)
(f)
I2(s) + Na2S2 O3(aq.)
(g)
Cl2O7(g) + H2O2(aq.) ® ClO2–(aq.) + O2(g) + H+ (aq.)
PHYSICAL /R # 15
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RACE # 16
PHYSICA L CHEMISTRY
MAX. TIME : 60 Min.
Single correct :
1.
Balance the following reaction
–
OH
® cZn2+ + NH4+ + dOH–
aZn + NO3– + bH2O ¾¾¾
2.
(A) a = 4, b = 7, c = 4, d = 10
(B) a = 2, b = 5, c = 6, d = 8
(C) a = 3, b = 3, c = 1, d = 9
(D) a = 1, b = 3, c = 7, d = 8
Which of the following is not a disproportionation reaction :(A) P4 + NaOH ® NaH2PO2 + PH3
(B) BaC2 + N2 ® Ba(CN)2
(C) Hg2I2 ® HgI2 + Hg
–
–
(D) Cl2(g) + 2OH–(aq) ® ClO(aq)
+ Cl(aq)
+ H2O
3.
Which reaction does not represent auto redox or disproportionation ?
4.
(A) Cl2 + OH– ¾® Cl– + ClO3– + H2O
(C) 2Cu+ ¾® Cu2+ + Cu
In the balanced chemical reaction,
(B) 2H2O2 ¾® H2O + O2
(D) (NH4)2Cr2O7 ¾® N2 + Cr2O3 + 4H2O
IO3– + aI– + bH+ ¾® cH2O + dI2
a, b, c and d respectively correspond to :(A) 5, 6, 3, 3
(B) 5, 3, 6, 3
(C) 3, 5, 3, 6
(D) 5, 6, 5, 5
Multiple correct :
5
In which of the following reaction(s), hydrogen(H2) is acting as an oxidising agent (A) With iodine, to give hydrogen iodide
(B) With lithium, to give lithium hydride
(C) With nitrogen, to give ammonica
(D) With oxygen, to give water
6
The oxide(s) which can not act as a reducing agent is/are (A) SO2
7.
(B) NO2
(C) CO2
(D) ClO2
In which of the following reaction(s), H2O2 acts as a reducing agent
(A) PbO2(s) + H2O2(aq.) ® PbO(s) + H2O(l) + O2(g)
(B) Na2SO2(aq.) + H2O2(aq.) ® Na2SO2(aq.) + H2O(l)
(C) 2KI(aq.) + H2O2(aq.) ® 2KOH(aq.) + I2(s)
(D) KNO2(aq.) + H2O2(aq.) ® KNO3(aq.) + H2O(s)
8.
Which of the following oxide(s) may be oxidised further ?
(A) SO2
9.
(B) MnO2
(C) Al2O3
(D) CO2
Which of the following may be oxidised as well as reduced, due to change in oxidation number
of chlorine
(A) HCl
PHYSICAL /R # 16
(B) Cl2
(C) HClO
(D) HClO4
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Subjective :
10.
11.
Balance following half reaction in acidic medium
(i) H2S ® S
(ii) SO3–2 ® S–2
(iii) H2O2 ® O2
(iv) Cl2 ® Cl–
(v) MnO4– + H+ ® Mn2+
(vi) NH3 ® NO
(vii) C2O42– ® CO2
(viii) S2O3–2 ® S4O6–2
(ix) Cr2O72– + H+ ® Cr3+
(x) MnO4– ® MnO2
Balance the following redox reactions by oxidation number method :
(i)
N2H4(l) + ClO3– (aq.) ¾® NO(g) + Cl–(aq.) (Basic medium)
(ii)
Cl2O7(g) + H2O2(aq.) ¾® ClO2–(aq.) + O2(g) + H+ (aq.) (Acidic medium)
(iii) Cr2O72– + SO32– + H+ ¾® Cr3+ + SO42– + H2O (Acidic medium)
(iv) MnO4–(aq.) + Br–(aq.) + H2O (l) ¾® MnO2 (s) + BrO3–(aq.) + OH–(aq.) (Basic medium)
(v)
H2S(g) + Cl2(g) ¾® HCl (aq.) + S(s) (Acidic medium)
(vi) Fe3O4(s) + Al(s) ¾® Fe(s) + Al2O3(s)
(vii) I2(s) + Na2S2O3(aq.) ¾® NaI(aq.) + Na2S4O6(aq.)
12.
Balance the following redox reactions by half-reaction method (Ion electron method):
(i) Cr2O72– (aq.) + Fe2+(aq.) + H+(aq.) ® Cr3+(aq.) + Fe3+(aq.) + H2O(l)
(ii)
XeO64–(aq.) + F–(aq.) + H+ (aq.) ® XeO3(g) + F2(g) + H2O(l)
(iii) CuSO4 + KI ® Cu2I2 + K2SO4 + I2
(iv) NO3–(aq.) + Mg(s) + H2O(l) ® Mg(OH)2(s) + OH–(aq.) + NH3(g)
(v)
H3PO2(aq.) + AgNO3(aq.) + H2O(l) ® H3PO4 (aq.) + Ag(s) + HNO3(aq.)
(vi) Sn2+ + Fe3+ ® Sn4+ + Fe2+
(vii) H2SO3(aq.) + Sn4+(aq.) + H2O (l) ® Sn2+(aq.) + HSO4– + H+(aq.)
13.
H2O2 decomposed as :
2H2O2 (aq.) ® 2H2O(l) + O2(g)
If 50% of H2O2 present in 400 ml of H2O2 solution decomposed as above, the volume (in ml) of O2(g)
produced at 27ºC and 608 torr is (R = 0.08 L-atm/K-mol)
PHYSICAL /R # 16
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RACE # 17
1.
2.
3.
PHYSICA L CHEMISTRY
MAX. TIME : 60 Min.
Calculate 'n' factor of following acids (i) HCl
(ii) H3PO2
(iii) H3PO3
(iv) H3PO4
(v) HCOOH
(vi) HNO2
(vii) H4P2O7
(viii) CO2
(ix) SO3
(x) N2O5
Calculate 'n' factor of following bases (i) Mn(OH)2
(ii) Al(OH)3
(iii) NH4OH
(iv) Zn(OH)2
(v) Sr(OH)2
(vi) NH3
(vii) Na2O
(viii) MgO
(ix) K2O
(x) Al2O3
Calculating n-factor of the following as oxidising agent (i) Cr2O72–
(ii) CrO42–
(v) CH4 (In combustion reaction)
(vii) F2
(iii) H2 O2
(iv) O3
(vi) C3H8(In combustion reaction)
(viii) MnO4– (basic medium)
(ix) HNO3 (converting into N2O)
(x) Cl2O5 (converting into Cl–)
4.
Calculate n-factor of the following as reducing agent
(i) H2C2O4
(ii) Na2C2O4
(iii) H2C2O4 . KHC2O4
(iv) FeC2O4
(v) H2C2O4.2NaHC2 O4 .2H2 O
(vi) H2O2
(vii) HCl
(viii) KNO2
(ix) Na2S2O3 (in the change : S2O32– ® S4O62–)
(x) Na2S2O3 (in the change : S2O32– ® SO42–)
5.
Equivalent weight of NH3 in the change N2 ® NH3 is :
(A)
6.
17
6
17
2
(D)
17
3
(B) Mol. wt./2
(C) 2 x Mol. wt.
(D) Mol. wt./6
In the reaction, VO + Fe2O3 ® FeO + V2O5 , the eq. wt. of V2O5 is equal to its :
(A) Mol. wt.
8.
(C)
In the reaction, 2S2O32– + I2 ® S4O62– + 2I–, the eq. wt. of Na2S2O3 is equal to its :
(A) Mol. wt.
7.
(B) 17
(B) Mol. wt./8
(C) Mol .wt./6
(D) Mol. wt./2
The eq. wt. of iodine in, I2 + 2S2O32– ® 2I– + S4O62– is :
(A) Its Mol. wt.
PHYSICAL /R # 17
(B) Mol. wt./2
(C) Mol. wt./4
(D) None of these
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9.
Molecular weight of KBrO3 is M. What is its equivalent weight, if the reaction is :
BrO3– ® Br– (acidic medium)
(A) M
10.
(C) M/6
(D) 6M
In the reaction : A–n2 + xe– ® A–n1, here x will be
(A) n1 + n2
11.
(B) M/4
(B) n2 – n1
(C) n1 – n2
(D) n1 . n2
The equivalent weight of Na2S2O3 as reductant in the reaction,
Na2S2O3+H2O+Cl2 ® Na2SO4+2HCl+S is :
(A) (Mol. wt.)/1
12.
(B) (Mol. wt.)/2
(C) (Mol. wt.)/6
(D) (Mol. wt.)/8
In a reaction 4 mole of electrons are transferred to one mole of HNO3 when it acts as an oxidant. The
possible reduction product is :
(A) (1/2) mole N2
13.
(C) 1 mole of NO2
(D) 1 mole NH3
The equivalent weight of MnSO4 is half of its molecular weight when it is converted to :(A) Mn2O3
14.
(B) (1/2) mole N2O
(B) MnO2
(C) MnO4–
(D) MnO4–2
Cr2O7–2 + I– + H+ ® Cr+3 + I2 + H2O
The equivalent weight of the reductant in the above equation is :– (At. wt. of Cr=52, I=127)
(A) 26
PHYSICAL /R # 17
(B) 127
(C) 63.5
(D) 10.4
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RACE # 18
PHYSICA L CHEMISTRY
MAX. TIME : 60 Min.
Single correct :
1.
How many mole of FeSO4, H2C2O4 and FeC2O4 are oxidised separately by one mole of KMnO4 in acidic
medium respectively :-
2.
(A) 5 ; 5/2 ; 5/3
(B) 2/5 ; 2 ; 5
(C) 5/3 ; 3/5 ; 2/5
(D) 3/5 ; 2 ; 5
Which of the following reagent can act as reducing agent with SO2 :(A) Cl2
(B) KMnO4
(C) HNO3
(D) H2S
Subjective :
3.
(i)
What is the equivalent mass of H3PO4 when neutralised to HPO42– ?
(ii)
Find no. of gram eq. of 66 gram NaIO3 when reduced to I–
(iii) Find ratio of molecular mass (M) to eq. mass (E) of H2CO3 in following neutralisation reaction.
H2CO3 + NaOH ® NaHCO3 + H2O
(iv) 5 gram eq. of KMnO4 reduced in acidic medium to give Mn2+. Find amount of KMnO4 taken,
4.
(v)
Find no. of gram eq. of 3 moles Na2S2O3 , oxidised into Na2S4O6
(i)
90 gram H2C2O4 dissolve into 2 litre of solution. Find Normality of solution
(ii)
How much amount of NaOH required to prepare 100 ml of 2N solution.
(iii) Determine the number of gram eq. of solute in 250 ml of 0.1N Na2CO3
(iv) Find Normality of 0.2M Cr2O72–, reduced into Cr3+
(v)
5.
49 gram H2SO4 dissolve in solution to make 10N solution. Find volume of solution.
Problem based on Acid - Base titration
(i)
25 ml of N/10 NaOH solution exactly neutralises 20 ml of a monbasic acid solution find Normality
of mono basic acid.
(ii)
How many ml of 1 M H2SO4 acid solution is required to neutralise 10 ml of 1 M NaOH
(iii) 10 ml, 10 M H2SO4 solution, mixed with 100 ml of NaOH solution. If resultant solution is neutral
then find Normality of NaOH solution.
(iv) How many moles of NaOH required to neutralise 3 moles of KHC2O4
(v)
45 gram H2C2O4 was dissolved in water and made upto 500 ml. How much volume of this solution
required to neutralise 120 ml of N/6 NaOH solution.
PHYSICAL /R # 18
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(i)
How many moles of K2Cr2O7 required to oxidise 3 moles of KHC2O4
(ii)
How many moles of I2 gas liberate when excess KI solution react with 25 ml , 2M K2Cr2O7 solution.
(iii) Number of moles of I2 required to oxidised, 100 ml of 2M Na2S2O3 into Na2S4O6.
(iv) What is volume of 0.1 M KMnO4 required to completely oxidize 0.5 litre 0.01M H2C2O4 into
CO2 in acidic medium.
(v)
In transforming 0.01 moles PbS to PbSO4, the volume of '11.35 V' H2O2 required will be
PHYSICAL /R # 18
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RACE # 19
PHYSICA L CHEMISTRY
MAX. TIME : 45 Min.
Single correct :
1.
When BrO3– ion reacts with Br– in acidic medium, Br2 is liberated. The equivalent weight of Br2 in this
reaction is :(A)
2.
5M
8
(B)
è
6
(D)
4M
6
ø
(B) (x1 – x2)
(C)
(3x1 – x2)
(D) (x1 – 3x2)
(B) Cl7+, Cl–
(C) Cl3+, Cl°
(D) Cl3+, Cl–
Equivalent weight of FeS2 in the half reaction, FeS2 ¾® Fe2O3 + SO2 is :(A) M/10
5.
3M
5
Four mole Cl2 molecules undergo a loss and gain of 6 mole of electrons to form two oxidation states
of Cl in auto redox change. What are the +ve and –ve oxidation states of Cl in the change :(A) Cl5+, Cl°
4.
(C)
N2 + 3H2 ¾® 2NH3 molecular weight of NH3 and N2 are x1 and x2 their equivalent weight are y1
and y2. Then (y1 – y2) is :2x - x
(A) æç 1 2 ö÷
3.
5M
3
(B) M/11
(C) M/6
(D) M/1
What mass of MnO2 is reduced by 35 ml of0.16 N oxalic acid (H2C2O4) in acidic solution? The skeleton
equation is :MnO2 + H+ + H2C2O4 ® CO2 + H2O + Mn2+
(A) 8.7 g
6.
(B) 15.8 g
(C) 6.32 g
(D) 31.6 g
(B) 0.8 M
(C) 0.25 M
(D) 0.16 M
20 ml of 0.8 M - H2SO4 solution is diluted to 100 ml. 25 ml of the diluted solution exactly require
30 ml NaOH solution for titration. The molarity of NaOH solution is (A)
9.
(D) 43.5 g
40 ml, 0.5 M - Na2S2O3 solution is required for complete reaction with 25 ml I2 solution. The molarity
of I2 solution is (A) 0.4M
8.
(C) 0.84 g
How many gram of KMnO4 are contained in 4 litre of 0.05 N solution. The KMnO4 is to be used as
an oxidant in acidic medium ?
(A) 1.58 g
7.
(B) 0.24 g
2
M
15
(B)
4
M
15
(C)
1
M
15
(D)
1
M
60
25 ml acidified of K2Cr2O7 solution is diluted to 200 ml. If 40 ml of the diluted solution exactly required
15 ml of 0.2 N - KI solution for titration, the normality of original K2Cr2O7 solution is (A) 0.3 N
PHYSICAL /R # 19
(B) 0.2 N
(C) 0.6 N
(D) 0.1 N
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10.
35 ml of 1.5 M – H2SO4 solution is mixed with 50 ml of 0.6 M-NaOH solution. If the resulting solution
exactly requires 75 ml of KOH solution for the neutralisation of excess acid, the molarity of KOH solution
is (A) 0.5M
11.
(B) 0.75 M
(C) 2.0 M
(D) 1.0 M
0.02 mole KMnO4 is added in 500 ml of 0.8 M - KI solution in presence of H2SO4. If the excess KI
exactly requires V ml of 0.2 M - K2Cr2O7 solution for titration, the value of 'V' is (A) 250
12.
(B) 125
(C) 375
(D) 500
12 ml KMnO4 solution is reacted with excess of KI solution in acidic medium. If the liberated I2 exactly
requires 30 ml of 0.25 N - Na2S2O3 solution for titration, the normality of KMnO4 solution is (A) 0.625 N
PHYSICAL /R # 19
(B) 1.25 N
(C) 0.125 N
(D) 0.25 N
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RACE # 20
PHYSICA L CHEMISTRY
MAX. TIME : 30 Min.
Single correct :
1.
The temperature (K) at which a pure sample of an ideal gas not only exhibit a pressure of one atm but
also has a concentration 1 mole/dm3.
(A) 12 K
2.
3.
(B) 312 K
(C) 285 K
(D) 273 K
Which one of these graphs for an ideal gas having a fixed amount the arrow indication is incorrectly
marked.
(A)
(B)
(C)
(D)
At the top of the mountain the thermometer reads 0°C and the barometer reads 710 mm Hg. At the
bottom of the mountain the temperature is 30°C and presure is 760 mm Hg. Ratio of density of air at the
top with that at the bottom is
(A) 1 : 1
4.
(B) 1.04 : 1
(C) 1 : 1.04
(D) 1 : 1.5
3gm of carbon reacts completely with 5gm of O2 leaving none of reactant. Mole fraction of CO in final
mixture is (A) 0
5.
(B) 1
(C) 0.75
(D) 0.25
At a constant temperature a gas occupies a volume of 200 ml at a pressure of 0.720 bar. It is subjected to
an external pressure of 0.900 bar. What is the resulting volume of the gas?
(A)160 ml
6.
(B) 320 ml
(C) 80 ml
(D) 400 ml
2.5 L of a sample of a gas at 27°C and 1 bar pressure is compressed to a volume of 500 ml keeping the
temperature constant, the percentage increase in pressure is
(A) 100%
7.
(B) 400%
(C) 500%
(D) 80%
An L.P.G. cylinder contains 15 kg of butane gas at 27°C and 10 atm pressure. It was leaking and its
pressure fell down to 8 atm pressure. The gas leaked is :(A) 2 kg
PHYSICAL /R # 20
(B) 1 kg
(C) 4 kg
(D) 3 kg
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8.
How much should the pressure be increased in order to decrease the volume of a gas by 5% at a constant
temperature.
(A) 5%
9.
(C) 10%
(D) 4.26%
Pressure of mixture of 4g of O2 and 2g of H2 confined in bulb of 1 lit at 0°C.
(A) 25.2 atm
10.
(B) 5.26%
(B) 31.2 atm
(C) 45.2 atm
(D) 15.2 atm
The density of a gas is 1.964 g/L at 0°C and 76 cm Hg. The gas is :(A)CH 4
PHYSICAL /R # 20
(B) C2H6
(C) CO2
(D) Xe
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RACE # 21
PHYSICA L CHEMISTRY
TIME : 30 Min.
Single correct :
1.
A gas at a pressure of 5.0 atm is heated from 0° to 546°C and simultaneously compressed to
one-third of its original volume. Hence final pressure is
(A) 10.0 atm
2.
3.
4.
(B) 30.0 atm
(C) 45.0 atm
(D) 5.0 atm
The pressure P of a gas is plotted against its absolute temperature T for two different constant volumes,
V1 and V2. (for same no. of moles) When V1 > V2, the correct statement is
(A) Curves have the same slope and do not intersect
(B) Curve must intersect at same point other than T = 0
(C) Curve for V2 has a greater slope than that for V1.
(D) Curve for V1 has a greater slope than that for V2.
P vs V curves were plotted for three different samples containing same masses of H2 ,O2 & N2 at same
temperature. Mark out which graph is applicable for which sample.
(A) 1® H2, 2® N2, 3® O2
(B) 1® O2, 2® N2, 3® H2
(C) 1® N2, 2® H2, 3® O2
(D) Data insufficient
A closed container contains N molecules at P atm and TK. If the absolute temperature is doubled,
(A) number of molecules present in the container will become 2N
(B) number of molecules present in the container will become N/2
(C) gas pressure become 2 P
(D) gas pressure become P/2
5.
The temperature of an ideal gas can be raised by
(A) decreasing the volume but keeping the quantity and pressure fixed
(B) decreasing the quantity but keeping the pressure and volume fixed
(C) decreasing the pressure but keeping the quantity and volume fixed
(D) decreasing the pressure and volume but keeping the quantity fixed
6.
7.
The molar volume of CO2 is maximum at
(A) 273K and 1 atm
(B) 546K and 1 atm
(C) 273K and 2 atm
(D) 546K and 2 atm
One litre of a certain gas weighs 1.16 gm at STP. The gas may be (A) C 2H 2
8.
(B) CO
(C) O2
(D) NH3
A vessel contains 1 mole of O2 gas at a temperature T. The pressure of the gas is P. An identical vessel
containing 1 mole of He gas at a temperature 2T has a pressure of
(A) P / 8
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(B) P
(C) 2P
(D) 8 P
PHYSICAL /R # 21
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9.
Which of the following percentage strength is not possible for a sample of oleum ?
(A) 104%
10.
(B) 109%
(C) 118%
(D) 127%
A quantity of hydrogen gas occupies a volume of 30.0 mL at a certain temperature and pressure. What
volume would half this mass of hydrogen occupy at triple the absolute temperature if the pressure were
one-ninth that of the original gas?
(A) 270 mL
E-2 /1
(B) 90 mL
(C) 405 mL
(D) 135 mL
PHYSICAL /R # 21
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RACE # 22
PHYSICA L CHEMISTRY
TIME : 30 Min.
Single correct :
1.
A certain mountain is 14,100 feet above sea-level. The pressure at the top is 17.7 inches of Hg. If you
blew up a balloon at sea level, where the pressure measured to be 29.7 inches and carried it to the top of
the mountain, by what factor would its volume change w.r.t. final volume
(A) 29.7 – 17.7
2.
3.
(B) 29.7 / 17.7
(D) 12 / 29.7
A vertical hollow cylinder height 1.52 m is fitted with a movable piston of negligible mass and thickness.
The lower half of the cylinder contains ideal gas and upper half is filled with Hg. The cylinder is initially
at 300 K. When the temperature is raised half of the mercury comes out of cylinder. The temperature is
(Assume no thermal expansion for Hg).
(A) 337.5 K
(B) 364.5 K
(C) 546 K
(D) 600 K
For a closed container containing 10 moles of an ideal gas, at constant pressure of 0.821 atm, which
graph correctly represent variation of log V v/s log T where volume is in litre & temp in kelvin
logV
logV
(A)
4.
(C) 17.7 / 29.7
45º
logT
(B)
logV
30º
logT
(C)
logT
45º
(D)
1
45º
logV
logT
In the given isobaric process shown by graph between T & V.
B
T
C
A
(0, 0)
(A) Moles decreases throughout
(C) Moles first decreases then increases
V
(B) Moles first increases then decreases
(D) Moles cannot be predicted form given data
5.
When 40 cc of hydrogen chloride gas is mixed with 20 cc of ammonia gas the final volume of gas left
at the same temperature and pressure will be
NH3(g) + HCl(g) ¾®NH4 Cl(s)
(A) 20 cc
(B) 40 cc
(C) 60 cc
(D) 100 cc
6.
In two different vessels X and Y, H2O (l) is kept at the same temperature, the vacant space left over the
(W )
surface of H O(l) is V and 3V respectively. What is the mass ratio W
( )
H2O x
2
(A) 1 : 3
PHYSICAL /R # 22
H2O
(B) 3 : 1
(C) 1 : 4
of vapours in two vessels?
y
(D) 1 : 1
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7.
The pressure of certain amount of gas becomes double when its volume is doubled. Which of the following
relation between initial temperature (T1 K) and final temperature (T2K) of gas is correct (A) T2 = T1
8.
(B) T2 = 2T1
(C) T2 = 4T1
(D) T2 = 8T1
0.05 moles of an ideal gas is collected over water at 27ºC and it occupied 1200 ml. The pressure exerted
on the walls of vessel is (Vapour pressure of water at 27ºC = 0.04 atm, R = 0.08 L-atm/K-mol)
(A) 1.0 atm
9.
(B) 1.04 atm
(C) 0.96 atm
(D) 0.04 atm
At constant pressure, what should be the percentage decrease in the density of an ideal gas for a 10%
increase in the absolute temperature?
(A) 10%
(B) 9.1%
(C) 11%
(D) 12.09%
Comprehension
10.
Two liters Duma’s bulb contains nitrogen gas at 0.5 atm. On adding 0.01 mole of O2 gas it is necessary
to cool bulb to a temperature 10°C to maintain the same pressure.
(i)
The total no. of moles of N2 in Duma’s bulb is
(A) 0.033
(ii)
(B) 0.066
(C) 3.34
(D) 0.334
(C) 555.12 K
(D) 273.0 K
The initial temperature of the Duma’s bulb is
(A) 95.6 K
PHYSICAL /R # 22
(B) 368.6 K
H-2 /1
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+ Advanced)
2022
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RACE # 23
PHYSICA L CHEMISTRY
TIME : 30 Min.
ONLY ONE OPTION IS CORRECT :
1.
Two container each containing liquid water are connected as shown in diagram.
Given that vapour pressure of H2O(l) at 300 K & 350 K are 22 mm of Hg and 40 mm of Hg. The final
pressure in each container if valve is opened while keeping the containers at the given temperature is
(A) 22 mm of Hg
2.
3.
(B) 40 mm of Hg
(C) 31 mm of Hg
(D) 62 mm of Hg
A vessel contains equal masses of three gases A,B,C and recorded a pressure of 3.5 bar at 25°C. The
molecular mass of C is twice that of B and molecular mass of A is half of B. Find the partial pressure
of B (in bar) in the vessel
(A) 3
(B) 2
(C) 4
(D) 1
Pressure versus temperature graph of an ideal gas of equal number of moles of different volumes is
plotted as shown in figure. Choose the correct alternatives P
4
2
3
1
(A) V1 = V2 , V3 = V4 and V2 > V3
(C) V1 = V2 = V3 = V4
MORE THAN ONE MAY BE CORRECT :
4.
6.
(B) V1 = V2 , V3 = V4 and V2 < V3
(D) V4 > V3 > V2 > V1
2 gm H2 diffuses in 10 min, then how long will 8gm O2 diffuse under same conditions (A) 5 min
5.
T
(B) 10 min
(C) 2 min
(D) 20 min
Choose the correct statement(s) among the following
(A) Average molecular speed of gases increases with decrease in fraction of molecules moving slowly
(B) Rate of diffusion of gases increases with increase in collision frequency at constant volume.
(C) Rate of diffusion is inversily proportional to molecular weight of gas
(D) Mean free path does not change with change in temperature at constant pressure.
Three closed vessels A, B and C are at the same temperature T and contain gases which obey the
Maxwellian distribution of velocities. Vessel A contains only O2, B only N2 and C a mixture of equal
quantities of O2 and N2. If the average speed of the O2 molecules in vessel A is V1, that of the N2
molecules in vessel B is V2, the average speed of the O2 molecules in vessel C is (A)
(V1 + V2 )
2
PHYSICAL /R # 23
(B) V1
(C) (V1 V2)1/2
(D)
3kT / M
E-1 /2
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7.
8.
9.
10.
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Rate of diffusion of a gas is :
(A) directly proportional to its density
(B) directly proportional to its molecular weight
(C) directly proportional to the square of its molecular weight
(D) inversely proportional to the square root of its molecular weight
The ratio of root mean square speed of H2 at 50 K and that of O2 at 800K is (A) 4
(B) 2
(C) 1
(D) 1/4
The average speed of an ideal gas molecule at 27ºC is 0.3 m/s. The average speed at 927ºC will be (A) 0.6 m/s
(B) 0.3 m/s
(C) 0.9 m/s
(D) 3.0 m/s
Two gases X and Y have their molecular speed in ratio of 3 : 1 at certain temperature. The ratio of their
molecular masses Mx : My is (A) 1 : 3
(B) 3 : 1
(C) 1 : 9
(D) 9 : 1
PHYSICAL /R # 23
E-2 /2
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RACE # 24
PHYSICA L CHEMISTRY
TIME : 30 Min.
Only one option is correct :
Q.1 Suppose that we change URMS of gas in a closed container from 5 × 10–2 cm/sec to 10 × 10–2 cm/sec,
which one of the following might correctly explain how this change was accomplished
(A) By heating the gas we double the temperature
(B) By removing 75% of the gas at constant volume we decrease the pressure to one quarter of its
original value
(C) By heating the gas we quadruple the pressure
(D) By pumping in more gas at constant temperature we quadruple the pressure.
Q.2 For one mole of ideal gas if p =
P0
æVö
1+ ç ÷
è V0 ø
2
where P0 & V0 are constant then temperature of gas when
V = V0 is(A)
P0V0
R
(B)
P0V0
4R
Q.3 urms =
xp
, here , x will be d
(A) 1
(B) 2
(C)
P0V0
2R
(D)
(C) 3
P0V0
3R
(D) 4
Q.4 Which graph represent the correct -relationship between various velocities for ideal gas uavg
urms
uavg
(A) dN
(B) dN
Ndu ump
urms
ump
Ndu
u
u
(C) dN
ump
urms
uavg
(D) dN
ump
uavg
urms
Ndu
Ndu
u
u
Q.5 Statement-1: The total kinetic energy of vapours formed over liquid H2O(l) in two closedcontainer A
& B having free space 1 litre & 2 litre respectively over H2O (l) at the same temperature is in the ratio
1 : 2.(Assuming ideal gas behaviour of vapours.)
Statement-2: Vapour pressure of a substance depends only on temperature.
(A) Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
(B) Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1.
(C) Statement-1 is true, statement-2 is false.
(D) Statement-1 is false, statement-2 is true.
E-1 /2
PHYSICAL /R # 24
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Q.6
At what temperature will most probable speed of the molecules of the second member of homologous
series CnH2n–2 be the same as that of oxygen at 527°C.
Q.7
Q.8
(A) 1000°C
(B) 727°C
(C) 1727°C
(D) 1044.5°C
Which pair of the gaseous species diffuse through a small jet with the same rate of diffusion at same
P and T :
(A) NO, CO (B) NO, CO2
(C) NH3,PH3
(D) NO, C2H6
The rate of diffusion of methane at a given temperature is twice that of a gas X. The molecular weight
of X is :
(A) 64
(B) 32
(C) 4.0
(D) 8.0
Q.9 The densities of two gases are in the ratio of 1 : 16. The ratio of their rates of diffusion is :
(A) 16 : 1
(B) 4 : 1
(C) 1 : 4
(D) 1 : 16
More than one correct:
Q.10 500 ml, 1M NaCl(aq.) solution is mixed with 1000ml, 1M AgNO3(aq.) solution. Which of the following
option is/are correct for resultant solution 1
+
(A) [Na ] = M
3
E-2 /2
+
(B) [Ag ] =
2
M
3
2
(C) [NO3 ] = M
3
1
1
(D) [Cl] = M
3
PHYSICAL /R # 24
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RACE # 25
PHYSICA L CHEMISTRY
TIME : 30 Min.
Single Correct
Q.1 Choose the correct alternative (more than one may be correct) (B.M.C.= Bimolecular collision)
(at constant P) (n- is constant throughout)
(A) l is constant
(B) BMC made by 1 molecule per second is directly proportional to T.
(C) BMC for all the molecules per unit volume is directly proportional to T2.
(D) None of these
Q.2 The value of ‘a’ for NH3 is greater than that of N2.
(A) NH3 has greater size
(B) NH3 has greater attractions
(C) NH3 has smaller size
(D) NH3 has smaller attractions
Q.3 When the temperature of a sample of H2S gas is lowered the pressure decreases more than predicted by
the ideal gas equation. To what is the deviation mostly attributed to
(I) attractive forces
(II) volume of the molecule
(A) only (I)
(B) only (II)
(C) either (I) or (II) anything
(D) both (I) & (II)
Q.4. If X is the total number of collisions which a gas molecule registers with other molecules per unit time
under particular conditions, then the collision frequency of the gas containing N molecules per unit volume
is (A) X/N
(B) NX
(C) 2NX
(D) NX/2
Q.5 At moderate pressure, the compressibility factor for a gas is given as: Z = 1 + 0.35P -
168
.P, where
T
P is in bar and T is in Kelvin. What is the Boyle's temperature of the gas?
(A) 168K
(B) 480K
(C) 58.8K
(D) 575K
Q.6. Consider an ideal gas contained in a vessel. If the intermolecular interactions suddenly begin to act,
which of the following happen?
(A) the pressure decrease
(B) the pressure increase
(C) the pressure remains unchanged
(D) the gas collapse
Q.7. A real gas obeying Vander waal's equation will resemble ideal gas if the constants
(A) a and b are small
(B) a is large and b is small
(C) a is small and b is large
(D) a and b are large
Q.8. The Vander waal's equation for (½) mole of a gas
a ö
æ
(A) ç P+ 2 ÷ (V - b)= RT
è V ø
a öæ
b ö RT
æ
(B) ç P+ 2 ÷ç V - ÷ =
2ø
2
è 4V øè
a öæ V - b ö
æ
(C) ç P+ 2 ÷ç
÷ = RT
è 4V øè 2 ø
a öæ V - b ö
æ
(D) ç P+ 2 ÷ç
÷ = 2RT
è 4V øè 2 ø
H-1 /2
PHYSICAL /R # 25
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Q.9. The behaviour of temporary like carbon dioxide approaches that of parmanent gases, such as nitrogen,
oxygen etc. , as we go
(A) below critical temeprature
(B) above critical temeprature
(C) above absolute zero
(D) below absolute zero
Subjective :
Q.10. Two bulbs A and B of equal capacity are filled with He and SO2 respectively at same temperature.
(i) How will the URMS be affected if volume of B becomes 4 times that of A at constant temperature.
(ii) How will the URMS be affected if half of the molecules of SO2 are removed at constant temperature.
H-2 /2
PHYSICAL /R # 25
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RACE # 26
PHYSICA L CHEMISTRY
TIME : 30 Min.
X+, Y2+ and Z– are isoelectronic with CO2. Increasing order of protons in X+, Y2+ and Z– is :
1.
(A) X+ = Y2+ = Z–
2.
(B) X+ < Y2+ < Z–
(C) Z– < X+ < Y2+
(D) Y2+ < X+ < Z–
The frequency of light for 1.0 Å wavelength is:-
3.
(A) 3 × 1018 Hz
(B) 3 × 1018 sec–1
(C) 3 × 1018 Cycles per sec
(D) All of the above
The number of photons emitted in 10 hours by a 60 W sodium lamp (l of photon = 6000 Å)
(A) 6.50 × 1024
(B) 6.40 × 1023
(C) 8.40 × 1023
(D) 3.40 × 1023
The specific charge of a proton is 9.6 × 107C kg–1, then for an a-particle it will be -
4.
(A)2.4 × 107C kg–1
5.
(B) 4.8 × 107C kg–1
(C) 19.2 × 107C kg–1 (D) 38.4 × 107C kg–1
It is known that an atom contains protons, neutrons and almost electrons. If the mass of neutron is assumed
to half of its original value where as that of proton is assumed to be twice of its original value then the
atomic mass of 7N14 will be :(A) same
(B) 25 % more
(C) 14.28 % more
(D) 28.5 % less
A dye absorbs a photon of wavelength l and re-emits the same energy into two photons of wavelengths
6.
l1 and l2 respectively. The wavelength l is related with l1 and l2 as :l +l
1
2
(A) l = l l
1 2
7.
ll
1 2
(B) l = l + l
1
2
l2l2
1 2
(C) l = l + l
1
2
ll
1 2
(D) l = (l + l )2
1
2
The number of photons of light having wave number 'x' in 10 J of energy source is :(A) 10hcx
8.
(B)
hc
10x
The energy of a 700-nm photon is :(A) 1.77 eV
(B) 2.47 eV
9.
The
(C)
10
hcx
(C) 700 eV
(D) None of these
(D) 3.57 eV
e
ratio for cathode rays :m
(A) is constant
(B) varies with Z of element forming cathode in discharge tube
(C) varies as Z of the gas in discharge tube varies
(D) has smallest value when discharge tube is filled with H2
10.
The energy required to break one mole of Cl–Cl bonds in Cl2 is 242 kJ mol–1. The longest wavelength
of light capable of breaking a single Cl–Cl bond is
(C = 3 × 108 ms–1 and NA = 6.02 × 1023 mol–1 )
(A) 494 nm
H-1 /2
(B) 594 nm
(C) 640 nm
(D) 700 nm
PHYSICAL /R # 26
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RACE # 27
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
The radius of which of the following orbit is same as that of the first Bohr’s orbit of hydrogen atom.
(A) He+ (n = 2)
(B) Li2+ (n = 2)
(C) Li2+ (n = 3)
(D) Be3+ (n = 2)
2.
If the velocity of an electron in Ist orbit of H is V, then what will be the velocity in 4th orbit of
Be+3 :(A) V
3.
4.
5.
6.
(B)
V
4
(C) 16 V
(D) 4 V
The wavelength of the radiation emitted when an electron falls from Bohr's orbit 4 to 2 in H atom is
(A) 972 nm
(B) 486 nm
(C) 243 nm
(D) 182 nm
In hydrogen atom the energy difference between the states n = 2 and n = 3 is E eV . The ionisation
potential of H atom is (A) 3.2 E
(B) 5.6 E
(C) 7.2 E
(D) 13.2 E
Which of the following statement (regarding an atom of H) is correct (A) Kinetic energy of the electron is maximum in the first orbit
(B) Potential energy of the electron is maximum in the first orbit
(C) Radius of the second orbit is two times the radius of the first orbit
(D) Various energy levels are equally spaced
An electron in an atom jumps in such a way that its kinetic energy changes from x to
x
. The change in
4
potential energy will be :(A) +
7.
8.
3
x
2
3
4
(C) + x
3
4
(D) – x
(A) Velocity of electron µ
1
r
(B) Frequency of revolution µ
(C) Velocity of electron µ
r
(D) mvr µ n
1
n3
In which transition minimum energy is emitted
(B) 2 ® 1
(C) 3 ® 2
(D) n ® (n – 1) [n ³ 4]
The ratio of the energy of the electron in ground state of hydrogen to the electron in first excited state
of Be3+ is :(A) 1 : 4
10.
3
x
8
Choose the wrong one on the basis of Bohr's theory:-
(A) ¥ ® 1
9.
(B) –
(B) 1 : 8
(C) 1 : 16
(D) 16 : 1
The I.P. of an atom is 16eV. What is the value of first excitation potential :–
(A) 10·2 eV
PHYSICAL /R # 27
(B) 12 eV
(C) 14 eV
(D) 16 eV
E-1 /1
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RACE # 28
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
An atom has a mass of 0.02 kg and uncertainty in its velocity is 9.218 × 10–6 m/s then uncertainty in
position is (h = 6.626 × 10–34 Js)
(A) 2.86× 10–28 m
(B) 2.86 × 10–32 cm
(C) 1.5 × 10–27 m
(D) 3.9 × 10–10 m
2.
Energy of H- atom in the ground state is –13.6 eV, Hence energy in the second excited state is(A) –6.8 eV
(B) –3.4 eV
(C) –1.51 eV
(D) –4.3 eV
Uncertainty in position of a particle of 25 g in space is 10–5 m. Hence uncertainty in velocity
(ms–1) is (Planck's constant h = 6.6 × 10–34 Js)
(A) 2.1 × 10–28
(B) 2.1 × 10–34
(C) 0.5 × 10–34
(D) 5.0 × 20–24
3.
h
4.
The orbital angular momentum for an electron revolving in an orbit is given by l(l + 1) . . This
2p
momentum for an s-electron will be given by
(A) 2.
5.
h
2p
(B) +
1 h
.
2 2p
(C) zero
(D)
h
2p
The number of d-electrons retained in Fe2+ (At. no. of Fe = 26) ion is :
(A) 6
(B) 3
(C) 4
(D) 5
The de Broglie wavelength of a tennis ball of mass 60 g moving with a velocity of 10 metres per second
is approximately :
6.
(A) 10–25 metres
7.
(B) 10–33 metres
(C) 10–31 metres
(D) 10–16 metres
In Balmer series of lines of hydrogen spectrum, the third line from the red end corresponds to which one
of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen ?
(A) 2 ® 5
(B) 3 ® 2
(C) 5 ® 2
(D) 4 ® 1
Which of the following sets of quantum number is correct for an electron in 4f orbital ?
8.
9.
10.
(A) n = 3, l = 2, m = – 2, s = +
1
2
(B) n = 4, l = 4, m = – 4, s = –
1
2
(C) n = 4, l = 3, m = + 1, s = +
1
2
(D) n = 4, l = 3, m = + 4, s = +
1
2
The wavelength of the radiation emitted, when in a hydrogen atom electron falls from infinity to stationary
state 1, would be
(Rydberg constant = 1.097× 107 m–1) :
(A) 9.1 × 10–8 nm
(B) 192 nm
(C) 406 nm
(D) 91 nm
Which of the following statements in relation to the hydrogen atom is correct ?
(A) 3s, 3p and 3d orbitals all have the same energy
(B) 3s and 3p orbitals are of lower energy than 3d orbitals
(C) 3p orbital is lower in energy than 3d orbital
(D) 3s orbitals is lower in energy than 3p orbital
E-1 /2
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RACE # 29
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
According to Bohr's theory angular momentum of electron in 5th shell is :(A) 1.0 h/p
(B) 10 h/p
(C) 2.5 h/p
(D) 25 h/p
2.
Uncertainty in the position of an electron (mass = 9.1 × 10 –31 Kg) moving with a velocity
300 ms–1, accurate upto 0.001%, will be :- (h = 6.63 × 10–34 Js)
(A) 5.76 × 10–2 m
(B) 1.92 × 10–2 m
(C) 3.84 × 10–2 m
(D) 19.2 × 10–2 m
3.
The ionziation enthalpy of hydrogen atom is 1.312 x 106 J mol–1. The energy required to excite the
electron in the atom from n =1 to n =2 is
(A) 8.51 x 105 J mol–1 (B) 6.56 x 105 J mol–1
4.
(C) 7.56 x 105 J mol–1 (D) 9.84 x 105 J mol–1
In an atom, an electron is moving with a speed of 600 m/s with an accuracy of 0.005%. Certainity with
which the position of the electron can be located is (h = 6.6 × 10 –34 kg m2 s –1 , mass of electron,
em = 9.1 × 10–31 kg):(A) 1.92 × 10–3 m
5.
(B) 3.84 × 10–3 m
(C) 1.52 × 10–4 m
(D) 5.10 × 10–3 m
Calculate the wavelength (in nanometer) associated with a proton moving at 1.0 × 103 ms–1 (Mass of proton
= 1.67 × 10–27 kg and h = 6.63 × 10–34 Js) :(A) 2.5 nm
(B) 14.0 nm
(C) 0.032 nm
(D) 0.40 nm
The angular momentum J of the electron in a hydrogen atom is proportional to nth power of r (radius
of the orbit) where n is:-
6.
(A) 1
(B) –1
(C)
1
2
(D) None
Ionisation energy of He+ is 19.6 × 10–18 J atom–1. The energy of the first stationary state (n = 1) of Li2+ is:(A) 8.82 × 10–17 J atom–1
(B) 4.41 × 10–16 J atom–1
7.
(C) –4.41 × 10–17 J atom–1
8.
(D) –2.2 × 10–15 J atom–1
A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emissions is at 680 nm,
the other is at :-
9.
10.
(A) 743 nm
(B) 518 nm
(C) 1035 nm
(D) 325 nm
The frequency of light emitted for the transition n = 4 to n = 2 of He+ is equal to the transition in H
atom corresponding to which of the following
(A) n = 3 to n = 1
(B) n = 2 to n = 1
(C) n = 3 to n = 2
(D) n = 4 to n = 3
The electrons identified by quantum numbers n and l :(a) n = 4 , l = 1
(b) n = 4, l = 0
(c) n = 3, l = 2
(d) n = 3, l = 1
Can be placed in order of increasing energy as
(A) (a) < (c) < (b) < (d)
(B) (c) < (d) < (b) < (a)
(C) (d) < (b) < (c) < (a)
(D) (b) < (d) < (a) < (c)
E-1 /1
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RACE # 30
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
Supposing the I.P. of hydrogen atom is 960 eV. Find out the value of principal quantum number having
the energy equal to – 60 eV :–
(A) n = 2
2.
(B) n = 3
(C) n = 4
(D) n = 5
The radiation of low frequency will be emitted in which transition of hydrogen atom :–
(A) n = 1 to n = 4
(B) n = 2 to n = 5
(C) n = 3 to n = 1
(D) n = 5 to n = 2
3.
The ionisation potential of a singly ionised helium ion is equivalent to :(A) Kinetic Energy of first orbit
(B) Energy of last orbit
(C) Average energy in orbits
(D) Maximum energy in orbits
4.
The ratio of the difference in energy between the first and second Bohr orbit to that between second
and third Bohr orbit in H-atom is :(A) 4/9
(B) 1/3
(C) 27/5
(D) 1/2
5.
The ratio of potential energy and total energy of an electron in a Bohr orbit of hydrogen like species is:(A) 2
(B) –2
(C) 1
(D) –1
st
nd
rd
Which is not a correct order of energy for 1 , 2 & 3 orbit :(A) E1 > E2 > E3
(B) (PE)1 < (PE)2 < (PE)3
(C) (KE)1 > (KE)2 > (KE)3
(D) '1' & '3' both
6.
7.
For any H like system, the ratio of velocities of I, II & III orbit i.e. V1 : V2 : V3 will be
(A) 1 : 2 : 3
(B) 1 : 1/2 : 1/3
(C) 3 : 2 : 1
(D) 1 : 1 : 1
Match the following :(A) Energy of ground
(i) +6.04 eV
+
state of He
(B) Potential energy of I
(ii) –27.2 eV
orbit of H–atom
(C) Kinetic energy of II
(iii) 8.72 ×10–18J
excited state of He+
(D) Ionisation potential
(iv) –54.4 eV
+
of He
(A) A – (i), B – (ii), C – (iii), D – (iv)
(B) A – (iv), B – (iii), C – (ii), D – (i)
(C) A – (iv), B – (ii), C – (i), D – (iii)
(D) A – (ii), B – (iii), C – (i), D – (iv)
Which transition emits photon of maximum frequency :–
(A) second spectral line of Balmer series
(B) second spectral line of Paschen series
(C) fifth spectral line of Humphery series
(D) first spectral line of Lymen series
8.
9.
10.
In an electronic transition H-atom cannot emit :(A) Visible light
(B) g - rays
(C) Infra red light
E-3 /15
(D) Ultra violet light
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RACE # 31
NURTURE COURSE
PHYSICA L CHEMISTRY
TIME : 30 Min.
Single correct
Q.1
A photon of energy hv is absorbed by a free electron of a metal having work - function f < hv . Choose
the correct option(s).
(A) The electron is sure to come out.
(B) The electron is sure to come out with a kinetic energy hn – f
(C) Either the electron does not come out or it comes out with a kinetic energy hn – f
Q.2
(D) It may come out with a kinetic energy less than and equal to hn – f
Photoelectric emission is observed from a surface for frequencies n1 and n2 of the incident radiation
(n1 > n2). If the maximum K.E. of the photoelectrons in two cases are in ratio 1 : K, then the threshold
frequency n0 is given by
n 2 - n1
Kn1 - n 2
Kn 2 - n1
n -n
(B)
(C)
(D) 2 1
K -1
K -1
K -1
K
Minimum accelerating potential (volts) needed to accelerate an electron to produce a yellow line
(l = 310 nm ) in the spectrum , in an electron tube containing some vapours is
(A) 1.2
(B) 4
(C) 6.4 × 10–19
(D) 2 × 10–15
Which of the following statement is wrong for H-like atom (A) Magnitude of energy of an orbit in H-like species is directly proportional to 1/n2
(B) Frequency of revolution of an electron in an orbit is proportional to n3
(C) Radius of a Bohr orbit is proportional to n2
(D) Time period of revolution of an electron is proportional to n3
a -particles are projected towards the nucleus of following metals, with the same kinetic energy.
Towards which metal, the distance of closest approach will be minimum?
(A) Cu (Z = 29)
(B) Ag (Z = 47)
(C) Au (Z = 79)
(D) Ca (Z = 20)
A proton and a deuteron are projected towards the stationary gold nucleus, in different experiments,
with the same speed. The distance of closest approach will be
(A)
Q.3
Q.4
Q.5
Q.6
(A) same
Q.7
(B) greater for proton (C) greater for deuteron
(D) depends on speed
Two particles, A and B, having same e/m ratio are projected towards silver nucleus, in different
experiment, with the same speed. The distance of closest approach will be.
(A) Same for both
(B) greater for A
(C) greater for B
(D) depends on speed
Subjective
Q.8 Find the number of spectral lines in Paschen series emitted by atomic H, when electron is excited from
ground state to 7th energy level returns back.
Q.9 Calculate the minimum & maximum kinetic energy in eV of photoelectrons produced in cesium by
400 nm light. The critical (maximum) wavelength for the photoelectric effect in cesium is 660 nm,
when the potential difference is 2V.
Q.10 A radio station emits the radiations of 400 kHz. The metre band of station is -
PHYSICAL / R # 31
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RACE # 32
PHYSICA L CHEMISTRY
TIME : 30 Min.
MORE THAN ONE MAY BE CORRECT:
1.
The volume (in ml) of 0.5 M NaOH required for the complete reaction with 150 ml of 1.5M H3PO3
solutions is (A) 1350
2.
(B) 900
(D) 1150
Calculate the mass % of CaCO3 in the 103gm mixture containing CaCO3 & Na2CO3, which produces
24 litre of CO2 at 1 atm & 300 K with excess of HCl
[Given : R = 0.08 atm.lit/mol/K]
(A) 50%
3.
(C) 1250
(B) 48.5%
(C) 53%
(D) 40%
Consider the following radial distribution function diagrams. Which of the following has the correct
matching of curve and orbital ?
II
III
2
4pr (y)
2
(A) I(3s), II(3p), III(3d)
I
(B) I(3d), II(3p), III(3s)
(C) I(3p), II(3d), III(3s)
r (distance from nucleus)
(D) I(3s), II(3d), III(3p)
Let the I.E. of hydrogen like species is 320 eV. Find out the value of principal quantum number having
the energy equal to – 20 eV :–
4.
(A) n = 2
(B) n = 3
(C) n = 4
(D) n = 5
A particle moving with a velocity of 6.626 × 107 m/s has a De-Broglie wavelength of 1 Å in a circular
path of radius 0.529 Å. The angular momentum of particle is.
(h = 6.626 × 10–35 J × sec).
(A) 3.5 × 10–35 kg m2sec–1
(B) 3.5 × 10–33 kg m2sec–1
(C) 3.5 × 10–31 kg m2sec–1
(D) 1.053 × 10–35 kg m2sec–1
More than one may be correct:
5.
6.
As an electron jumps from 4th orbit to the 2nd orbit in Be3+ ion, its
(A) K.E. increases
(B)
speed increases
(C) frequency of revolution increases
(D)
P.E. decreases
V
B
A
7.
C
T
With reference to above graph, which of the following is/are incorrect.
(A) PA = PB = PC
(B) Pressure first increases then decreases
(C) PC > PA
(D) PB < PA
E-1 /2
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8.
Which of following has correct matching of curve and orbital
2
4pr Ry
2
2
2
4pr Ry
2
4pr Ry
r
9.
III
II
2
I
r
r
(A) I(2p)
II(1s)
III(4p)
(B) I(3p)
II(3d)
III(3s)
(C) I(4d)
II(2p)
III(5d)
(D) I(2s)
II(4f)
III(3d)
The orbital angular momentum of an electron is
3
h
. Which of the following may be the permissible
p
value of angular momentum of this electron revolving in unknown Bohr orbit?
(A)
10.
h
p
(B)
h
2p
(C)
3h
2p
(D)
2h
p
PCl5(g) decomposes according to following reaction,
PCl5(g) ¾¾
® PCl3(g) + Cl2(g)
Calculate density (in gm / l) of mixture at 24 atm & 300 K, when PCl5(g) undergo 50% decomposition.
[R = 0.08 atm l mol–1 K–1]
E-2 /2
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RACE # 33
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
48 g of SO3, 12.8 g of SO2 and 9.6 g of O2 are present in one litre. The respective active masses will be
(A) 1.0, 0.5 and 0.3
(B) 0.6, 0.2 and 0.3
(C) 0.6, 0.4 and 0.2
(4) 1.0, 0.5 and 1.5
2.
If the forward rate constant of reversible reaction is 0.16 and backward rate constant is 4 × 104, then the
equilibrium constant will be.
(A) 2.25 × 10–6
(B) 2.5 × 10–5
(C) 4 × 10–6
(4) 4 × 10–5
3.
Kp value for
C2H4 + H2ƒ C2H6 is 5×1018 atm–1 and Kp for
C2H2 + H2 ƒ C2H4 is 5 × 1026 atm–1 at 50°C.
Calculate Kp for the reaction
2H2 + C2H2 ƒ C2H6
(A) 2.5 × 1045
(B) 21 × 108
(C) 1.5 × 10–45
(4) 2.5 × 10–45
4.
Given that the equilibrium constant for the reaction
ˆˆˆ
†
2SO2(g) + O2(g) ‡ˆˆ
ˆ 2SO3(g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following
reaction at the same temperature ?
1
ˆˆˆ
†
SO3(g) ‡ˆˆ
O
ˆ SO2(g) +
2 2(g)
(A) 6.0 × 10–2
5.
(B) 1.3 × 10–5
(C) 1.8 × 10–3
(4) 3.6 × 10–3
For a given exothermic reaction, Kp and K¢P are the equilibrium constants at temperatures T1 and T2,
respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is
readily observed that (T2 > T1) :(A) Kp > K¢P
6.
For a reaction
(B) Kp < K¢P
(C) Kp = K¢P
(4) Kp =
(C) K
(4) 2K
1
K ¢P
1
1
H2 +
I ƒ HI ;
2
2 2
Equilibrium constant is K.
Then what will be equilibrium constant for
2HI ƒ H2 + I2
will be :(A)
E-1 /15
1
K2
(B)
1
K
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7.
If the equilibrium constant for
1
1
ˆˆˆ
†
ˆˆˆ
†
N2(g) + O2(g) ‡ˆˆ
ˆ 2NO(g) is K, the equilibrium constant for N2(g) + O2(g) ‡ˆˆ
ˆ NO(g) will
2
2
be:(A) K
8.
(B) K2
(C) K1/2
(4)
1
K
2
If the value of an equilibrium constant for a particular reaction is 1.6 × 1012, then at equilibrium the system
will contain :(A) mostly reactants
(B) mostly products
(C) similar amounts of reactants and products (4) only reactants
For a reaction A(g) ƒ B(g) if initial pressure at 300°C is 1 atm and its KP is 4, Then calculate PB at
9.
equilibrium state.
(A)
10.
1
atm
5
(B)
2
atm
5
(C)
4
atm
5
(4)
3
atm
5
In a container 96g O2 and 335g Ne are present. If total pressure of gaseous mixture is 25 atm. Then
what will be partial pressure of Ne?
(A) 21.20 atm
E-2 /15
(B) 15.7 atm
(C) 42.6 atm
(4) 3.56 atm
PHYSICAL /R # 33
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RACE # 34
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
In a chemical equilibrium, the rate constant for the backward reaction is 7.5 × 10–4 and the equilibrium
constant is 1.5. The rate constant for the forward reaction is:(A) 2 × 10–3
(B) 5 × 10–4
(C) 1.12 × 10–3
(D) 9.0 × 10–4
2.
At 1000 K, the value of KP for the reaction :
ˆˆˆ†
A(g) + 2B(g) ‡ˆˆ
ˆ 3C(g) + D(g)
is 0.05 atm The value of KC in terms of R would be
(A) 20000 R
(B) 0.02 R
(C) 5 × 10–5 R
3.
(D) 5 × 10–5 × R–1
KP
Match List –I (hypothetical reactions) with List–II (ratio K for the given reactions) and select the correrct
C
answer using the code given below the lists :ˆˆˆ†
‡ˆˆ
ˆ
(a) A2(g) + 3B2(g)
ˆˆˆ†
‡ˆˆ
ˆ
(b) A2(g) + B2(g)
2AB3(g)
2AB(g)
ˆˆˆ†
‡ˆˆ
ˆ
(c) A(s) + 1.5 B2(g)
(i) (RT)–2
(ii) (RT)0
1
AB3(g)
(d) AB2(g)
ˆˆˆ†
‡ˆˆ
ˆ
AB(g) + 0.5 B2(g)
CODES :
a
(A) (i)
(B) (ii)
(C) (i)
(D) (i)
b
(ii)
(i)
(iv)
(ii)
c
(iii)
(iv)
(iii)
(iv)
(iii) (RT) 2
1
(iv) (RT) – 2
d
(iv)
(iii)
(ii)
(iii)
4.
ˆˆˆ†
For the reaction C(s) + CO2(g) ‡ˆˆ
ˆ 2CO(g) the partial pressure of CO and CO2 are 2.0 and 4.0 atm.
respectively at equilibrium. The KP for the reaction is
(A) 0.5
(B) 4.0
(C) 8.0
(D) 1
5.
For which reaction at 298 K, the value of K is maximum and minimum respectively:c
Kp
(a) N2O4(g)
ˆˆˆ†
‡ˆˆ
ˆ
2NO2(g)
(b) 2SO2(g) + O2(g)
(c) X(g) + Y(g)
ˆˆˆ†
‡ˆˆ
ˆ
(d) A(g) + 3B(g)
(A) d, c
E-1 /2
ˆˆˆ†
‡ˆˆ
ˆ 2SO
3(g)
4Z(g)
ˆˆˆ†
‡ˆˆ
ˆ
7C(g)
(B) d, b
(C) c, b
(D) d, a
PHYSICAL /R # 34
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6.
For the reactions :- A
B
ˆˆˆ†
‡ˆˆ
ˆ
C ; KC = 4, C
ˆˆˆ†
‡ˆˆ
ˆ
B ; KC = 2,
ˆˆˆ†
‡ˆˆ
ˆ
D ; KC = 6
ˆˆˆ†
ˆ D :KC for the reaction A ‡ˆˆ
(A) 12
(B) 4/3
7.
(C) 24
(D) 48
The equilibrium constant for the reaction
ˆˆˆ†
ˆ 2Br at 500 K and 700 K are 1 × 10–10 and 1 × 10–5 respectively. The reaction is:Br2 ‡ˆˆ
(A) Endothermic
(B) Exothermic
(C) Fast
(D) Slow
8.
ˆˆˆ†
ˆ PCl (g) + Cl (g) is 16. If the
The equilibrium constant (KP) for the reaction PCl 5 (g) ‡ˆˆ
3
2
volume of the container is reduced to one-half its original volume, the value of KP for the reaction at the
same temperature will be :(A) 32
(B) 64
(C) 16
(D) 4
9.
The equilbrium constant for the reaction :
4
ˆˆˆ†
N2(g) + O2(g) ‡ˆˆ
ˆ 2NO(g) at 2000 K is 4 × 10 . In presence of catalyst the equilibrium is established
ten times faster at the same temperature. What is the value of equilibrium constant in presence of catalyst
(A) 40 × 10–4
(B) 4 × 10–4
(C) 4 × 104
(D) None
10.
ˆˆ†
For the reaction : P ‡ˆ
ˆ Q + R. Initially 2 mol of P was taken. Up to equilibrium 0.5 mol of P was
dissociated. What would be the degree of dissociation :(A) 0.5
(B) 1
(C) 0.25
(D) 4.2
E-2 /2
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RACE # 35
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
ˆˆ†
PCl5 (g) ‡ˆ
ˆ PCl3 (g) + Cl2 (g)
In above reaction, at equilibrium condition mole fraction of PCl5 is 0.4 and mole fraction of
Cl2 is 0.3. Then find out mole fraction of PCl3
(A) 0.3
(B) 0.7
(C) 0.4
(D) 0.6
2.
4 mol of PCl5 are heated at constant temperature in closed container. If degree of dissociation for PCl5 is 0.5 then calculate total number of moles at equilibrium
(A) 4.5
(B) 6
(C) 3
(D) 4
3.
ˆˆ†
The dissociation of CO2 can be expressed as 2CO2 ‡ˆ
ˆ 2CO + O2. If the 2 mol of CO2 is taken
initially and 38% of the CO2 is dissociatated completely. What is the total number of moles at
equilibrium:(A) 2.38
(B) 2.0
(C) 2.76
(D) 1.24
4.
ˆˆ†
Evaluate KP for the reaction : H2 + I2 ‡ˆ
ˆ 2HI. If 2 moles each of H2 and I2 are taken initially.
The equilibrium moles of HI are 2.
(A) 2.5
(B) 4
(C) 0.25
(D) 1.0
5.
ˆˆ†
AB dissociates as 2AB (g) ‡ˆ
ˆ 2A (g) + B2 (g)
When the initial pressure of AB is 500 mm, the total pressure becomes 625 mm when the
equilibrium is attained. Calculate KP for the reaction assuming volume remains constant.
(A) 500
(B) 125
(C) 750
(D) 375
6.
Match list –I (equilibrium) with List –II (conditions for reaction) and select the correct answer using the codes given below the lists :List–I
(Equilibrium)
List–II
(Conditions)
P.
ˆˆ†
A2(g) + B2(g) ‡ˆ
ˆ 2AB(g)
Endothermic
1.
High
temperature
Q.
ˆˆ†
2AB2(g)+B2(g) ‡ˆ
ˆ 2AB3(g)
Exothermic
2.
Low
temperature
R.
ˆˆ†
2AB3(g) ‡ˆ
ˆ A2(g) + 3B2(g)
Endothermic
3.
4.
5.
High pressure
Low pressure
Independent
of pressure
CODE :
P
(A) 1 & 3
(B) 2 &3
(C) 1 & 5
(D) 2 & 4
E-1 /2
Q
2&3
1&4
2&3
1&5
R
2&4
1&3
1&4
1&3
PHYSICAL /R # 35
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ˆˆ†
aA ‡ˆ
ˆ bB + cC, DH = - x kcal.
7.
If high pressure and low temperature are the favourable condition for the formation of the
product in above reaction, hence:(A) a > b + c
(B) a < b + c
(C) a = b + c
(D) None of them
The reaction in which yield of production cannot be increased by the application of high
8.
pressure is :ˆˆ†
(A) PCl3(g) + Cl2(g) ‡ˆ
ˆ PCl5(g)
ˆˆ†
(B) N2(g) + O2(g) ‡ˆ
ˆ 2NO (g)
ˆˆ†
(C) N2(g) + 3H2(g) ‡ˆ
ˆ 2NH3(g)
ˆˆ†
(D) 2SO2(g) + O2(g) ‡ˆ
ˆ 2SO3(g)
At 60° C and initial pressure of 1atm of N2O4 is 50% dissociated into NO2 then Kp is :-
9.
(A) 1.33 atm
10.
(B) 2 atm
(C) 2.67 atm
(D) 3 atm
At a certain temperature and total pressure of 1 atm., equilibrium mixture contains 20% by
ˆˆ† 2A(g). The KP of reaction isvolume of A atoms A2(g) ‡ˆˆ
(A) 5 × 10–2
E-2 /2
(B) 2 × 10–3
(C) 5 × 10–3
(D) 4 × 10–4
PHYSICAL /R # 35
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RACE # 37
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
At the equilibrium of the reaction,
N2O4(g) ƒ 2NO2(g),
the observed molar mass of N2O4 is 77.70 g. The percentage dissociation of N2O4 is :(A) 28.4
(B) 46.7
(C) 22.4
(D) 18.4
2.
A ƒ 2B, K p ; C ƒ D + E, K p' . If degrees of dissociation of A and C are same and
Kp = 2Kp' , then the ratio of total presure P/P'=?
(A)
3.
4.
5.
1
2
(B)
(C)
1
4
(D) 2
When sulphur is heated at 800 K, the initial pressure of 1 atm decreases by 20% at equilibrium. Kp of the
reaction S8(g) ƒ 4S2(g) is :(A) 0.2
(B) 0.512
(C) 1.51
(D) 2
For the reaction
NH4HS(s) ƒ NH3(g) + H2S(g); Kp = 0.09.
The total pressure at equilibrium is :(A) 0.3 atm
(B) 0.09 atm
(C) 0.6 atm
(D) 0.36 atm
In the dissociation of I2(g) at 1000 K in a container of 1 litre :I2(g) ƒ 2I–(g) ; KC = 1010
Select the correct relation:(A) [I2] > [I–]
6.
1
3
(B) [I2] < [I–]
(C) [I2] = [I–]
(D) [I2] =
1 –
[I ]
2
For the dissociation reaction
N2O4(g) ƒ 2NO2(g),
the degree of dissociation (a) in terms of Kp and total equilibrium pressure P is
(A) a =
4P + K p
KP
(B) a =
Kp
4P + K P
(C) a =
Kp
4P
(D) None of these
7.
The ionisation energy of a hydrogen like atom is 14.4 eV. The amount of energy released when
electron jumps from 4th orbit to the 1st orbit in this atom, is
(A*) 13.5 eV
(B) 10.8 eV
(C) 0.9 eV
(D) 12.75 eV
8.
The orbital angular momentum of an electron is
3h
Which of the following may be the permissible
p
value of angular momentum of this electron revolving in unknown Bohr orbit?
(A)
E-1 /2
h
p
(B)
h
2p
(C)
3h
2p
(D*)
2h
p
PHYSICAL /R # 37
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At constant temprature on increasing pressure which is correct :(A) Solid ƒ Liquid more liquid formed
(B) Formation of ammonia from N2 and H2 decreases
(C) CO2(g) + C(s) ƒ 2CO(g) reaction will shifted in forward direction
*(D) Solubility of gas in liquid increases
10.
For reaction
A + 2B ƒ 2C
Initally 2 mole of A and B are taken in 10 lit flask at equilibrium 1 mole of C is formed then calculate KC
for given reaction :*(A) 6.66
(B) 3.33
(C) 2.22
(D) 1.11
E-2 /2
PHYSICAL /R # 37
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RACE # 38
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
For the reaction: I2(g) ƒ 2I(g), KC = 1.0 × 10–2 mol lit–1. What volume of the vessel should be taken
so that at equilibrium 1 mole of I2(g) and 0.5 mole of I(g) are present at equilibrium?
(A) 25 L
(B) 0.04 L
(C) 0.25 L
(D) 5 L
2.
The equilibrium constant for the mutarotation, a-D-glucose ƒ b-D-glucose is 1.8. What percent of
the a-form remains under equilibrium?
(A) 35.7
(B) 64.3
(C) 55.6
(D) 44.4
3.
If 0.3 moles of hydrogen gas and 2.0 moles of sulphur solid are heated to 87ºC in a 2.0L vessel, what
will be the partial pressure of H2S gas at equilibrium? (Given: R = 0.08 L-atm/K-mol)
H2(g) + S(s) ƒ H2S(g); KC = 0.08
(A) 0.32 atm
(B) 0.43 atm
(C) 0.62 atm
(D) 0.48 atm
4.
In the equilibrium mixture: H2(g) + I2(g) ƒ 2HI(g), the mole ratio of gases are
2 : 2 :10
,
respectively. What would be the effect on the mole ratio on adding 5 mole of He gas at constant
pressure?
(A) no change
(B) The new molar ratio becomes 1 : 1 : 5
(C) The new molar ratio becomes 2 : 2 : 5
(D) The new molar ratio becomes 2 : 2 : 5 2
The process: 2A(g) ƒ A2(g) has KP = 8 × 108 atm-1. If 'A' atoms are taken at 1atm pressure, what
should be the equilibrium pressure of 'A'?
(A) 0
(B) 2.5 × 10–5 atm
(C) 4 × 104 atm
(D) 1.25 × 10–5 atm
MORE THAN ONE CORRECT :
6.
What is/are true about equilibrium state?
(A) Catalyst has no effect on equilibrium composition.
(B) Equilibrium constant is independent of initial concentration of reaction.
(C) The reaction ceases at equilibrium.
(D) Equilibrium constant is independent of pressure.
7.
A chemical system is in equilibrium. Addition of a catalyst would result in
(A) increase in the rate of forward reaction.
(B) increase in the rate of reverse reaction.
(C) a new reaction pathway to reaction.
(D) increase the amount of heat evolved.
PARAGRAPH BASED :
0.20 moles of CO taken in a 2.463 litre flask is maintained at 750K along with a catalyst so that the
5.
ˆˆ† CH OH(g). Hydrogen is introduced until the
following reaction can take place: CO(g) + 2H2(g) ‡ˆˆ
3
total pressure of the system is 7.5 atm at equilibrium and 0.1 mole of methanol is formed.
(R = 0.0821 L-atm/K-mol).
E-1 /2
PHYSICAL /R # 38
JEE (Main + Advanced) 2022
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8.
For the reaction, KP is
(A) 0.16 atm–2
9.
(B) 6.25 atm–2
(C) 0.04 atm–2
(D) 1.56 atm–2
(C) 151.75 M–2
(D) 2428 M–2
For the reaction, KC is [Given: (2.463)2 = 6.07]
(A) 6.07 M–2
10.
(B) 607 M–2
What is the final pressure if the same amount of CO and H2 as before used, but with no catalyst so that
the reaction does not take place?
(A) 18.75 atm
E-2 /2
(B) 10.0 atm
(C) 15.0 atm
(D) 12.5 atm
PHYSICAL /R # 38
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JEE (Main + Advanced) 2022
NURTURE COURSE
Path to success KOTA (RAJASTHAN)
RACE # 39
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
4 gm H2 reacts with 9 × 1023 Cl2 molecules and forms HCl gas. If the total pressure of the system after
reaction is 700 mm. What is the partial pressure of HCl? Assume complete reaction. (NA = 6 × 1023)
(A) 200 mm
(B) 350 mm
(C) 300 mm
(D)600 mm
2.
If only one gas molecule is taken in a container, the correct relation between average speed, c, root mean
square speed, u, and most probable speed, a, becomes
(A) a < c < u
(B) a = c = u
(C) c < u < a
(D) u < c < a
3.
Number of nodal surface in 5s orbital is
(A) 5
(B) 4
(C) 3
(D) 0
4.
The ionisation energy of a hydrogen like atom is 14.4 eV. The amount of energy released when electron
jumps from 4th orbit to the 1st orbit in this atom, is
(A) 13.5 eV
(B) 10.8 eV
(C) 0.9 eV
(D) 12.75 eV
5.
Electrons are de-exciting from 5th orbit in hydrogen atoms but 1st is not available for them. The maximum number of spectral lines should be
(A) 10
(B) 6
(C) 15
(D) 3
6.
The assumptions of the kinetic theory of gases are most likely to be incorrect for gases under which of
the following conditions?
(A) High temperature and high pressure
(B) High temperature and low pressure
(C) Low temperature and low pressure
(D) Low temperature and high pressure
7.
Equivalent weight of H2SO4 in the reaction:
2KMnO4 + 3H2SO4 + 10 HCl
¾¾
® 2 MnSO4 + K2SO4 + 5Cl2 + 8H2O, is
(A) M/2
(B) M
(C) 3M/10
(D) 3M/5
0.1M-KMnO4 is used for the following titration. What volume of the solution will be required to react
with 0.158 gm of Na2S2O3?
S O 2– + MnO – + H O ¾¾
® MnO (s) + SO 2– + OH–
8.
2
9.
10.
3
4
2
2
4
(A) 80 ml
(B) 26.67 ml
(C) 13.33 ml
(D) 16 ml
When 0.03 litre of a mixture of hydrogen and oxygen was exploded, 0.003 litre of oxygen remained.
The initial mixture contains (by volume)
(A) 60% O2
(B) 40% O2
(C) 50% O2
(D) 30% O2
The minimum mass of CaCO3 required to establish the equilibrium:
CaCO3(s) ¾¾
® CaO(s) + CO2(g), KC = 0.05M
at a certain temperature in a 1.0L container is
(A) 10.0 gm
(B) 7.5 gm
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(C) 5.0 gm
(D) 20.0 gm
PHYSICAL /R # 39
TM
JEE (Main + Advanced) 2022
Path to success KOTA (RAJASTHAN)
RACE # 40
NURTURE COURSE
PHYSICA L CHEMISTRY
TIME : 30 Min.
SINGLE CORRECT :
1.
When the temperature of an ideal gas is increased at constant pressure,
(A) collision number increases
(B) collision frequency increases
(C) mean free path increases
(D) number of molecules per unit volume increases
2.
Which of the following does not change during compression of a gas at constant temperature?
(A) density of a gas
(B) molecular distance
(C) average speed of molecules
(D) number of collisions in a gas
3.
Equivalent mass of a bivalent metal is 32.7. Molecular mass of its chloride is
(A) 68.2
(B) 103.7
(C) 136.4
(D) 166.3
4.
A volume of 12.5 ml of 0.05M selenium dioxide, SeO2, reacted with exactly 25.0 ml of 0.1M-CrSO4. In
this reaction, Cr2+ is converted to Cr3+. To what oxidation state the selenium converted by the
reaction?
(A) 0
(B) +1
(C) +2
(D) +4
5.
KIO3 reacts with oxalic acid, H2C2O4, in solution to yield K2C2O4, CO2 and I2. How many grams of
oxalic acid will be required to react with one gram of KIO3? (K = 39, I = 127)
(A) 1.262 gm
(B) 1.622 gm
(C) 1.747 gm
(D) 1.022 gm
6.
If rocket were fueled with kerosene and liquid oxygen, what mass of oxygen would be required for
every litre of kerosene? Assume kerosene to have the average composition C14H30 and density,
0.792 gm/ml.
(A) 5.504 kg
(B) 2.752 kg
(C) 1.376 kg
(D) 3.475 kg
7.
How many gm of solute should be added in 100 gm water to get a solution of density 1.2 gm/ml and
strength 5% (w/v)?
(A) 5 gm
(B) 6 gm
(C) 4.07 gm
(D) 4.35 gm
8.
10 gm of acetic acid is dissolved in 100 gm of each of the following solvents. In which solvent, the
mole-fraction of solute is maximum? Assume no any dissociation or association of acetic acid in the
solvent.
(A) water
(B) Ethanol
(C) Benzene
(D) Same in all solvents
9.
50 ml of a gas mixed with 70 ml of oxygen gave after explosion 50 ml of CO2 and after absorption by
KOH, 45 ml of oxygen are left. What is the molecular formula of the gas?
(A) CH4
(B) C2H4
(C) CO
(D) C2H2
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PHYSICAL /R # 40
TM
JEE (Main + Advanced) 2022
NURTURE COURSE
Path to success KOTA (RAJASTHAN )
10.
Match the following
Column - I
(Reactions)
Column - II
(Effect on addition of water)
ˆˆ† 2B(aq) + H O(l)
(A) A(aq) ‡ˆˆ
2
(P) Moles of 'A' increases
(B)
ˆˆ† 2B(aq)
3A(aq) ‡ˆˆ
(Q) Moles of 'B' increases
(C)
ˆˆ† B(aq)
2A(aq) + H2O(l) ‡ˆˆ
(R) Molar concentration of 'A' decreases
ˆˆ† 3B(aq)
(D) 2A(aq) ‡ˆˆ
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(S) Molar concentration of 'B' decreases
PHYSICAL /R # 40