Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
TOPIC States of Matter
1. Boyle’s law represents the relation between
(a)
The number of moles of a gas and its pressure
(b)
The volume of a gas and its pressure
(c)
The volume of a gas and its temperature
(d)
The pressure of a gas and its temperature
2. The value of gas constant ‘R’ in CGS unit is
(a)
1.987
(b)
8.314
(c)
8.314  10-7 (d)
0.082
3. Which of the following is incorrect according to the kinetic molecular theory of gases ?
(a)
All the molecules are in continuous in motion
(b)
Molecule of a gas creates pressure on the walls of the container by striking with the
walls of the container.
(c)
All the molecules in each gas have same volume and weight.
(d)
All the molecules of the gas move with uniform velocity.
4. The solid substances are classified into four types on the basis of
(a)
Their physical properties
(b)
Their appearance
(c)
The types of bonds between components (d)
Their Melting points
5. The radii r + / r- for the unit cell of NaCl is
(a)
0.92
(b)
1.53
(c)
0.53
(d)
0.155
6. The co-ordinate number of Cs+ ion in CsCl is
(a)
4
(b)
6
(c)
8
(d)
2
7. If 1000 Atmospheric pressure is applied on water at 20 C, the decrease in volume observed
is by
(a)
0.4%
(b)
1.4 %
(c)
4%
(d)
40%
8. If r+ / r- ratio in CsCl unit cell is
(a)
0.53
(b)
0.92
(c)
1.55
(d)
0.55
9. The rate of diffusion of any gas is
(a)
Directly proportional to the Molecular weight of the gas
(b)
Inversely proportional to the volume of the gas
(c)
Inversely proportional to the square root of the density of the gas
(d)
Inversely proportional to the temperature of the gas.
10.A mixture contains 4 moles of N2 and 8 moles of H2. If the total pressure of the mixture is 6
atmosphere, the partial pressure of nitrogen in the mixture in the mixture would be :
(a)
2 atm.
(b)
1 atm
(c)
4 atm
(d)
6 atm
1 marks
Explain the classification of Matter.
11.State Boyle’s Law in words and symbols.
12.How the idea of absolute scale of temperature is evolved.
13.Explain the relationship between Kelvin temperature (T) and Celsius temperature
(t).
14.State Charle’s Law in words and symbols.
15.State Lussac’s Law in words and symbols.
16.Derive Simple Gas Equation.
17.Derive the formula for Gas Constant (R).
18.Calculate the value of Gas Constant (R).
19.What is STP (Standard Temperature and Pressure).
20.Define Partial Pressure of gas.
2nd & 3rd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166 (M) +91- 98250-31559, +91-98981-74762
1
Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
TOPIC States of Matter
2 marks
21.Explain Dalton’s Law of Partial Pressure.
22.Define Graham’s Law of Gaseous Diffusion.
23.Explain Graham’s Law of Gaseous Diffusion in words and symbols.
24.Derive the relationship between Volume of gas diffused (V) and Molecular Mass
(M).
25.Explain Graham’s Law of Diffusion with Experiment.
26.Explain the importance of Graham’s Law of Diffusion.
27.Define Avogadro’s Hypothesis.
28.Explain the Avogadro’s Hypothesis.
29.Explain the relationship among Mole number (n), number of particles (N), Volume
(V) at STP and gram molecular weight (M).
30.Define Kinetic Molecular Principle.
31.Give the important points of Kinetic Molecular Theory.
32.What are the Classification of Solid Substances.
33.Define Unit Cell of the Crystal Structure.
34.Explain Unit cell of NaCl
35.Explain Unit cell of CsCl
36.Explain Unit cell of Lil
37.Define the co-ordination number of positive ions.
38.How the co-ordination number can get by knowing the ratio of the radii of positive
and negative ions.
39.What is Fix Volume.
40.What is Fluidity.
41.What is Non-compressibility.
42.What is Diffusion.
43.What is Evaporation
44.What is Vapour Pressure.
36.What is Equilibrium Vapour Pressure.
37.What is Surface Tension.
38.What is Viscosity.
Important Formulae To Remember
1. Boyle’s Law :
(i)
(ii)
V
1
P
(n, T constant ) PV = K
P1V1
= P2 V2 = K
(Initial)
(Final)
(Constant temperature)
2nd & 3rd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166 (M) +91- 98250-31559, +91-98981-74762
2
Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
2. Absolute Zero Temperature :
TOPIC States of Matter
Where,
T  Kelvin temperature
T = (t C + 273) K
t  Celsius temperature
3. Charle’s law :
(i)
VT
(n, P constant).
(ii)
V1 V2
V
V

or 1  1
T1 T2
T2 T2

V
K
T
Where,
(Constant Pressure)
V  Volume
P  Pr essure
4. Gay Lussac’s Law :
(i)
PT
(n, V constant).
(ii)
P1 P2
P
T

or 1  1
T1 T2
P2 T2

P
K
T
Where,
(Constant Volume
V  Volume
T  Kelvin Temperature
5. Combined Gas Equation :
P1V1 P2V2

T1
T2
6. Simple (General) Gas Equation :
(i)
PV = KT
(ii)
PV = nRT
Where,
(iii)
K  Cons tan t
g
PV =
RT
M
n  number of Moles
g  weight of the subs tan ce
M  molecular weight
7. Standard Temperature and Pressure (STP) :
Standard temperature : T = 0 C or 273 Kelvin.
Standard pressure : P = 1 atmosphere or 760 mm.
8. Dalton’s Law of Partial Pressure :
Where,
(i)
Total pressure P = p1 + p2 + p3+…….(T constant)
p1, p 2, p , ......are the
3
partial pressure of
constituent gases.
(ii)
Partial pressure can be calculated as follows :
nRT
or P =
V
(n1 n 2  n3  ......) RT
(in same volume)
V
(a)
P=
(b)
(c)
P1V1 = P2V2 (if volume is changed)
p = x . p (x = mole fraction and P = total pressure)
Mole Fraction =
Number of individual mole
Total number of moles
2nd & 3rd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166 (M) +91- 98250-31559, +91-98981-74762
3
Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
When gas is collected over water, then
Total pressure P = p(dry gas) + p
(d)
p(dry gas) = P (e)
TOPIC States of Matter
H O
2
= Total pressure – Partial pressure of water
p
H O
2
When % of volume is given then,
Partial pressure p =
% of volume  total pressure
.
100
9. Graham’s Law of Gaseous Diffusion :
(i)
r
1
(P, T constant)
d
(ii)
r=K
Where,
1
r  diffusion rate
d
d  density of a gas
Volume of gas diffused (V )
.
Time required for doffusion (t )
(iii)
Diffusion rate (R) =
(iv)
For two different gasses diffusing under identical conditions :
r1 V1 t 2


r2 t 1 V 2
d2

d1
M2
M1
10.Number of atoms in a molecule =
Molecular weight
Atomic weight
11.Molecular weight of a gas = 2  vapour density.
Exercises:
1. The pressure and volume of a constant quantity of gas at constant temperature are 1
atmosphere and 3.15 litre respectively. If the pressure is increased to 2.50 atmosphere, what
will be its volume ?
Ans : 1.26 lit.
2. The pressure of 500 ml air at constant temperature is 760 mm. If the volume of his air is
decreased to 200 ml. What will be its pressure ?
Ans : 1900 mm
3. The volume of a sample of an unknown gas at constant pressure and 27 C is 900 ml. If
thevolume of this sample is made 500 ml, what temperature will have to be kept ?
Ans : -106.3 C
4. The volume of a sample of nitrogen gas is 320 millitre at STP. What will be its volume if the
temperature of the sample is made 66 C and pressure is made 0.825 atmosphere?
Ans :482 millilitre
5. How many moles of oxygen will be in its 10 litre volume at 27 C temperature and 750 mm
pressure? What will be its weight? (Atomic weight of oxygen = 16 gram / mol)
Ans : 12.84 g
6. In a closed vessel of 5 litre volume, 20 gram sulphur trioxide gas and 2 gram helium gas are
filled at 27 C temperature. Calculate the partial pressures of gases and the total pressure of
2nd & 3rd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166 (M) +91- 98250-31559, +91-98981-74762
4
Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
the gaseous mixture.
Ans : 3.69 atmosphere
TOPIC States of Matter
7. The diffusion rates of ozone and carbon dioxide gases in uniform experimental conditions at
normal temperature and pressure are 27 ml/second and 28 ml/ second. If the molecular
weight of carbon dioxide is 44 gram/mole, find the molecular weight of ozone.
Ans : 47.3 g/mol.
8. The times required for diffusion of 114 ml. hydrogen gas and 29.4 ml. unknown gas are
found to be same. If the density of hydrogen gas is 1.0, calculate the density of unknown
gas.
Ans : 15.04 g/ml.
9. What will be the mole number in 27 gram of hydrogen? (Molecular weight of H2 = 2 g/mole)
Ans : 13.5 mole
10. How many carbon atoms will be there in 0.0022 gram carbon dioxide ? ( Molecular weight of
carbon dioxide CO2 = 44 gram / mole).
Ans : 30.11  1019
11. The density of a gaseous hydrocarbon at constant temperature and pressure is 0.963
gram/litre. The density of oxygen at this temperature and pressure is 1.032 gram / litre.
Calculate the molecular weight of hydrocarbon. (Molecular weight of CO2 = 32 gram / mole)
Ans : 29.86 g/mol
12. The molecular weight of one oxide of nitrogen is 108 gram/mole. Find the molecular of this
oxide.
Ans : N2O5
13. The volume of a gas is 200 litre at constant temperature and 700 mm. pressure. If its
volume is made 1400 litre, what will be the pressure ?
Ans : 100 mm.
14. The volume of a gas is 350 ml. at constant pressure and 23 C. If its volume is reduced and
made 39 ml. What eill be its final temperature ?
Ans : -10 C OR 263 K
15. The pressure of a definite quantity of a gas is 760 mm. at constant volume and 25 C
temperature. At what pressure its temperature will be 100 C?
Ans : 967.5 mm.
16. The volume of one sample of oxygen is 35 ml. at 6 C temperature and 756 mm. pressure.
Find out the volume of this gas at STP.
Ans : 34.16 ml
17. Find out the weight and mole-molecules number of nitrogen gas of 5 litre volume at 2
atmosphere pressure and 60 C temperature. (Atomic weight of N = 14 gram/mole)
Ans : 10.25 g N2
18. The volume of 1.2 gram of a gas is 1.2 litre at 27 C temperature and 740 mm pressure. Find
out the molecular weight of this gas.
Ans : 25.26 g / mol.
19. 2 gram of gas A when filled in a vessel at 25 C temperature, its pressure becomes 1
atmosphere. 3 gram of second gas B is filled in the same vessel at the same temperature its
pressure becomes 1.5 atmosphere. If both the gases behave as ideal gases, compare their
molecular weights.
Ans : The molecular weight of gas A is three times the molecular weight of gas B.
20. The volume of 10.254 gram of a diatomic gas is litre at 60C temperature and 2 atmosphere
pressure. Calculate the weight of one atom of this gas.
Ans : 2.324  10-23 g
21. The volume of vapour of 1.043 gram phosphorous is 100 ml. at 800 Kelvin temperature and
700 mm. pressure. Calculate the number of phosphorous atoms in each molecule of it.
Ans : Four atoms of phosphorous are in one molecule of Phosphorous.
2nd & 3rd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166 (M) +91- 98250-31559, +91-98981-74762
5
Baroda High School
Alkapuri
11TH (GSEB)
Pr. By. Smita Malik
Chapter - 2
SUB. CHEMISTRY
TOPIC States of Matter
22. The volume of a gas collected over water is 50 ml. at 15C temperature and 740 mm.
pressure. If the vapour pressure of dry gas of same volume at STP us 45.3 mm. What will be
the vapour pressure of a water at 15 C?
Ans : pH2O = 13.7 mm
23. 110 ml hydrogen gas is collected over water at 18 C and 749mm pressure. What will be the
volume of this gas at STP ? (vapour pressure of water at 18 C = 15.4 mm)
Ans : 98.4 ml.
24. Students in one school are seated on 12 benches in a class-room having two doors. The
laughing gas (N2O) from one door and tear gas (C6H11OBr) from other door are released at
the same time. The students sitting on which bench will experience at a time feeling of
laughing-crying ?
Ans : H = 1, c = 12, N = 14, O = 16, Br = 80 g/mole.
25. The molecular weight of an oxide of phosphorous is 284 gram/mole. If there are four atoms
of phosphorous in this oxide, fins its molecular formula. (Atomic weight : P = 31,
O = 16 gram / mole)
Ans : Molecular formula P4O10
26. The vapour density of one oxide of nitrogen is 3. If the nitrogen is diatomic in this oxide, find
molecular formula of the oxide.
Ans : N2O3
27. In a one-day cricket match, a cricketer drinks two glasses of a drink of glucose. If each glass
of water contains 1018 glucose molecules, how many grams of glucose be must have drunk ?
Ans : 2.988 10-4 g gram glucose.
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