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Assignment questions
ASSIGNMENT 1
Due date: To be made available online on myunisa
This assignment must be completed electronically on myUnisa. Assignment 1 is based
on Study Units 1-3 of the syllabus. This corresponds to chapters (1, 2, 6 & 7) of the
prescribed textbook: Chemistry 2e.
Assignment Questions:
Question 1
Silver cannot be broken down into simpler substances by chemical means. It is therefore
[1] a mixture
[2] an element
[3] a proton
[4] a compound
[5] an electron
Question 2
Which of these are homogeneous mixtures and which are heterogeneous mixtures?
(a) Fine gas bubbles in water, rising to the surface.
(b) Fine sand in water, constantly mixed.
(c) An aqueous solution of sodium chloride and ink.
(d) Soil.
(e) Air.
(f) A cup of coffee with sugar stirred in.
1. (a), (b), (d) are homogeneous mixtures and (c), (e), (f) are heterogeneous mixtures.
2. (a), (c), (e) are heterogeneous mixtures and (b), (d), (f) are homogeneous mixtures.
3. (a), (b), (c), (d), (e), (f) are all homogeneous mixtures.
4. (a), (b), (d) are heterogeneous mixtures and (c), (e), (f) are homogeneous mixtures.
5. (a), (b), (c), (d), (e), (f) are all heterogeneous mixtures.
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Question 3
Which of the following is a compound?
[1] Gold
[2] Iron
[3] Milk
[4] Sucrose
[5] Coffee
Question 4
Which of these changes below are physical and which are chemical?
(a) Plants make sugar from carbon dioxide and water.
(b) Water vapour in the air forms frost.
(c) A goldsmith melts a nugget of gold and pulls it into a wire.
(d) iron that rusts.
(e) tobacco converted to smoke.
1. (a), (d), (e) are physical changes and (b), (c) are chemical changes.
2. (a), (b), (c), are chemical changes and (d), (e) are physical changes.
3. (a), (b), (c), (d), (e) are all chemical changes.
4. (a), (d), (e) are chemical changes and (b), (c) are physical changes.
5. (a), (b), (c), (d), (e) are all physical changes.
Question 5
Convert 2.34 m3 to μm3. Write the answer in scientific notation. The power of the ten in the
answer is …
1. +18.
2. -18.
3. +9.
4. -9.
5. +6.
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Question 6
The length of an object was measured as 0.0000340 nm. This length expressed in scientific
notation is …
1. 3.4 x 105 nm.
2. 3.40 x 105 nm.
3. 3.4 x 10-5 nm.
4. 3.40 x 10-5 nm.
5. None of the above.
Question 7
Consider the following three measured quantities: 1.00340 x 10-4 mg, 0.0023030 L, 100.00303
kg. The correct numbers of significant figures in these values are …, respectively.
1. 6, 8, 8
2. 5, 5, 6
3. 6, 4, 8
4. 5, 7, 6
5. 6, 5, 8
Question 8
The mass of a metal cylinder was determined on an analytical balance to be 33.745 g. The
volume of a cylinder is measured and determined to be 2.70 mL. What is the density of a
cylinder, expressed to the proper number of significant figures?
1. 0.0800 g/mL
2. 0.080012 g/mL
3. 12.498 g/mL
4. 12.5 g/mL
5. 12 g/mL
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Question 9
Which one of the following phrases corresponds with the meaning of the term “accuracy”?
1. how precise
2. how trustworthy
3. number of significant figures
4. how correct
5. how scientific
Question 10
Precision refers to:
[1] how close a measured number is to zero.
[2] how close a measured number is to infinity.
[3] how close a measured number is to the calculated value.
[4] how close a measured number is to the true value.
[5] how close a measured number is to other measured numbers.
Question 11
An ion has a mass number of 37, atomic number 17, and a charge of -1. How many protons
does it have?
[1] 1
[2] 16
[3] 17
[4] 37
[5] 54
Question 12
How many protons, neutrons and electrons are there in the naturally occurring isotope
.
[1]
[2]
[3]
[4]
[5]
protons=17,
protons=19,
protons=36,
protons=20,
protons=17,
neutrons=19,
neutrons=21,
neutrons=36,
neutrons=36,
neutrons=19,
electrons=17
electrons=14
electrons=17
electrons=14
electrons=18
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Question 13
Magnesium is the ninth most abundant element in the universe and has three isotopes. Given
the following information table, and that the average atomic mass of magnesium is 24.31 amu,
determine and write the atomic symbol of the unknown isotope.
[1] 24Mg[2] 26Mg2+
[3] 25Mg
[4] 12Mg
[5] None of the above
Question 14
A white powder compound was analysed and found to contain 4 phosphorus atoms and 10
oxygen atoms. What is the empirical formula of this compound?
1. PO3
2. PO2
3. PO2,5
4. P2O5
5. P4O10
Question 15
What are the respective formulae for the cyanate and sulfite ions?
1. CN- and SO322. NCO- and S2O323. C2O42- and S24. NCO- and SO325. CN- and S2O32-
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Question 16
Which formula / name pair is incorrect?
[1] Mn(NO2)2 Manganese(II) nitrite
[2] Mg(NO3)2 Magnesium nitrate
[3] Mn(NO3)2 Manganese(II) nitrate
[4] Mg3N2 Magnesium nitrite
[5] Mg(MnO4)2 Magnesium permanganate
Question 17
Give the condensed (noble core) electron configuration for the carbon (C) atom.
1. 1s22s2
2. 1s22s22p2
3. [He] 2s2
4. [He] 2s22p2
5. None of the above
Question 18
How many valence electrons in a C atom having quantum number, ℓ = l?
1. 2
2. 4
3. 6
4. 0
5. None of the above
Question 19
Write a valid set of four quantum numbers for the valence electron of C with ℓ = 1
1. n = 2, ℓ = 1, ml = -1, ms = + ½
2. n = 1, ℓ l = 1, ml = -1, ms = - ½
3. n = 2, ℓ = 1, ml = 0, ms = + ½
4. Both 1 and 3
5. None of the above
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Question 20
Which of the following electron configurations is not possible?
1. 1s2 2s2 2p6
2. 1s2 2s1
3. 1s2 2s2 2p6 3s1
4. 1s2 2s3 2p3.
5. All of the above are possible
Question 21
Which one of the following sets of atoms/ions is isoelectronic?
1. H+, H and H2. Li+, Na+ and K+
3. Cl-, Br- and I4. F-, Ne and Na+
5. None of the above sets of atoms/ions is isoelectronic
Question 22
Which quantum number(s) do 2s and 2p orbitals have in common?
1. ℓ
2. ℓ and mℓ
3. n
4. n, mℓ and ms.
5. None of the above
Question 23
Which of the following has the greatest difference between the first and the second ionisation
energy?
1. Si
2. S
3. P
4. Mg
5. Na
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Question 24
The radius of an anion is always larger than the radius of the neutral atom of that element
because …
1. the core of the anion is larger.
2. energy was released when the anion was formed.
3. of the repulsion between the valence electrons in the anion.
4. the anion is in the excited state.
5. there is more shielding by the core electrons in an anion.
Question 25
Place the following elements in order of decreasing radii: Se, Rb, In, Br, As, Ga
1. Rb > In > Ga > As > Se > Br
2. Ga > In > Rb > Se > As > Br
3. Se > Br > Ga > As > Rb > In
4. Br > Se > As > In > Rb > Ga
5. In > Rb > As > Ga > Br > Se
Question 26
Which one of the following elements has the highest first ionization energy?
1. Br
2. As
3. N
4. Sb
5. all the above has the same ionization energy
Question 27
Which one of the following elements has the lowest electron affinity?
1. Se
2. As
3. Ga
4. K
5. all of the above has the same electron affinity
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Question 28
Bonds formed by elements of widely different electronegativities are:
1. Covalent double bonds
2. Non-polar covalent bonds
3. Hydrogen bonds
4. Ionic bonds
5. Carbon bonds
Consider each of the following pairs of atoms below in questions 29-32 and predict the type of
bonding that will occur between the atoms.
Question 29
LiBr
1. Non-polar covalent bond
2. Polar covalent bond
3. Covalent coordinate
4. Ionic bond
5. None of the above
Question 30
NO
1. Polar covalent bond
2. Non-polar covalent bond
3. Covalent coordinate bond
4. Ionic bond
5. None of the above
Question 31
FeO
1. Non Covalent coordinate
2. Transition element bond
3. Covalent coordinate bond
4. Ionic bond
5. None of the above
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Question 32
CH
1. Hydrogen bond
2. Non-polar covalent bond
3. Polar covalent bond
4. Ionic bond
5. None of the above
Question 33
Consider the sulfite ion molecule: SO32-. Calculate the number of valence electrons in this
molecule.
[1] 24
[2] 12
[3] 22
[4] 26
[5] 18
Question 34
How many lone pairs of electrons are there in the Lewis structure of XeF4
[1] 2
[2] 4
[3] 6
[4] 12
[5] 14
Question 35
Draw the Lewis structure of SO3. The formal charge of the O atoms is
[1] +2
[2] +1
[3] 0
[4] -1
[5] -2
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Question 36
In the AB4 molecule there are 2 lone pairs of electrons on the A atom. What is the shape of the
molecule?
[1] tetrahedral
[2] trigonal pyramidal
[3] bent
[4] square planar
[5] linear
Question 37
Find a pair that are isoelectronic with one another and hence have the same geometry:
[1] carbonate and phosphate ions
[2] sulphite and chlorate ions
[3] sulphate and sulphite ions
[4] nitrate and chlorate ions
[5] carbonate and chlorate ions
Question 38
For the species XeF3+, the electronic and molecular geometry are …, respectively.
1. trigonal pyramidal and seesaw
2. trigonal pyramidal and T-shaped
3. tetrahedral and tetrahedral
4. octahedral and square pyramidal
5. trigonal bipyramidal and T-shaped
Question 39
Which of the following has a dipole moment?
[1] IF5
[2] XeF4
[3] SF6
[4] PCl5
[5] CH4
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ASSIGNMENT 2
Due date: To be made available online on myunisa
This assignment must be completed electronically on myUnisa. Assignment 2 is based
on Study Units 4, 5 & 6 of the syllabus. This corresponds to chapters (3 & 4) of the
prescribed textbook: Chemistry 2e.
Assignment Questions:
Question 1
According to the solubility rules, which of the following compounds will be soluble in
water?
[1] Silver bromide.
[2] Calcium sulfate.
[3] Magnesium fluoride.
[4] Lead sulfate.
[5] Lithium nitrate.
Question 2
Consider an acid-base reaction when hydrochloric acid is added to copper(II) hydroxide. What is
the net ionic equation for this reaction?
[1] H+(aq) + OH-(aq) → H2O(l)
[2] 2H+(aq) + Cu(OH)2(s) → Cu2+(aq) + 2H2O(l)
[3] 2HCl(aq) +Cu(OH)2(s) → CuCl2(s) + 2H2O(l)
[4] 2H+(aq) + 2Cl-(aq) + Cu2+(aq) + 2OH-(aq) → CuCl2(s) + 2H2O(l)
[5] 2H+(aq) + 2Cl-(aq) + Cu2+(aq) + 2OH-(aq) → Cu2+(aq) + 2Cl-(aq) + 2H2O(l)
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Question 3
Consider the following chemical reaction:
CdCl2(aq) + NaOH(aq) → Cd(OH)2 + NaCl
After correctly balancing the reaction above, the coefficient of NaOH will be?
[1] 1
[2] 2
[3] 3
[4] 4
[5] 5
Consider the following balanced redox reaction, and answer Questions 4 - 7
2 PbS (s) + 3O2 (g) → 2PbO (s) + 2SO2 (g)
Question 4
Which species contains an element acting as the reducing agent.
[1] O2
[2] PbO
[3] SO2
[4] PbS
[5] None of the above
Question 5
Which element is reduced?
[1] P
[2] O
[3] S
[4] Both P and S
[5] None of the above
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Question 6
Which species contains the element with the highest oxidation number?
[1] O2
[2] PbS
[3] SO2
[4] PbO
[5] None of the above
Question 7
How many electrons are lost by the Sulphur atom?
[1] 2
[2] 0
[3] 4
[4] 1
[5] 6
Question 8
What type is the following reaction: Ba(OH)2(aq) + HNO3(aq) → Ba(NO3)2 + H2O
[1] Combustion
[2] Precipitation
[3] Redox
[4] Synthesis (Combination)
[5] Neutralization
Question 9
Identify the type of a reaction in the following reaction: Mg(OH)2(s) → MgO(s) + H2O (l)
[1] Combustion
[2] Precipitation
[3] Decomposition
[4] Synthesis (Combination)
[5] Neutralization
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Question 10
How many number of moles of carbon atoms are there in one mole of Glucose, C6H12O6
[1] 72
[2] 12
[3] 12.01
[4] 6
[5] None of the above
Question 11
Iron is the most common element on earth, forming much of earth's outer and inner core. How
many iron atoms are in 6.00 g of iron metal?
[1] 6.47 x 1023 atoms
[2] 0.107 atoms
[3] 5.61 x 1024 atoms
[4] 6.47 x 1022 atoms
[5] 9.31 atoms
Question 12
Calculate the number of moles of CH4 present in 45.0 g of CH4
[1] 0.356 mol
[2] 2.81 mol
[3] 3.46 mol
[4] 45.0 mol
[5] 28.1 mol
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Question 13
Magnesium hydroxide, Mg(OH)2, is white inorganic solid compound which occur in nature as
mineral brucite, and is a common component of antacids, such as milk of magnesia. A sample
of this mineral brucite is found to contain 0.525 moles of magnesium. Calculate the mass
Mg(OH)2 contained in this sample.
[1] 111 g
[2] 3.06 g
[3] 0.525 g
[4] 30.6 g
[5] None of the above
Question 14
A certain compound has the following percent composition of 49.47% C, 5.21% H, 28.84% N,
and 16.48% O. If the compound has a molecular mass of 194.2 g.mol -1, calculate the empirical
formula mass (g/mol) for this compound.
[1] 43.03 g/mol
[2] 4.303 g/mol
[3] 97.1 g/mol
[4] 194.2 g/mol
[5] None of the above
Question 15
What is the molecular formula of the compound in question 14 above?
[1] C4H5N2O
[2] C12H15N6O3
[3] C8H10N4O2
[4] C2H2,5NO1,5
[5] None of the above
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Consider the reaction of hydrogen and oxygen to form water:
2H2 + O2 → 2H2O
And answer questions 16 – 18 below
Question 16
Which is the limiting reactant when 5.00 g of H2 and 10.0 g of O2 react?
[1] H2 is the limiting reagent
[2] H2O is the limiting reagent
[3] There is no limiting reagent
[4] O2 is the limiting reagent
[5] Both H2 and O2 are limiting reagents
Question 17
What is the maximum number of moles of H2O that can be formed?
[1] 0.3125 mol
[2] 2.48 mol
[3] 1.855 mol
[4] 4.96 mol
[5] 0.625 mol
Question 18
How many moles of the excess reagent remain unreacted?
[1] 0.625 mol
[2] 1.86 mol
[3] 2.48 mol
[4] 0.3125 mol
[5] 4.96 mol
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Question 19
Upon reaction of 32.9 g of CCl4 with excess HF, 12.5 g of the gas of Freon, CF2Cl2, was
obtained according to the equation: CCl4 + 2HF ⟶ CF2Cl2 + 2HCl
Calculate the percent yield of Freon.
[1] 38.0%
[2] 12.5%
[3] 48.3%
[4] 27.5%
[5] None of the above
Question 20
Calculate the molarity of 6.52 g of CoCl2 dissolved in an aqueous solution with a total volume of
75.0 mL.
[1] 6.69 x 10-4 mol. L-1
[2] 0.669 mol. L-1
[3] 6.69 mol. L-1
[4] 1.49 mol. L-1
[5] None of the above
Question 21
How many grams of CaCl2 are contained in 250.0 mL of a 0.200 mol. L-1 solution of calcium
chloride?
[1] 5.55 g
[2] 88.7 g
[3] 138.7 g
[4] 55.5 g
[5] None of the above
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Question 22
If I prepare a solution by adding 75.0 mL of 1.25 mol. L-1 HCl into a 250 mL volumetric flask, and
filling the flask to the mark with water, what will the final concentration of the solution be?
[1] 0.288 mol. L-1
[2] 4.17 mol. L-1
[3] 0.962 mol. L-1
[4] 0.375 mol. L-1
[5] None of the above
Question 23
The concentration of acetic acid in white vinegar was determined to be 0.745 mol. L-1. What
volume of vinegar contains 8.05 x 104 mg of acetic acid?
[1] 1.80 x 103 L
[2] 1.80 x 106 L
[3] 0.556 L
[4] 1.80 L
[5] None of the above
Question 24
A solution is prepared by dissolving 50.0 g of cesium chloride (CsCl) in 50.0 g of water. The
volume of the solution is 63.3 mL. What is the molality of the cesium chloride?
[1] 29.7 mol/kg
[2] 55.4 mol/kg
[3] 5.94 mol/kg
[4] 4.69 mol/L
[5] 0.00469 mol/L
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Question 25
What is the mole fraction of the cesium chloride in question 24?
[1] 0.0968
[2] 0.903
[3] 1.00
[4] 0.968
[5] 0.00
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ASSIGNMENT 3
Due date: To be made available online on myunisa
This assignment must be completed electronically on myUnisa. Assignment 2 is based
on Study Units 6, 8 & 11 of the syllabus. This corresponds to chapters (13 & 9) of the
prescribed textbook: Chemistry 2e.
Assignment Questions:
Question 1
If a reaction is reversible, when can it be said to have reached equilibrium?
[1] When the reactants and the products are homogeneous.
[2] When the amount of products is equal to the amount of reactants.
[3] When the forward and reverse reactions continue to proceed, but at equal rates.
[4] When the reactants and the products are heterogenous.
[5] When the amount of products is greater than the amount of reactants.
Question 2
What is the expression for the equilibrium constant for the reaction represented by the equation:
Pb2+(aq) + 2Cl-(aq) ⇌ PbCl2 (s)
[1]
Kc = [PbCl2] / [Pb2+][Cl-]2
[2]
Kc = [Pb2+][Cl-]2 / [PbCl2]
[3]
Kc = [Pb2+][Cl-]2
[4]
Kc = 1 / [Pb2+][Cl-]2
[5]
None of the above.
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Question 3
Consider the reaction: HF (aq) ⇆ H+ (aq) + F- (aq)
Suppose that the value of the equilibrium constant is very large, which species will predominate
at equilibrium?
[1] Only the reactant (HF) will predominate at equilibrium.
[2] Only H+
[3] Only F[4] The products (both H+ and F-) will predominate at equilibrium
[5] All species will predominate at equilibrium.
Question 4
The initial concentrations of reactants and products are given for the following system. Calculate
the reaction quotient and determine the direction in which this system will proceed to reach
equilibrium.
2NH3 (g) ⇆ N2 (g) + 3H2 (g)
Kc = 17;
[NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M
[1] Qc < Kc, the system will proceeds left
[2] Qc > Kc, the system will proceeds left
[3] Qc > Kc, the system will proceed right
[4] Qc < Kc, the system will proceeds left
[5] Qc = Kc, the system is at equilibrium
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Question 5
Which of the systems listed below are homogeneous equilibria? Which are heterogeneous
equilibria?
(a) 2Bi3+ (aq) + 3S2- (aq) ⇆ Bi2S3 (s)
(b) N2 (g) + O2 (g) ⇆ 2NO (g)
(c) CH4 (g) + 2O2 (g) ⇆ CO2 (g) + 2H2O (ℓ)
(d) CuSO4.5H2O (s) ⇆ CuSO4 (s) + 5H2O (g)
Choose the correct answer below:
[1] (b), (c) are homogeneous equilibria; (a), (d) are heterogeneous equilibria
[2] (b), (c) are heterogeneous equilibria; (a), (d) are homogeneous equilibria
[3] (a), (c), (d), are homogeneous equilibria; (b) is heterogeneous equilibria.
[4] all the systems listed are heterogeneous equilibria.
[5] (a), (c), (d), are heterogeneous equilibria; (b) is homogeneous equilibria.
Consider the following reaction, for which ΔH(reaction) = + 879.35 kJ, at 750°C, and answer
questions 6 – 10 below:
CH4(g) + H2O(g) CO(g) + 3H2(g)
Question 6
What will happen to the reaction mixture at equilibrium if some H2O(g) is removed??
[1]
The equilibrium will shift to the right.
[2]
The equilibrium will shift to the left
[3]
There is no effect on the equilibrium.
[4]
The reaction will stop.
[5]
None of the above.
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Question 7
What will happen to the reaction mixture at equilibrium if the temperature is increased?
[1]
The equilibrium will shift to the right.
[2]
The equilibrium will shift to the left.
[3]
There is no effect on the equilibrium.
[4]
The reaction will stop.
[5]
None of the above.
Question 8
What will happen to the reaction mixture at equilibrium if an inert gas is added?
[1]
The equilibrium will shift to the left.
[2]
The equilibrium will shift to the right.
[3]
There is no effect on the equilibrium.
[4]
The reaction will stop.
[5]
None of the above.
Question 9
What will happen to the reaction mixture at equilibrium if more of CO(g) is added?
[1]
The equilibrium will shift to the right.
[2]
The equilibrium will shift to the left.
[3]
There is no effect on the equilibrium.
[4]
The reaction will stop.
[5]
None of the above.
Question 10
What will happen to the reaction mixture at equilibrium if the volume of the container is
increased?
[1]
The equilibrium will shift to the right.
[2]
The equilibrium will shift to the left.
[3]
There is no effect on the equilibrium.
[4]
The reaction will stop.
[5]
None of the above.
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Question 11
A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344
torr at 23 C. If the can is thrown into a fire (T = 475 C), what will be the pressure in the hot
can?
[1]
2.4 x 104 Torr
[2]
65 torr.
[3]
532 Torr.
[4]
340 Torr.
[5]
3.40 x 103 Torr.
Question 12
A 2.50 x 103 mL volume of hydrogen measured at –196 C is warmed to 100 C. Calculate the
volume of the gas (in liters) at the higher temperature, assuming no change in pressure.
[1] The volume will decrease by 1.28 L
[2] The volume will increase by 1.28 L
[3] The volume will be 12.1 L at the higher temperature
[4] The volume will be -1.28 L at the higher temperature
[5] There will be no change in volume
Question 13
A weather balloon contains 8.80 moles of helium at a pressure of 0.992 atm and a temperature
of 25 C at ground level. What is the volume of the balloon under these conditions?
[1] 18.2 L
[2] 4.61 x 10-3 L
[3] 2.17 L
[4] 217 L
[5] None of the above
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Question 14
How many grams of CO2 gas are present with the following information provided?
0.100 L of CO2 at 307 torr and 26 C
[1] 7.25 x 10-2 g
[2] 55.1 g
[3] 634 g
[4] 7.25 g
[5] 7.25 x 10-4 g
Question 15
Calculate the density of Freon 12, CF2Cl2, at 30.0 C and 0.954 atm.
[1] 46.4 g/L
[2] 4.64 g/mL
[3] 4.64 g/L
[4] 6.40 g/L
[5] None of the above
Question 16
A 36.0–L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories
contains 350 g CO2, 805 g O2, and 4880 g N2. At 25° C, what is the pressure in the cylinder in
atmospheres.
[1] 141 atm
[2] 107000 atm
[3] 14300 atm
[4] 14.1 atm
[5] None of the above
Question 17
What is the partial pressure of oxygen in a container that contains 2.0 mol of oxygen, 3.0 mol of
nitrogen, and 1.0 mol of carbon dioxide when the total pressure is 900 Torr?
[1]
100 Torr
[2]
200 Torr
[3]
300 Torr
[4]
400 Torr
[5]
None of the above
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Question 18
A flask of 1.00 L contains a mixture of 1.00 g of hydrogen gas and 1.00 g of helium gas at 27°C.
What is the total pressure in the flask?
[1]
6.15 atm
[2]
12.2 atm
[3]
18.4 atm
[4]
22.1 atm
[5]
None of the above
Question 19
A sample of carbon monoxide was collected over water at a total pressure of 756 torr and a
temperature of 18 C. What is the pressure of the carbon monoxide? The vapor pressure of
water at 18 °C is 15.5 torr.
[1] 772 torr
[2] 77.2 torr
[3] 74.0 torr
[4] 740 torr
[5] 15.5 torr
Question 20
Calculate the mass of carbon monoxide gas collected in question 19 above, if the volume of
the collected gas is 3.00 L.
[1] 3.43 g
[2] 5.38 g
[3] 34.2 g
[4] 342 g
[5] 538 g
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UNISA 2023
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