Honors Chemistry Quiz: Chapter 5 Gas Laws
Name: ____________________ Period: ____ Date: _____________________
This quiz is worth 48 points. Only those quizzes completed in black ink will
be graded. Useful information: R= 0.08206 L-atm/mol-K. Good luck!
1) Convert 1.25 atm to mm Hg.
A) 760 mm Hg
B) 875 mm Hg
C) 950 mm Hg
D) 1000 mm Hg
E) 1520 mm Hg
2) The volume of a gas is proportional to number of moles of a gas is
known as
A) Avogadro's Law
B) Ideal Gas Law
C) Charles's Law
D) Boyle's Law
E) Dalton's Law
3) What volume will a balloon occupy at 1.0 atm, if the balloon has a
volume of 7.6 L at 3.8 atm?
A) 2.0 L
B) 5.0 L
C) 29 L
D) 35 L
E) 17 L
4) To what volume will a sample of gas expand if it is heated from 50.0°C
and 2.33 L to 500.0°C?
A) 5.58 L
B) 9.74 L
C) 10.3 L
D) 17.9 L
E) 4.38 L
5) The volume of a gas is proportional to the temperature of a gas is known
as
A) Avogadro's Law
B) Ideal Gas Law
C) Charles's Law
D) Boyle's Law
E) Dalton's Law
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6) If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions,
what volume will 0.66 moles occupy under the same conditions?
A) 12 L
B) 8.6 L
C) 17 L
D) 5.0 L
E) 15 L
7) A gas is at 35.0°C and 4.50 L. What is the temperature at 9.00 L?
A) 343°C
B) 70.0°C
C) 616°C
D) 1.16°C
E) 17.5°C
8) Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at
3.30 atm.
A) 64.0 K
B) 5.25 K
C) 337 K
D) 28.0 K
E) None of the above.
9) What pressure will 2.6 x 1023 molecules of H2 exert in a 3.9 L container
at 45°C?
A) 5.7 atm
B) 1.7 atm
C) 2.9 atm
D) 3.4 atm
E) 4.6 atm
10) Give the temperature and pressure at STP.
A) 0°C and 1.00 atm
B) 0K and 1.00 atm
C) 25°C and 30.00 in Hg
D) 300K and 1 torr Hg
E) 0°C and 1 mm Hg
11) Which of the following gas samples would be most likely to behave
ideally under the stated conditions?
A) Ne at STP
B) CO at 200 atm and 25°C
C) SO2 at 2 atm and 0 K
D) N2 at 1 atm and -70°C
E) O2 at 400 atm and 25°C
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12) The density of a gas is 1.43 g/L at STP. What is the gas?
A) Cl2
B) S
C) O2
D) Ne
E) None of the above.
13) Which of the following samples has the greatest density at STP?
A) NO2
B) Xe
C) SO2
D) SF6
E) All of these samples have the same density at STP.
14) A 0.465 g sample of an unknown compound occupies 245 mL at 298 K
and 1.22 atm. What is the molar mass of the unknown compound?
A) 26.3 g/mol
B) 33.9 g/mol
C) 12.2 g/mol
D) 38.0 g/mol
E) 81.8 g/mol
15) In a container containing CO, H2, and O2, what is the mole fraction of
CO if the H2 mole fraction is 0.22 and the O2 mole fraction is 0.58?
A) 0.20
B) 0.30
C) 0.10
D) 0.50
E) 0.75
16) Define vapor pressure.
A) partial pressure of water in a liquid mixture
B) partial pressure of water in a gaseous mixture
C) condensation of water
D) water dissolved in a liquid
E) water molecules
17) A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a
total pressure of 2.95 atm. What is the pressure of CO?
A) 1.86 atm
B) 0.649 atm
C) 0.536 atm
D) 1.54 atm
E) 0.955 atm
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18) A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm.
What is the partial pressure of Ne?
A) 1.1 atm
B) 0.80 atm
C) 0.54 atm
D) 0.40 atm
E) 1.3 atm
19) The following reaction is used to generate hydrogen gas in the
laboratory. If 243 mL of gas is collected at 25 °C and has a total pressure of
745 mm Hg, what mass of hydrogen is produced? A possibly useful table
of water vapor pressures is provided below.
Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
T (°C)
20
25
30
P (mm Hg)
17.55
23.78
31.86
A) 0.0196 g H2
B) 0.0717 g H2
C) 0.0190 g H2
D) 0.0144 g H2
E) 0.0449 g H2
20) Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce
55.0 g of S. Assume that there is excess SO2 present.
2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)
A) 44.0 L
B) 29.3 L
C) 22.7 L
D) 34.1 L
E) 66.0 L
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21) Determine the volume of SO2 (at STP) formed from the reaction of 96.7
g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2
is 119.99 g/mol.
4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)
A) 36.1 L
B) 45.3 L
C) 18.1 L
D) 27.6 L
E) 32.9 L
22) A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container.
Which of the following statements is TRUE?
A) Both gases have the same average kinetic energy.
B) Both gases contribute equally to the density of the mixture under these
conditions.
C) Both gases have the same molecular speed.
D) The mixture has a volume of 22.4 L
E) All of the above are TRUE.
23) Which statement is TRUE about kinetic molecular theory?
A) A single particle does not move is a straight line.
B) The size of the particle is large compared to the volume.
C) The collisions of particles with one another is completely elastic.
D) The average kinetic energy of a particle is not proportional to the
temperature
E) None of the above statements is true.
24) According to Kinetic Molecular Theory,
A) Boyle’s Law cannot be explained because gas particles cannot be
forced closer together by increasing the pressure exerted on the gas.
B) Charles’ Law can be explained because higher temperatures mean that
on average gas particles have greater energy and therefore expand,
creating a greater volume.
C) Avogadro’s Law can be explained because more molecules create more
pressure which causes the volume to increase when pressure is held
constant.
D) Dalton’s Law of Partial Pressure can be explained because particles of
different gases act dependently, therefore it is difficult to determine each
gas’ contribution to the total pressure.
E) Both B and C are correct.
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