Honors Chemistry Quiz: Gas Laws
Name: ____________________ Period: ____ Date: _____________________
This quiz is worth 40 points. Only those quizzes completed in black ink will
be graded. Good luck!
R = 0.08206 L-atm/mol-K
1) What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5
atm, if the F2 has a volume of 25.0 mL at 1.2 atm?
A) 11 mL
B) 17 mL
C) 3.8 mL
D) 5.5 mL
E) 7.6 mL
2) A large balloon is initially filled to a volume of 25.0 L at 353 K and a
pressure of 2575 mm Hg. What volume of gas will the balloon contain at
1.35 atm and 253 K?
A) 22.2 L
B) 87.5 L
C) 11.4 L
D) 45.0 L
E) 58.6 L
3) How many moles of CO are contained in a 5.00 L tank at 155°C and 2.80
atm?
A) 0.399 moles
B) 1.10 moles
C) 2.51 moles
D) 0.455 moles
E) 0.289 moles
4) What is the volume of 5.60 g of O2 at 7.78 atm and 415K?
A) 1.53 L
B) 565 L
C) 24.5 L
D) 25.0 L
E) 0.766 L
5) 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
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6) Which of the following samples will have the greatest volume at STP?
A) 22 g CO
B) 22 g He
C) 22 g O2
D) 22 g Cl2
E) All of these samples would have the same volume at STP.
7) Which of the following samples will have the lowest pressure if they are
all at the same temperature and in identical containers (same volume)?
A) 15 g F2
B) 15 g Ne
C) 15 g Kr
D) 15 g CO2
E) All of these samples will have the same pressure.
8) Determine the density of CO2 gas at STP.
A) 1.96 g/L
B) 1.80 g/L
C) 2.24 g/L
D) 4.46 g/L
E) 5.10 g/L
9) A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and
1.41 atm. What is the identity of the halogen?
A) Br2
B) F2
C) Cl2
D) I2
E) Ge
10) 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
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11) 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
12) 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
13) 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
14) What pressure would a gas mixture in a 10.0 L tank exert if it were
composed of 48.5 g He and 94.6 g CO2 at 398 K?
A) 39.6 atm
B) 7.02 atm
C) 32.6 atm
D) 46.6 atm
E) 58.7 atm
15) 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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16) Determine the mass of water formed when 12.5 L NH3 (at 298 K and
1.50 atm) is reacted with 18.9 L of O2 (at 323 K and 1.1 atm).
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
A) 17.0 g H2O
B) 20.7 g H2O
C) 37.7 g H2O
D) 13.8 g H2O
E) 27.9 g H2O
17) 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.
18) Which statement is TRUE about kinetic molecular theory?
A) A single particle does not move in 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.
19) Identify the gas particle that travels the fastest.
A) H2
B) O2
C) Ne
D) N2
E) CO
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20) According to Kinetic Molecular Theory,
A) Boyle’s Law can be explained because gas particles can be forced
closer together by increasing the pressure exerted on a gas.
B) Charles’ Law can be explained because higher temperatures means
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 can be held constant by increasing the volume.
D) Dalton’s Law of Partial Pressure can be explained because particles of
different gases act independently, therefore each gas contributes its own
pressure to the total pressure of the mixture.
E) All the above.
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