Chapter 5 - Review
1. The atmospheric pressure at the top of a ski run was 615 Torr. What is this pressure in
kPa?
A) 101 kPa B) 125 kPa C) 0.809 kPa D) 82.0 kPa E) 1.24 kPa
2. A gas sample has a volume of 9.8 L at 720 Torr. If the temperature is constant, what
volume does the gas sample have at 1.5 atm?
A) 6.9 L B) 5.7 L C) 0.16 L D)6.2L E) 9.3 L
3. A 2.50-L sample of neon has a pressure of 1.59 atm at 45.0°C. What volume would the
sample have if the pressure is 725 Torr and the temperature 22.0°C?
A) 3.07 L B) 1.62 L C) 3.87 L D) 2.04 L E) 0.733 L
4. Ammonia burns in air as follows:
4NH3(g) + 302(g) -* 2N2(g) + 6H20(g)
How many liters of N2(g) are formed by burning 2.50 L of ammonia in excess oxygen
with all species at the same temperature and pressure?
A) 2.00 L B) 2.50 L C) 1.25L D) 5.00 L E) 0.625 L
5. What is the pressure of 10.0 g of nitrogen gas in a container of volume 3.00 L at a
temperature of-88.0°C?
A) 183 kPa B) 87.1 kPa C) 174 kPa D) 1.81 kPa E) 366 kPa
6. A 1.00-L sample of a gas at 705 Torr and 47°C has a mass of 0.988 g. The gas is
A) CO B) CO2 C) CH4 D) CF4 E) C12
7. What mass of sulfur dioxide will exert the same pressure as 50.0 mg of carbon dioxide in
the same container under the same conditions?
A) 36.4 mg B) 72.8 mg C) 1.14mg D) 50.0 mg E) 24.3 mg
8. What volume of carbon dioxide measured at 40°C and 760 Torr would be produced by
the combustion of 454 g of glucose, C6H12O6(s)?
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9. Calculate the volume occupied by 10.0 moles of chlorine gas at STP.
A) 224 L B) 112L C) 22.4 L D) 245 L E) 448 L
10. The volume of 1.10 g of an unknown diatomic gas is 625 mL at STP. What is the molar
mass of the gas?
A) 15.4 g-mol B) 25.4g-mol C) 39.4 g-mol D) 30.7 g-mol E) 35.8 g-mol
11. Consider the following reaction.
4NH4C104(s) -* 2Cl2(g) + 8H20(g) + 2N2O(g) + 3O2(g)'
Calculate the total volume of all gases produced at STP by the decomposition of two
moles of ammonium perchlorate.
A) 15.0 L B) 168 L Q78.4L D) 336 L E)7.50L
12. Consider the following reaction.
CS2(g) + 302(g) - C02(g) + 2S02(g)
If 8.83 L of SO2(g) are produced at STP, how many grams of CS2(g) are required?
A) 30.0 g B) 98.9 g C) 12.6 g D) 25.3 g E) 15.0 g
13. Which of the following gases has the lowest density at STP?
A) methane, CH4 B) argon C) fluorine D) nitrogen E) ozone, O3
14. An unknown sample of a gas has a density of 3.09 g/L at 245 kPa and 75°C. Which of the
following is the gas?
A) HC1 B) HF C) BF3 D) NO2 E) SO2
15. A 500-mL sample of dry air (measured at sea-level pressure, 760 Torr) contains 0.2314 g
of oxygen at 25°C. Calculate the partial pressure of oxygen in the sample.
A) 0.707 atm B) 0.231 atm C) 0.0358 atm D) 0.354 atm E) 0.0297 atm
16. Which gaseous molecules (choose one species) effuse slowest?
A) S02(g) B) Ar(g) C) N0(g) D) Ne(g) E) CO2(g)
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17. The time required for 0.010 moles of SC>3(g) to effuse through an opening was 22 s.
Under the same conditions, an unknown gas required 30 s. The unknown gas is probably
A) SiF4(g) B) SF4(g) C) CF4(g) D) SF6(g) E) PF5(g)
18. The rate of diffusion of H2Te(g) at 25 °C would be what factor times the rate of diffusion
of gaseous ammonia at 25°C?
A) 0.362 B) 0.761 C) 0.131 D) 2.76 E) 0.181
19. In air at 25°C, which gas has the lowest average speed?
A) C02(g) B) H20(g) C) C0(g) D) Ne(g) E) CH4(g)
20. Consider the gas ethylene, C2H4(g) at 48 atm and 25°C. Calculate the volume of ethylene
using the van der Waals equation and the ideal gas equation. The van der Waals constants
for ethylene are a = 4.47 L2 atm moh2 and b = 0.057 L moH. Explain the results.
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