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Chapter 9: Gases: Their Properties and Behavior

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Self Quiz 2

Self Quiz 2

This activity contains 20 questions.

	According to Charles' law, the straight line resulting from the relationship of volume and temperature can be extrapolated to   -300°C. -273°C. -273°F. 0°F. 0°C.

	According to Graham's law, the rate of effusion is   inversely proportional to the molar mass of a gas. directly proportional to the square root of the molar mass of a gas. directly proportional to the molar mass of a gas. inversely proportional to the square root of the molar mass of a gas. inversely proportional to the square of the molar mass of a gas.

	As the pressure on a sample of gas increases,   the volume occupied by the gas particles becomes smaller. the percentage of volume occupied by the gas particles remains constant. the percentage of volume occupied by the gas particles becomes larger. the volume occupied by the gas particles becomes larger. the percentage of volume occupied by the gas particles becomes smaller.

	One component of a two-component gaseous mixture has a partial pressure of 455 mm of mercury. The total number of moles of gases in the mixture is 3.50 moles, and the total pressure is 856 mm of mercury. If this component is water vapor, then how many grams of water vapor are in this mixture?   29.5 g of water vapor. 31.7 g of water vapor. 9.57 g of water vapor. 119 g of water vapor. 33.5 g of water vapor.

	The molar mass (in amu) of a gas if it diffuses 1.45 times faster than C4H10 is   40.1 amu. 1.61 x 103 amu. 122 amu. 27.6 amu. 84.3 amu.

	The most likely identity of a gas with an average molecular speed of 498 m/s at 25°C is   NO2. CH3. H2. C2H6. H.

	The ozone layer in the Earth's stratosphere effectively   absorbs microwave radiation from the sun. absorbs ultraviolet radiation from the sun. absorbs radio waves from the sun. reflects infrared radiation emitted from the Earth. reflects ultraviolet radiation from the sun.

	The partial pressure in millimeters of mercury of O2 in a gaseous mixture containing 3.00 g of O2, 3.00 g of N2, and 3.00 g of Ar and having a pressure of 6.00 x 102 millimeters of Hg is   112 mm Hg. 2.00 x 102 mm Hg. 56.2 mm Hg. 2.04 x 102 mm Hg. 2.36 x 102 mm Hg.

	The reaction of sulfuric acid with iron was often used to produce hydrogen gas for balloons in the nineteenth century. If the reaction is H2SO4(aq) + Fe(s) ---> FeSO4(aq) + H2(g), what mass of iron (in grams) is required to produce enough H2 to fill an 18.0 L balloon at a temperature of 15°C and pressure of 755 mm of mercury?   1.53 g 3.21 x 104 g 73.8 g 42.3 g 811 g

	The temperature of a 10.0 L sample of nitrogen is increased from 22°C to 202°C, while its pressure is increased from 1.00 atm to 3.00 atm. What is the new volume (in liters) of the nitrogen sample?   7.39 L 2.07 L 0.363 L 5.37 L 30.6 L

	What amount of carbon dioxide (in grams) is generated by a reaction if 40.2 mL of the gas is collected at 23°C and 755 mm Hg?   0.931 g 72.3 g 7.24 x 10-2 g 4.60 x 10-2 g 1.64 x 10-3 g

	What is the pressure of a gas in millimeters of mercury in the sample container connected to a water-filled, open-ended manometer if the level in the arm connected to the atmosphere is 42.4 mm higher than in the arm connected to the sample container and if atmospheric pressure is 1.003 atm? The density of mercury is 13.6 g/mL, and the density of water is 1.00 g/mL (1 atm/760 mm Hg).   804.7 mm Hg 719.9 mm Hg 765.4 mm Hg 759.2 mm Hg 1338.9 mm Hg

	What is the pressure of a gas in millimeters of mercury in a sample container connected to a mercury-filled, open-ended manometer if the level of mercury in the arm connected to the atmosphere is 3.41 cm lower than the arm connected to the sample container and if atmospheric pressure is 99.54 kPa (101.325 kPa/1 atm)?   743.2 mm Hg 712.5 mm Hg 780.7 mm Hg 490.8 mm Hg 1002 mm Hg

	What volume of Cl2 (in milliliters) is required to produce 1.00 g of PCl3 according to the equation P4(s) + 6Cl2(g) ---> 4PCl3(l) if the temperature is 125°C and the pressure is 1.02 atm?   3.50 x 102 mL 1.55 x 102 mL 7.23 x 102 mL 2.33 x 102 mL 1.10 x 102 mL

	Which gas sample does not occupy a volume of 22.4L?   70.90 g of chlorine at 1.013 x 105 Pa and 273K 64.07 g of SO2 at 1.00 atm pressure and 0°C 16.05 g of CH4 at 760 mm Hg pressure and 273 K 1.00 mole of neon at 760 mm Hg pressure and O°F 83.80 g of krypton at 1.00 atm pressure and 32°F

	Which gas, based on molar mass, is in a 1.00 L tank if 2.03 g of the gas has a temperature of 12°C and a pressure of 1.29 x 103 mm Hg?   H C3H5Cl2 He C2H6O CO

	Which is not characteristic of gases?   They interact strongly with other gases in a mixture. The chemical identities of the gases in a mixture are irrelevant when considering their physical properties. They exert a pressure on the walls of their container. They are compressible. They will always form homogeneous mixtures.

	Which relationship is true at a constant temperature?   A more massive gas particle has a larger kinetic energy than a less massive gas particle. A more massive gas particle has a smaller kinetic energy than a less massive gas particle. A more massive gas particle has a lower average speed than a less massive gas particle. A more massive gas particle has the same average speed as a less massive gas particle. A more massive gas particle has a higher average speed than a less massive gas particle.

	Which relationship will produce a graph of a straight line?   volume versus pressure pressure versus 1/amount volume versus amount volume versus 1/amount volume versus 1/temperature(K)

	Which statement best describes the change in the distribution of molecular speeds as the temperature changes?   As the temperature decreases, the fraction of gas particles that have close to the average speed decreases. As the temperature decreases, the distribution curve broadens. As the temperature increases, the distribution curve remains unchanged. As the temperature increases, the distribution curve broadens. As the temperature increases, the fraction of gas particles that have values close to the average speed increases.

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