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10.107 Using the Gas Laws activity (eChapter 10.3), select a mass and a pressure to be held constant, and compare the volumes of N₂ and Xe at various temperatures. Under identical conditions—the same mass at the same pressure and temperature—are the volumes of N₂ and Xe equal? If not, explain why.

10.108 The P-V Relationships movie (eChapter 10.3) illustrates Boyle's law and points out that this law holds only when temperature is constant. (a) Reproduce the pressure versus volume graph presented in the movie. (b) Using the ideal-gas equation, deduce and superimpose on your graph from part (a) the line you would expect on the P-V plot at a temperature higher than the original and at a temperature lower than the original. (c) Do the same for the V versus 1/P plot.

10.109 Automobile air bags are inflated by the explosive decomposition of sodium azide, as shown in the Air Bags movie (eChapter 10.5). (a) If an air bag is to be inflated with 40.0 L of gas, initially at 110°C and 1.05 atm pressure, what mass of sodium azide must be available for decomposition? (b) What does the notation O(s) stand for in the decomposition reaction? (c) Why is it important that the reactants include an oxidant to react with the sodium metal produced by the decomposition?

10.110 Use the Density of Gases activity (eChapter 10.5) to compare the densities of two different gases at the same pressure and temperature. Explain in terms of kinetic-molecular theory why the molar mass of a gas is necessary to calculate the density of a gas, but not to determine its pressure.

10.111 The relative speeds of helium and neon atoms are shown in the Kinetic Energy in a Gas movie (eChapter 10.7). (a) If the average kinetic energies of both gases are the same at a given temperature, determine how much faster helium atoms are moving (on average) than neon atoms. (b) How does the fact that average kinetic energy of a gas is directly proportional to absolute temperature explain Boyle's observation that pressure decreases with increasing volume at constant temperature? (c) How does it explain Charles's observation that pressure increases with increasing temperature at constant volume?