<p>Chapter 14 Review Sheet Name ______</p><p>A. True and False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.</p><p>____ 1. Halving the number of particles in a given volume of gas decreases the pressure by one-half, if temperature is kept constant. ____ 2. Reducing the volume of a container of gas by one-half has the same effect on pressure as reducing the quantity of the gas in the container by one-half, if temperature is kept constant. ____ 3. According to kinetic theory, the particles of an ideal gas have no volume and are not attracted to each other. ____ 4. Gas pressure depends on the number and kind of gas particles in a given volume and on their average kinetic energy. ____ 5. The proportionate pressure exerted by each gas in a mixture does not change as the temperature, pressure, or volume changes. ____ 6. A balloon with a volume of 60 L at 1 atm pressure will expand to a volume of 120L at a pressure of 0.5 atm. ____ 7. Charles’ law concerns a direct proportion between volume and Kelvin temperature and can be represented on a graph as a straight line.</p><p>____ 8. According to the combined gas law, T2 = Pl x V2 x T1 P2 x V1 ____ 9. The ideal gas law allows us to solve for the number of moles of a contained gas when P, V, and T are known.</p><p>B. Problems Solve the following problems in the space provided. Show your work. 10. A volume of 3.0 L of air is warmed from 50°C to 100°C . What is the new volume if the pressure remains constant?</p><p>11. What is the temperature of the gas inside a 750 mL balloon filled with 0.030 g H2 gas? The pressure of the balloon is 1.2 atm.</p><p>12- A gas sample occupies 200 mL at 760 mm Hg. What volume does the gas occupy at 400 mm Hg?</p><p>13. Nitrogen gas in a steel cylinder is under a pressure of 150 atm at 27°C. What will the pressure in the tank be if the tank is left in the sun and the internal temperature rises to 55°C? 14. Determine the total pressure of a gas mixture that contains CO, Ne, and He if the partial pressures of the gases are PCO = 1.53 atm, PNe = 0.82 atm, and PHe = 0.34 atm.</p><p>15. A mass of air occupies a volume of 5.7 L at a pressure of 0.52 atm. What is the new pressure if the same mass of air at the same temperature is transferred to a 2.0 L container?</p><p>16. A volume of 20.0 L of O2 is warmed from-30.0°C to 85.0°C. What is the new volume, if the pressure is kept constant?</p><p>17. A rigid container holds a gas at a pressure of 0.55 atm at a temperature of -100°C. What will the pressure be when the temperature is increased to 200°C?</p><p>18. What is the volume at STP of a sample of CO2 that has a volume of 75.0 mL at 30.0°C and 680 mm Hg?</p><p>19. What is the volume of a sample of O2 that has a mass of 50.0 g and is under a pressure of 1.20 atm at 27.0°C?</p><p>20. A sample of gas occupies a volume of 80 mL at a pressure of 0.50 atm and a temperature of 0°C What will be its volume at a pressure of 1.50 atm and a temperature of 50°C?</p><p>21. A 20.0 g nitrogen gas and 7.10 g of hydrogen gas is introduced into a 3.00 L container at 25°C. A spark is set off in the container and the container is cooled to 25°C . The equation is N2(g) + 3H2(g)  2NH3(g) A. What was the pressure in the container before the reaction in atm?</p><p>B. What was the pressure in the container after the reaction, in atm?</p>