1. At a temperature of __________ °C, 0.444 mol of CO gas occupies 11.8 L at 889 torr.

2. In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is __________ ifthe partial pressures of He and Ne are 1.50 and 2.00 atm, respectively.

3. The amount of gas that occupies 60.82 L at 31 °C and 367 mmHg is __________ mol.

4. A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was __________ atm.

5. Which of the following is not part of the kinetic-molecular theory?

6. A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121 °C while maintaining the pressure at 629 torr.

7. A gas at a pressure of 325 torr exerts a force of __________ N on an area of 5.5 m² .

8. The pressure of a sample of CH₄ gas (6.022 g) in a 30.0 L vessel at 402 K is __________ atm.

9. A sample of an unknown volatile liquid was injected into a Dumas flask (mflask = 27.0928 g, Vflask = 01040 L) and heated until no visible traces of the liquid could be found. The flask and its contents were then rapidly cooled and reweighed (mflask + vapor = 27.4593 g) The atmospheric pressure and temperature during the experiment were 0.976 atm and 18.0 °C, respectively. The unknown volatile liquid was __________.

10. The National Weather Service routinely supplies atmospheric pressure data to help pilots set their altimeters. The units the NWS uses for atmospheric pressure are inches of mercury. A barometric pressure of 30.51 inches of mercury corresponds to __________ kPa.

11. A sample of O₂ gas (2.0 mmol) effused through a pinhole in 5.0 s. It will take __________ s for the same amount of CO₂ to effuse under the same conditions.

12. In ideal gas equation calculations, expressing pressure in Pascals (Pa), necessitates the use of the gas constant, R, equal to __________.

13. A closed-end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mmHg. The pressure of the argon in the container was __________ mmHg.

14. The molecular weight of a gas that has a density of 6.70 g/L at STP is __________ g/mol.

15. Which statement about ideal behavior of gases is false?

16. A sample of He gas (2.0 mmol) effused through a pinhole in 53 s. The same amount of an unknown gas, underthe same conditions, effused through the pinhole in 248 s. The molecular mass of the unknown gas is __________ g/mol.

17. The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation:
Cl₂ (g) + C₂H₄ (g) . C₂H₄Cl₂ (g) will produce a total of __________ mL of products if pressure and temperature are kept constant.

18. A mixture of carbon dioxide and an unknown gas was allowed to effuse from a container. The carbon dioxide took 1.25 times as long to escape as the unknown gas. Which one could be the unknown gas?

19. A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of gas. If the partial pressureof Ne is 2.75 atm, how many moles of Ar are in the mixture?

20. A sample of H₂ gas (2.0 L) at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm.

21. The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP?

22. A real gas will behave most like an ideal gas under conditions of __________.

23. The root-mean-square speed of CO at 113 °C is __________ m/s.

24. The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is __________ mmHg.

25. A sample of gas (1.3 mol) occupies __________ L at 22 °C and 2.5 atm.