1. Define each of the following.
        a) pressure
        b) Boyle’s law
        c) Charles’s law
        d) Dalton’s law
        e) Graham’s law
        f) diffusion
        g) Avogadro’s law
        h) Ideal gas law
        i) R
        j) allotropes

2. What volume will one mole of a gas occupy at STP?

3. What happens to the total kinetic energy of a system when the gas molecules in the system collide?

4. If given several gases, how could you tell which one has the greatest density?

5. Standard pressure is equal to _______ atm, ________ kPa, ________ mm Hg, ________ torr, or ________ lb/in2.

6. What happens to gas molecules if they are heated under constant pressure? (Assume the container is expandable.)

7. If one gas has twice the mass of another gas and they are at the same temperature, under what conditions would their densities be the same?

8. Why does a confined gas exert pressure?

9. If given several gases and their temperatures, how can you tell which one has the highest kinetic energy?

10. Draw a graph relating volume of a given mass of an ideal gas to its Kelvin temperature at constant pressure.

11. Draw a graph relating pressure of a given mass of a gas to its volume at constant temperature.

12. What happens to the volume of a sample of gas originally at STP if the pressure decreases and the temperature increases?

13. What would happen to the pressure of a gas if it is heated in a rigid container?

14. When do deviations from ideal gas behavior become most significant?

15. Why does real gas behavior deviate from ideal gas behavior?

16. What happens to the temperature of a sample of a gas if the average kinetic energy of the molecules in the sample increases?

17. What property of gas molecules account for the fact that the volume of a confined gas can be decreased by the application of pressure at constant temperature?

18. What property of a mixture of gases is described by Dalton’s law?

19. When real gases do not behave exactly according to the predictions of the gas laws, what are they said to exhibit?

20. In an evaporating liquid substance, which molecules will leave the system first?

21. At a given temperature, how does the average kinetic energy of a liquid compare to the average kinetic energy of a gas?

22. What column length of mercury can the pressure of the atmosphere at sea level support?

23. At 21EC and 715 torr pressure, what will be the volume of 0.68 mole of CH₄(g)?

24. A gas occupies a volume of 368 mL at 29EC and 615 mm Hg pressure. Calculate the volume the gas would occupy at 198EC and 575 mm Hg pressure.

25. What are the relative rates of effusion of CH₄(g) and SO₂(g)?

26. A 398 mL sample of a gas is at a pressure of 635 mm Hg. What must be the pressure at constant temperature, if the volume is changed to 315 mL?

27. A 250 mL sample of chlorine, Cl₂, was collected over water at 25EC and 752 torr pressure. If the vapor pressure of water at 25EC is 23.8 torr, what would the volume of dry Cl₂ at STP be?

28. Given 2.99 mL of SO₂ gas at -18EC, what volume will the sulfur dioxide gas occupy at 29EC?