AP ChemistryName :

Worksheet : Ch. 5 and 10 : Obj. 1-20Date :

  1. Read Ch. 5 and answer the following questions (Show all work):
  1. Gas ______is the collective result of gas particles striking an object or the walls of a container.
  1. A ______is a device made of an evacuated glass tube inverted into a pool of mercury used to measure air pressure.
  1. A ______is another device used to measure air pressure and consists of an "s" shaped tube containing mercury and an evacuated vessel.
  1. Name and compare the values of four units used to measure air pressure.
  1. State Boyle's law and give the mathematical equation for Boyle's law.

6. _____ (T/F) Boyle's law indicates an inverse relationship between gas pressure and gas volume at varying temperatures.

7. _____ (T/F) A plot of volume vs 1/P at a constant temperature will produce a straight line according to Boyle's law.

8. _____ (T/F) Boyle’s law is precise at all temperatures.

9. ______gases strictly obey Boyle’s law (and the other gas laws) at all temperature and pressure conditions.

10. Which of the following graphs show a plot of V vs 1/p? ______


  1. b.
  1. Freon is a gas that is used in air conditioners. If a 1.3 L sample of freon in an air conditioner(at 1 672 torr) escapes into an atmosphere with a pressure of 758 torr, what will the new volume of the freon be? (Assume temperature will be held constant).(Ans. 2.9L)

12. State Charles’ law and give the mathematical equation for Charles’ law.

13. _____ (T/F) The Kelvin scale must always be used in gas laws.

14. A sample of a gas has a volume of 2.2L at 22.0 ºC and 1.2 atm. What will the volume be at 32.0 ºC and 1.2 atm?(Ans. : 2.3L)

15. _____ (T/F) If a plot of V vs T (in K) is extrapolated to zero volume the temperature would be O K (absolute zero).

16. State Avogadro's law and give the mathematical expression for Avogadro's law.

17. In the Haber process gaseous hydrogen and nitrogen are combined to form ammonia. If a 5.50 L volume of hydrogen gas and nitrogen gas are combined(in the correct stoichiometric ratio), what would the resulting volume of ammonia be (assume constant T and P). Balanced equation : 3 H2(g) + N2(g)  2 NH3(g) (Ans. : 2.75 L)

  1. Give mathematical expression for the ideal gas law(include the value if the ideal gas constant).

19. Use the ideal gas law to solve this problem : A reaction vessel with a volume of 55.0 L is used to generate 8.00 moles of oxygen gas. The pressure needs to be maintained at 5.0 atm. What temperature will the reaction vessel need to be at? (Ans. : 420 K)

  1. Use an ideal gas law derivation to solve this problem : A sample of nitrogen gas has a volume of 2.50 L and a temperature of 20.0 ºC. If the pressure is held constant, what will the temperature be if the gas volume changes to 3.00L? (ans. : 352 K)
  1. Use the ideal gas law to solve this problem : A sample of chlorine gas , at a pressure of 100.0 torr and a temperature of 30.0 ºC has a volume of 2.24L. If the pressure changes to 150.0 torr and the temperature changes to 35.0 ºC, what will the new volume be? (ans. : 1.52 L)
  1. ______(to 4 sig. Fig.) is the volume of one mole of any gas at STP (standard temperature and pressure).
  1. What are standard temperature and pressure conditions?
  1. A sample of oxygen gas has a mass of 48.0 g. What is the volume of this gas at STP? (ans. : 33.6 L)
  1. What volume of ammonia would be produced (at STP) if 2.3 g of hydrogen combined with an excess of nitrogen? (See no. 17 above). (ans. : 17 L)
  1. A sample of acetylene gas (C2H2) has a volume of .50 L at a temperature of 20.0 ºC and a pressure of 755 mmHg. This is mixed with a .50 L volume of oxygen gas which has a temperature of 15.0 ºC at a pressure of 762 mmHg. When the mixture is combusted, what volume of carbon dioxide will be formed at a pressure of 1.10 atm and a temperature of 112 ºC? (see pr. 5.13). (ans. : .49L)
  1. A gas has a density of 1.32 g/L at a temperature of 102 ºC and a pressure of 818 mm Hg. Calculate the molar mass of the gas. (ans. 37.6 g/mol)

28. _____ (T/F) According to the kinetic molecular theory (KMT), the identity, or composition, of an ideal gas will affect the pressure exerted by that gas.

29. _____ (T/F) According to the KMT, the gas particles make up a significant portion of the volume of an ideal gas.

30. _____ (T/F) According to the KMT, the forces between gas particles play a significant role in the behavior of ideal gases.

31. State Dalton's law of partial pressures and give its mathematical formula.

32. At 0 ºC a 1.0 L flask contains 5.0 x 10-2 mol N2, 1.5 x 102 mg O2 and 5.0 x 1021 molecules NH3. What is the partial pressure of each gas, and what is the total pressure in the flask? (see pr. 5.15 - calc moles O2 and NH3 then go to 2nd part - since you already know moles). (ans. : PN2 = 1.1 atm, PO2 = .11 atm, PNH3 = .19 atm, Ptotal = 1.4 atm)

33. The partial pressure of nitrogen in air with an atmospheric pressure of 762 mm Hg is 595 mm Hg. What is the mole fraction of N2? (See. Pr. 5.16)(ans. : .781)

34. The mole fraction of oxygen in the same atmosphere (Ptotal = 762 mm Hg) is .201. What is the partial pressure of O2 in this atmosphere? (See pr. 5.17)(ans. 153 mm Hg)

35. _____ (T/F) If a pure gas is collected by water displacement, the total gas pressure in the collecting vessel will be due to the gas collected.

36. A sample of oxygen gas is collected over water at 25.0 ºC and at a total pressure of 641 torr. The volume of the gas collected is 500.0 mL. What mass of oxygen is collected? (At 25.0 ºC the vapor pressure of water is 23.8 torr). (see pr. 5.18)(1 atm = 760 torr ; K = ºC + 273.15) (ans. .531 g)