# UNIT 10 REVIEW WORKSHEET

PART 1 - Completion

The   1   of the particles in a gas with the walls of the container    1. ______________________
results in gas   The total pressure in a mixture of gases is       2. ______________________
equal to the sum of the   3   of each gas present.
This is known    3. ______________________
as   4   law of partial pressures.                                                4. ______________________
The pressure and volume of a fixed mass of gas are   5   related.    5. ______________________
If one decreases, the other   This relationship is known as      6. ______________________
7   law.
The   8   of a fixed volume of gas is directly related to    7. ______________________
its   9   temperature.
The   10   of a gas at constant pressure is   8. ______________________
11   related to its Kelvin temperature.  This is known as   12        9. ______________________
law.
10. ______________________
These three separate gas laws can be written as a single             11. ______________________
expression called the   13  Another expression is the ideal gas    12. ______________________
law,   14  , where n =   15  .  The letter R is the   16   constant,   13. ______________________
and is equal to   17  .                                                             14. ______________________
15. ______________________
16.
______________________
17.
______________________

PART 2 - True or False (Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.)

___ 18. Halving the number of particles in a given volume of gas decreases the pressure by one-
half, if the temperature is kept constant.
___ 19. 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 the temperature is
kept constant.
___ 20. According to the Kinetic-Molecular theory, the particles of an ideal gas have no volume
and are not attracted to each other.
___ 21. Avogadro's hypothesis states that gases with the same size particles have equal volumes
at the same temperature and pressure.
___ 22. The proportionate pressure exerted by each gas in a mixture does not change as the
temperature, pressure, or volume changes.
___ 23. A balloon with a volume of 60 L at 100 kPa pressure will expand to a volume of 120 L at a
pressure of 50 kPa.
___ 24. Charles's law concerns a direct proportion between volume and Kelvin temperature and can
be represented on a graph as a straight line.
___ 25. According to the combined gas law, T2 = P1 x V2 x T1
P2 x V1
___ 26. The ideal gas law allows us to solve for the number of moles of a contained gas when
P, V, and T are known.

___ 27. When the effect of the volume of the molecules of gas dominates the effect of the
attraction between gas molecules, the ratio (P x V) / (R x T) is greater than one.

___ 28. The rate of diffusion of a gas is not influenced by its molar mass.

___ 29. When two bodies of different mass have the same kinetic energy, the lighter body moves
faster.

___ 30. In a mixture of Ar and CO, the Ar would diffuse at a faster rate.

PART 3 - Problems

31. A volume of 3.0 L of air is warmed from 50 oC to 100 oC.  What is the new volume if the
pressure remains constant?

32. 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 120 kPa.

33. A gas sample occupies 200 mL at 100 kPa.  What volume does the gas occupy at 53 kPa?

34. Nitrogen gas in a steel cylinder is under a pressure of 15,200 kPa at 27.0 oC.  What will the
pressure in the tank be if the tank is left in the sun and the internal temperature rises to 55 oC?

35. A sample of gas occupies a volume of 80 mL at a pressure of 0.50 atm and a temperature of 0
oC.  What will be its volume at a pressure of 1.50 atm and a temperature of 50 oC?

36. Compare the rates of effusion of H2 and CO2.

37. A 20.0 L container is filled with nitrogen gas at STP.  Then, 71 L of hydrogen gas is introduced
into the container, still at STP.  A spark is set off in the container and the container is cooled
at 0 oC.  If the reaction had gone to completion, what would the pressure in the container be?
N2  +  3 H2  -->  2 NH3