PART 1 - Completion

The __
1 __ of the particles in a gas with the walls of the
container 1. ______________________

results in gas __ 2 . __ 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 __ 6 . __ 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, T_{2}
= __P___{1}__ x V___{2}__ x T___{1}__
__
P

___ 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 ^{o}C to 100 ^{o}C. 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 ^{o}C. What will the

pressure in the tank be if the tank is left in the sun
and the internal temperature rises to 55 ^{o}C?

35. A sample of gas
occupies a volume of 80 mL at a pressure of 0.50 atm and a temperature of 0

^{o}C. What
will be its volume at a pressure of 1.50 atm and a
temperature of 50 ^{o}C?

36. Compare the rates of
effusion of H_{2} and CO_{2}.

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 ^{o}C. If
the reaction had gone to completion, what would the pressure in the container
be?

N_{2} + 3 H_{2}
--> 2 NH_{3}

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