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Chapter 6
Gases
39. A sample of gas has a volume of 4.25L at
25.6°C and 748 mm Hg. What will the
volume of this gas be at 742 mm Hg and
26.8°C?
P
1
V
1
= P
2
V
2
T
1
T
2
V
2
= P
1
V
1
T
2
P
2
T
1
= 748 mm Hg x 4.25L x 299.95K
=
742 mm Hg x 298.75K
4.30L
41. A constantvolume vessel contains 12.5g
of a gas at 21°C. If the pressure of the gas
is to remain constant as the temperature of
the gas is raised to 210°C, how many grams
of gas must be released?
n
1
T
1
=PV
= n
2
T
2
R
n
1
T
1
= n
2
T
2
n
2
= T
1
n
1
T
2
= 294K
483K
= 0.609
n
2
= 0.609n
1
m
2
/MW = 0.609m
1
/MW
=0.609x12.5g = 7.609g 12.5g7.609g = 4.89g
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View Full Document43. A 12.8L cylinder contains 35.8g O
2
at 46°C.
What is the pressure of this gas in atmospheres
PV = nRT
P = nRT
V
= 35.8g/32.0g mol
1
x 0.08205L atm mol
1
K
1
x 319K
12.8L
= 2.29 atm
45. A 72.8L cylinder containing 1.85 mol He is
heated until the pressure reaches 3.50 atm. What
is the final temperature in degrees Celcius
PV = nRT
T = PV
nR
=
3.50 atm x 72.8L
1.85 mol x 0.08205L atm mol
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 Winter '10
 Lioudmila

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