Gases Chemistry Worksheet - Chapter 13, An Introduction To Chemistry Page 17

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13.2 Ideal Gas Calculations
If such a change is anticipated, car designers and mechanics, such as Lilia’s brother Ted,
can make adjustments. For example, because of its altitude, Denver has about 15%
lower air density than does a city at sea level. Therefore, Indy cars that race in Denver
are fitted with larger-than-normal brakes to compensate for the lower air resistance
and greater difficulty stopping. Ted can do calculations similar to Example 13.3 to
determine the density of air on different days and at different racetracks. An example
is the following set of equations calculating the density of air at 762 mmHg and
32 °C and at 758 mmHg and 4 °C. (The average molar mass for the gases in air is 29
g/mol.)
g
PV =
RT
M
O
17
29 g
bjeCtive
762 mmHg
g
PM
1 atm
1 mol
=
=
= 1.2 g/L
V
RT
760 mmHg
0.082058 L atm
305 K
K mol
29 g
758 mmHg
g
PM
1 atm
1 mol
= 1.3 g/L
=
=
V
RT
760 mmHg
0.082058 L atm
277 K
K mol
You can read about why the measured, real properties differ from the
properties calculated from the ideal gas equation at the textbook’s Web site.
e
13.1 - Using the Ideal Gas Equation
xerCise
Krypton gas does a better job than argon of slowing the evaporation of the tungsten
O
15
bjeCtive
O
16
bjeCtive
filament in an incandescent light bulb. Because of its higher cost, however, krypton is
O
17
bjeCtive
only used when longer life is considered to be worth the extra expense.
a. How many moles of krypton gas must be added to a 175-mL incandescent
light bulb to yield a gas pressure of 117 kPa at 21.6 °C?
b. What is the volume of an incandescent light bulb that contains 1.196 g Kr
at a pressure of 1.70 atm and a temperature of 97 °C?
c. What is the density of krypton gas at 18.2 °C and 762 mmHg?

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