Unit 10—Gases
Name
Pre-AP Chemistry: Worksheet #4—Ideal Gas Law
Period
Date
1.
What did Avogadro assume to be true about equal volumes of gases? What conditions must
be met for his assumption to be true?
2.
Write the ideal gas law equation, identifying each variable and constant.
3.
How many moles of a gas will occupy 58.9 L at a temperature of 455 K and a pressure of 32.4
kPa?
4.
Find the pressure, in atm, exerted by 3.50 moles of neon gas filling a 2.78 L container at a
temperature of 490 K.
5.
At what temperature will 1.24 moles of hydrogen fill a 10.0 L vessel at standard pressure? If
the pressure is then reduced to 79.8 kPa, what will the new temperature be? Which gas law(s)
did you use?
6.
What is the molar mass of a 1.25 g sample of gas that occupies a volume of 1.00 L at a
pressure of 0.961 atm and a temperature of 27.0°C?
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Unit 10—Gases
7.
Determine the density of argon gas under the following conditions.
a.
STP
b.
pressure of 551 torr and a temperature of 25°C
8.
The density of a gas was found to be 2.0 g/L at 1.50 atm and 27°C. What is the molar mass of
the gas?
9.
Iron reacts with hydrochloric acid to produce iron (II) chloride and hydrogen gas. The
hydrogen gas from the reaction of 1.0 g of iron with excess hydrochloric acid is collected in a
15.0 L flask at 25C. What is the pressure, in atm, of the hydrogen gas in this flask?
10.
Sodium azide (NaN3), the explosive compound in automobile air bags decomposes to form
solid sodium and nitrogen gas. What mass of sodium azide is required to inflate a 25.0 L bag
to a pressure of 1.3 atm at 25C?
11.
Tungsten, W, a metal used in light-bulb filaments, is produced industrially by the reaction of
tungsten oxide with hydrogen.
WO3(s) + 3H2(g) → W(s) + 3H2O(l)
How many liters of hydrogen gas at 35°C and 0.980 atm are needed to react completely with
875 g of tungsten oxide?
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Unit 10—Gases
12.
What volume of chlorine gas at 38°C and 1.63 atm is needed to react completely with 10.4 g of
sodium to form NaCl?
13.
How many liters of gaseous carbon monoxide at 27°C and 0.247 atm can be produced from
the burning of 65.5 g of carbon according to the following equation?
2C(s) + O2(g) → 2CO(g)
14.
What volume of oxygen gas in liters can be collected at 0.987 atm pressure and 25.0°C when
30.6 g of KClO3 decompose by heating, according to the following equation?
2KClO3(s) → 2KCl(s) + 3O2(g)
15.
Gaseous ammonia is synthesized from nitrogen and hydrogen. Assume that you take 355 L of
hydrogen gas at 25.0C and 542 mm Hg and combine it with excess nitrogen gas. What is the
theoretical yield of ammonia gas in moles? If this amount of ammonia gas occupies a 125 L
tank at 25.0C, what is its pressure in atm?
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