Gas Laws: Quantitative Analysis
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Boyle’s Law states that the volume (V) of a gas varies inversely with its pressure (P) if temperature is
constant. Boyle’s Formula: P1 x V1 = P2 x V2
1.
A 2.0 L sample of nitrogen has a pressure of 3.2 atm. What volume would be necessary to
decrease the pressure to 1.0 atm?
2. A sample of hydrogen gas decreases in pressure from 1.5 atm to 0.50 atm. If its final volume is
0.750L what would its original volume be?
3. Chlorine gas occupies a volume of 1.2 L at 0.947 atm pressure. What volume will it occupy at 1
atm pressure?
Charles’ Law states that the volume (V) of a gas varies directly with temperature (T), assuming that
pressure is constant. Charles’ Formula: V1/T1 = V2/T2
1.
A sample of nitrogen occupies a volume of 250 mL at 298 Kelvin. What volume will it occupy at
368 Kelvin?
2. If oxygen gas has a temperature of 313 Kelvin when it occupies a volume of 2.3 L what would its
temperature be if it occupies a volume of 6. 5 L?
3. Chlorine gas occupies a volume of 25 mL at 300 Kelvin. What volume will it occupy at 600
Kelvin?
Gay-Lussac Law states that pressure (P) of a gas varies directly with temperature (T) when volume is
constant. Gay-Lussac’s Formula: P1/T1 = P2/T2
1.
A sample of nitrogen gas has a pressure of 0.0650 atm at 539 Kelvin. If the volume does not
change, what will the pressure be at 211 Kelvin?
2. The pressure in a car tire is 1.95 atm at 300 Kelvin. After a long drive, the pressure increases to
2.22 atm. Calculate the temperature of the air in the tire after the drive?
3. The gas in a used aerosol can is at a pressure of 1.02 atm at 298 Kelvin. If the can is thrown into
a fire, what will the pressure be when the temperature reaches 1,201 Kelvin?
Combined Gas Law Formula: P1V1/ T1= P2V2/T2, where only the amount of gas (n) is held constant.
1.
A gas at 1.53 atm and 298 Kelvin has an initial volume of 1.00 L. The pressure of the gas
increases to 5.97atm as the temperature is raised to 398 Kelvin. What is the new volume?
2. A 5.00L air sample has a pressure of 1.06 atm at a temperature of 223 Kelvin. If the
temperature is raised to 375 Kelvin and the volume expands to 7.00 L, what will the new
pressure be?
Ideal Gas Law formula: PV = nRT, takes into consideration all four variables that affect the
properties of a gas: pressure (P), volume (V), amount of gas (n) in moles, and temperature(T).
R is the gas constant: 0.0821L-atm/mol-K
1.
How many moles of oxygen will occupy a volume of 2.5L at 1.2 atm and 298 Kelvin?
2. What volume will 2.0 moles of nitrogen occupy at 0.947 atm and 293 Kelvin?
3.
At what temperature will 5.00 grams of Cl2 exert a pressure of 1.18 atm at a volume of 0.750 L?