Gas Law Problems
At what temperature would 2.10 moles of N2 gas have a pressure of 1.25 atm and in a 25.0 L tank?
181 K
What is the total pressure of a gas mixture with these partial pressures: He = 2.3 atm, Kr = 6.3 atm, O2 = 0.23 atm.
8.83 atm
When the temperature of a gas is increased, will the volume increase or decrease?
Increase
What unit is used for temperature in the gas law equations?
Kelvin (K)
V1 / n1 = V2 / n2
Avogadro's Law
A sample of carbon dioxide occupies a volume of 3.50 liters at 1.23atm pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters?
2.15 atm
If the total pressure of a mixture of N2, He, CO2, and Kr is 13.2 atm and the partial pressures are N2 = 1.45 atm, He = 2.98 atm, and CO2 = 4.82 atm then what is the partial pressure of Kr?
3.95 atm
When the amount of gas (n) is increased, what happens to the volume?
It increases
What unit is used for volume in the gas law equations?
Liters (L)
P1 x V1 = P2 x V2
Boyle's Law
A 250.0 L sample of chlorine gas is collected when the barometric pressure is 1.04 atm. What is the volume of the sample after the barometer drops to 0.99 atm?
262.62 L
Using numbers, compare the rates of F2 and Cl2. How much quicker is F2 than Cl2?
F2 = 40.00 g/mol
Cl2 = 70.91 g/mol
1.33
When the pressure of a gas is decreased, what happens to the temperature?
It decreases
What unit is used for pressure in the gas law equations?
V1 / T1 = V2 / T2
Charles' Law
If a gas is cooled from 323.0 K to 273.15 K, what final pressure would result if the original pressure was 7.40 atm?
6.26 atm
Using numbers, compare the rates of effusion of Ne and CO. How much quicker is Ne than CO?
Ne = 20.16 g/mol
CO = 28.01 g/mol
1.18
Which will move faster: a heavy molecule or a light molecule?
Light
What unit is used for amount (n) in the gas law equations?
Moles (mol)
P1 / T1 = P2 / T2
A student collects 125.0 L of hydrogen. Later, the sample is found to have a volume of 128.6 L at a temperature of 26° C. At what temperature in Kelvin was the hydrogen collected?
291 K
An unknown gas is 3.10 times faster than H2. What is the molar mass of the unknown gas?
CO2 = 44.01 g/mol
4.57 g/mol
When a gas is compressed (when the volume goes down), what is happening to the pressure inside its container?
It is increasing
What unit is used for molar mass in the Graham's Law equation?
grams/mole (g/mol)
PV=nRT
Ideal Gas Law