WorksheetsGas Laws
Total questions: 20
Worksheet time: 33mins
If the pressure of a gas starts out at 200 kPa and increases to 600kPa, what would the initial temperature be if it ended up at 300K?
[P1V1 / T1 = P2V2 / T2]
50K
200K
400K
100K
Calculate the volume that a 0.323 mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
Remember: PV = nRT; R = 0.082 atm⋅L/mol⋅K and 8.314 kPa⋅L/mol⋅K
7.18 L
7.81 L
4.63 L
4.36 L
You have a gas that has a pressure of 2 atm and a volume of 10 L. What would be the new volume if the pressure was changed to 1 atm?
[P1V1 / T1 = P2V2 / T2]
5 L
20 L
It would stay at 10L
1 L
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?
[P1V1 / T1 = P2V2 / T2]
60.0 mL
15.0 mL
27.5 mL
32.5 mL
Determine the number of moles in a container of gas at a temperature of 273 K and a pressure of 1 atm with a volume of 99.2 L.
Remember: PV = nRT; R = 0.082 atm⋅L/mol⋅K and 8.314 kPa⋅L/mol⋅K
2222.08 moles
4.43 moles
22.4 moles
76.8 moles
If a gas is measured to have a volume of 0.5 atm at 273 K, what would happen to the pressure if the temp increased to 300 K?
[P1V1 / T1 = P2V2 / T2]
increase
decrease
remain the same
A balloon is filled with 1.9 moles of helium at 45°C. What would happen to the pressure in the balloon if 0.2 moles of He are removed at the same pressure?
increase
decrease
remain the same
If I have an unknown quantity of oxygen gas at a pressure of 880 mmHg, a volume of 41 liters, and a temperature of 67 0C, how many moles of gas do I have? Grams of gas?
3.4 mol, 27.27 g
3.4 mol, 54.55 g
1.7 mol, 54.55 g
1.7 mol, 27.27 g
If there is 5 moles of gas in a container with a volume of 65 liters and at a temperature of 560 K, what is the pressure inside the container?
3.5 atm
4.0 atm
2.5 atm
2.0 atm
If I have 4.3 moles of gas at a pressure of 0.09 atm and at a temperature of 325 K, what is the volume of the container that the gas is in?
1273.121 L
1280 L
1274209.44 L
1274.21 L
A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.50 atm, 3.50 atm, and 3.00 atm, respectively. What is the total pressure inside the container?
8.5 atm
9.5 atm
9 atm
8 atm
A sample of carbon monoxide initially at 29.0 °C was heated to 58.0°C. If the volume of the carbon monoxide sample is 816.5 mL at 58.0 °C , what was its volume at 29.0 °C?
745 mL
744.96 mL
744.964 mL
744.9637 mL
A gas cylinder contains 2.35 mol He, 2.25 mol Ne, and 1.55 mol Ar. If the total pressure in the cylinder is 2450 mmHg, what is the partial pressure of each of the components? Assume constant temperature.
A gaseous mixture contains 445.0 Torr H2(g), 338.1 Torr N2(g), and 65.7 Torr Ar(g). Calculate the mole fraction, 𝜒, of each of these gases.
A gas sample is collected in a 0.265 L container at 0.945 atm and 297 K. The sample is found to have a mass of 0.308 g.
What is the identity of the gas?
CH4
HCl
NO
CO
If 22.5 mol of an ideal gas is at 5.97 atm at 97.30 ∘C, what is the volume of the gas?
113.50 L
113 L
114.50 L
114.52 L
For a fixed amount of gas at a fixed temperature, what will happen if the volume is doubled?
The pressure exerted by the gas will not change.
The pressure exerted by the gas will halve.
The pressure exerted by the gas will double.
The pressure exerted by the gas will quadruple.
