Partial Pressure of Gases Using Moles

What Gas Law would you use to solve the following: A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. There are 2 moles of hydrogen, 5 moles of nitrogen, and 8 moles of water vapor. What is the partial pressure of the water vapor?

• Ideal Gas Law

• Combined Gas Law

• Dalton's Law

You have a gas that has a pressure of 2 ATM and a volume of 10L. What would be the new volume if the pressure was changed to 1 ATM?

• 5 L

• 20 L

• It would stay at 10L

• 1 L

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

• 2.00 atm

• 4.00 atm

• 3.00 atm

• 9.00 atm

What is the volume of 1 mole of a gas at STP?

• 62.3L

• 22.4L

• 0.04L

• 12.2L

A sample of hydrogen gas is collected over water at 25 °C and a pressure of 745.6 mmHg. What is the pressure of the dry hydrogen in mmHg?

• 722 mmHg

• 23.8mmHg

• 770mmHg

• 745mmHg

A gaseous mixture contains 5.0 moles of nitrogen and 10.0 moles of helium. The total pressure in the container is 3.0 atmospheres. What is the partial pressure of the nitrogen?

• 1 atm

• 0.5 atm

• 3.0 atm

• 2.0 atm

A sealed vessel contains 0.5 moles of oxygen, 0.1 moles of carbon dioxide, and 0.4 moles of nitrogen gas. The total pressure of the gas mixture is 5 atmospheres. What is the partial pressure of the carbon dioxide?

• 0.5 atm

• 2.5 atm

• 2.0 atm

• 0.1 atm

If two gases, A and B, in separate 1 liter containers exert pressures of 2 atm and 3 atm respectively, what will be the pressure exerted when both gases are put together in a 2 liter container?

• 5 atm

• 2.5 atm

• 10 atm

• 6 atm

Argon makes up 0.93% of the atmosphere. In a given sample of air, the partial pressure of argon is 6.54 mmHg. What is the pressure of the sample?

• 703 mmHg

• 70.3 mmHg

• 654 mmHg

• 760 mmHg

Which container will have a lower pressure?

• left

• right

• they both have the same pressure

• I don't know