AP Chemistry Gas Laws Practice!

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

• 1.5 atm

• 15 atm

• 0.67 atm

• 3.3 atm

• 7.5 atm

Which of the following would increase the (gas) pressure of a system?

• Increase the Temperature
• Pump in more gas
• Decrease the volume
• All of these

Tags

NGSS.HS-PS1-6

A container is filled with H₂, and H₂O. Calculate the partial pressure of H₂ when the pressure of water is 17torr. The total pressure of the gases is 750torr.

• 767.5torr
• 732torr
• 42.86torr

Tags

NGSS.HS-PS1-7

Which container will have lower pressure?

• left
• right
• they both have the same pressure

Pick the best answer to explain all properties of gases....

• They're fluids 
  Can be compressed
  Little space between particles 
• They're solids 
  Can be compressed
  Lots of space between particles 
• They're fluids 
  Cannot be compressed
  Lots of space between particles 
• They're fluids 
  Can be compressed
  Lots of space between particles 

A sample of gas with a volume of 30.0 mL at 25.0^oC is heated to 50.0^oC.  What is the new volume of the gas?

• 60.0 mL
• 15.0 mL
• 27.5 mL
• 32.5 mL

Tags

NGSS.HS-PS1-5

The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127^oC. What is the molar mass of this gas?

• (254/3) R

• 188 R

• (800/3) R

• 600 R

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

• 0.13 atm

• 0.27 atm

• 0.63 atm

• 0.90 atm

A flask contains 0.25 mole of SO₂(g), 0.50 mole of CH₄(g), and 0.50 mole of O₂(g). The total pressure of the gases in the flask is 800 mm Hg. What is the partial pressure of the SO₂(g) in the flask?

• 600 mm Hg

• 250 mm Hg

• 200 mm Hg

• 160 mm Hg

Under what conditions will a real gas most closely follow ideal gas behavior?

• high pressure and low temperature

• low pressure and low temperature

• low pressure and high temperature

• high pressure and high temperature