Unit 2: Gases Review

With pressure, volume, and temperature being known values, the ideal gas law can be used to 

• calculate the chemical formula
• calculate the density
• calculate the kinetic energy
• calculate the number of moles

At a constant pressure, the volume decreases.  What happens to the temperature?

• increases
• decreases
• stays the same

At a constant volume, the pressure increases.  What happens to the temperature?

• increases
• decreases
• stays the same

At a constant temperature, the volume decreases.  What happens to the pressure?

• increases
• decreases
• stays the same

Calculate the volume that a 0.323-mol sample of a gas will occupy at -8^oC and a pressure of 0.900 atm.

• 7.18 L 
• 7.81 L
• 4.63 L
• 4.36 L

A hot air balloon uses heat to inflate the balloon. What two variables does this relate?

• Pressure and Volume

• Volume and Temperature

• Temperature, Volume, and Pressure

• Temperature and amount of gas

Convert -53 ⁰C to K

• 326 K
• -53 K
• 220 K
• Probably impossible.

Which of the following would increase the pressure on a system?

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

___________________ is a measure of the average kinetic energy of particles.

• Volume

• Pressure

• Moles

• Temperature

What pressure is exerted by 2.50 L of gas containing 1.35 mol at 47 ^oC? Which equation is best to use to solve the problem?

• PV=nRT

• Stoichiometry Gas Conversion

• P_{T =} P₁ + P₂ + P₃ + ....

• P₁V₁ = P₂V₂

  n₁T₁ = n₂T₂