Bellwork 1 Week 4 4th Nine Weeks

If the pressure exerted by a gas at 298 K in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?

• P1/T1 = P2/T2
• PV = nRT
• V1/n1 = V2/n2
• P1V1 = P2V2

A gas fills a balloon at a temperature of 27 ^oC and 1 atm of pressure. What will the pressure of the balloon be if the gas is heated to 127 ^oC?

• P1V1 = P2V2
• PV = nRT
• P1/T1 = P2/T2
• V1/T1 = V2/T2

A 220.0 mL sample of helium gas is in a cylinder at 105 kPa and 275 K. The piston is pushed in until the sample has a new temperature of 310 K and new pressure of 150 kPa. What is the new volume of the gas? 

• P1V1/T1 = P2V2/T2
• PV = nRT
• P1V1 = P2V2
• Pt = P1 + P2 + P3 + ...

A container has 0.504 moles of a gas at a volume of 2680 mL.  When the number of moles changes to 0.423 moles, what is the new volume?

• PV = nRT
• V1/n1 = V2/n2
• P1V1/T1 = P2V2/T2
• P1V1 = P2V2

If the total pressure is 0.99 atm, and the partial pressure of carbon dioxide and hydrogen sulfide is 0.05 atm and 0.02 atm respectively.  What will be the partial pressure of the remaining air?

• P1V1 = P2V2
• Pt = P1 + P2 + P3 + ...
• PV = nRT
• P1/T1 = P2/T2

Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 

• 0 K 
• 107 K 
• 207 K 
• 307 K 

What is 50 °C in Kelvin?

• 223
• 323
• 100
• 50

If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be

• 250 mL
• 204 mL
• 196 mL
• 160 mL

What will happen to the volume of a gas under constant temperature if the pressure increases?

• Increase
• Decrease
• Nothing
• Explosion!

The following graph shows ____ relationship. 

• Direct
• Inverse