Gas Law 1 DOL

Which gas law equation would you use to solve the problem below?

If I have 45 liters of helium in a balloon at 25⁰ C and increase the temperature of the balloon to 55⁰ C, what will the new volume of the balloon be?

• P1V1=P2V2

• PV=nRT

• V1T1=V2T2

• V1/T1=V2/T2

Which gas law equation would you use to solve the problem below?

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

For his chemistry demonstration, Davy filled up a 5 L balloon with nitrous oxide gas at 25°C and an atmospheric pressure of 1.08 atm. For easier transportation he stored it in a pressurized container at 1.5 atm and temperature of 5°C. What volume will the balloon have?

• 9.77 L
• 3.36 L
• 7.56 L
• 4.35 L

A gas has a pressure of 1.50 atm at a temperature of 273 K.  What will be the pressure at 410 K?

• .99 atm
• 2.25 atm
• .75 atm
• 2.5 atm

Charles's law states that:

• Equal amounts of gases occupy the same volume at constant temperature and pressure.

• The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

• The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

• The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

• The rates of effusion of gases are inversely proportional to the square roots of their molar masses.