Ideal Gas Law Review

In the Ideal Gas Law, choose the correct definition to the variable (multiple answers)

• R = number of moles of a gas

• R = Gas constant

• n = Number of moles of a gas

• n = Gas constant

A balloon containing 150 L of gas at 52°C and 101.3 kPa rises to an altitude where the pressure is 62.1 kPa and the temperature is -20°C.  What would the volume become at this new altitude?

• 165.25 Liters

• 189.91 Liters

• 196.02 Liters

• 178.63 Liters

Which of the following are correct gas constants?

• 0.0821 (atm)

• 8.314 (kPa)

• 0.0821 (kPa)

• 8.314 (atm)

If 2.4 L of gas is at a pressure of 387 kPa, what would the pressure be if the volume was expanded to 29.8 L?

• 62.34 kPa

• 31.17 kPa

• 41.86 kPa

• 25.52 kPa

A rigid container of oxygen gas has a pressure of 180 kPa at a temperature of 351 K.  What is the pressure at 193 K?

• 98.97 kPa

• 120.82 kPa

• 72.65 kPa

• 82.15 kPa

How many moles of nitrogen gas are in a flask with a volume of 24 L at a pressure of 320 kPa and a temperature of 87°C?

• 4.75 moles

• 1.04 moles

• 3.92 moles

• 2.57 moles

A balloon has a volume of 43.6 L at 310 K.  What is the temperature of the balloon if the volume is decreased to 27.8 L?

• 310 kelvin

• -76 celsius

• 197.66 kelvin

• 37 celsius

What does the ideal gas law allow you to calculate that the other gas laws do not?

• number of moles

• pressure

• volume

• temperature

Why does the pressure inside a container of gas increase if more gas is added to the container?

• There is an increase in the number of collisions between particles and the walls of the container.

• There is an increase in the temperature of the gas.

• There is a decrease in the volume of the gas.

• There is an increase in the force of the collisions between the particles and the walls of the

  container.

A gas that follows laws at all temperatures and pressures

• barometer

• pressure

• ideal gas

• effusion