4th Summative Test in Science 10

A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is increased to 60.0 mmHg at constant temperature?

• 9.2 L
• 8.2 L
• 7.2 L
• 10.2 L

A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L?

• 0.69 atm
• 0.67 atm
• 0.64 atm
• 0.66 atm

Imagine that a gas occupies a volume of 2.0 L at a temperature of 27°C. To what temperature in Kelvin scale must the gas be cooled to reduce its volume to 1.5 L if the pressure is held constant?

• 225K
• 325K
• 300K
• 250K

Imagine that you are skiing on a beautiful, clear day with a temperature outside of -3°C. The cold air that you breathe is warmed to a body temperature of 37°C as it travels to your lungs. If you inhale 425 mL of air at -3°C, what volume does it occupy in your lungs? (Assume that the pressure is constant.)

• 588.96 mL
• 599.96 mL
• 487.96 mL
• 432.96 mL

If the pressure of a confined gas is doubled while the temperature remains constant, what change would be observed in the volume?

• It would be half as large
• It would be doubled.
• It would be four times as large.
• It would remain the same.

Refer to the table below Based on the table, what relationship can be derived between pressure (P) and volume (V) at constant temperature?

• The volume is directly proportional to its pressure
• The volume is insignificantly related to its pressure.
• The volume is inversely proportional to its pressure.
• The volume is inversely proportional to the square of its pressure.

Which of the following properties does not describe a gas?

• Malleability
• Pressure
• Temperature
• Volume

Which of the items below is an application of Charles’s Law?

• Incubator
• Syringe
• Medical Respirator
• Automobile Engine

What property of gas molecule varies directly according to the kinetic molecular theory?

• Temperature
• Pressure
• Volume
• Volume And Pressure

Which of the following causes gas pressure?

• Gas molecules heating up.
• Gas molecules knocking other gas molecules.
• Gas molecules hitting the walls of a container.
• Gas molecules bonding with other gas molecules.