Worksheet: Boyle's Law
In this worksheet, we will practice using the formula PV = constant (Boyle's law) to calculate the pressure or volume of a gas that is allowed to expand or contract at a constant temperature.
At sea level on Earth, the atmospheric air pressure is about 101 kPa. At the top of Mount Everest, the air pressure is about 34 kPa. A balloon with a fixed amount of helium gas is taken from sea level up to the top of Mount Everest. The temperature of the air is the same at both locations. What happens to the size of the balloon?
- AIt decreases.
- BIt increases.
- CIt remains the same.
For a gas at a constant temperature, if the volume is , then the pressure .
- Aincreased, stays the same
- Bdecreased, stays the same
- Cincreased, decreases
- Dincreased, increases
- Edecreased, decreases
A gas in a sealed container is kept at a constant volume. The temperature of the gas is increased. What happens to the pressure of the gas?
- AIt increases.
- BIt decreases.
- CIt stays the same.
A gas with a volume of 3 m3 is at a pressure of 500 Pa. The gas is compressed at a constant temperature until it is at a pressure of Pa. What is the volume of the gas after it is compressed?
A gas with a volume of 2 m3 is at a pressure of 500 Pa. The gas is compressed at a constant temperature to a volume of 0.5 m3. What is the pressure of the gas after it is compressed?
Which of the following is the correct formula for Boyle’s law, where is the pressure of a gas, is the volume, is the temperature, and is a constant?
A gas initially has a pressure of 800 Pa and a volume of 2 m3. It is compressed at a constant temperature until its volume is half its initial value. At this point it has a pressure . It is then allowed to expand again until the pressure is . What is the final volume of the gas?