If the pressure of 1.50 L of hydrogen gas at 100°C decreases from 0.500 atm to 0.115 atm, what is the final volume? Assume temperature remains constant.

A sample of gas has an initial volume of 5.6 L at a pressure of 735 mmHg. If the volume of the gas is increased to 9.4 L, what is its pressure, assuming temperature and amount of gas remain constant?

A sample of nitrogen gas has a pressure of 986 torr at 186°C. Assuming the volume and amount of gas remain constant, at what temperature in °C will the sample of gas have a pressure of 685 torr?

Consider 4.20 L of a gas at 365 mmHg and 20°C. If the container is compressed to 3.00 L and the temperature is increased to 36°C, what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside.

Which of the following equations represents Boyle's Law?

In an underground gas reserve, a bubble of methane gas (CH₄) has a volume of 45.0 mL at 1.60 atm pressure. What volume, in milliliters, will the gas bubble occupy when it reaches the surface where the atmospheric pressure is 744 mmHg, if there is no change in temperature?

Which of the following correctly describes the relationship between variables in Boyle's Law?

What was the original temperature of a gas, in °C, if the volume changed from 1.00 L to 1.10 L and the final temperature was 255.0 °C, assuming constant pressure?