Gas Laws and Properties

According to the gas laws, what happens to the pressure of a gas if its volume is decreased at constant temperature and number of moles?

A container of gas is heated while maintaining a constant volume. How does this affect the pressure of the gas inside the container?

A balloon is taken from a warm room to the outside on a cold winter day. What happens to the volume of the balloon, assuming the pressure remains constant?

What does Dalton's Law of Partial Pressures state?

According to the ideal gas law, which factor is directly proportional to the number of moles (n) of a gas, assuming pressure and temperature are constant?

If 2.0 moles of gas are added to a container already holding 1.0 moles of gas, how will the pressure change if the volume and temperature are kept constant?

A gas is compressed to half of its original volume and its temperature is doubled. By what factor does the pressure change?

What is the standard temperature in Kelvin that is used in gas law calculations?

A container with a fixed volume has gas at a pressure of 2 atm at 27C. If the temperature is raised to 227C, what is the new pressure?

A sample of gas occupies 10.0 L at standard temperature and pressure (STP). If the amount of gas is doubled, what is the new volume, assuming temperature and pressure remain constant?

What units are used to express the Ideal Gas Law Constant (R)?

If a gas is removed from a container with a fixed volume, what happens to the gas pressure inside the container?

Given $P_1 = 830.26$ kPa, $V_1 = 9.357$ L, and $P_2 = 7.6978$ atm. What is $V_2$ in liters, according to Boyle's Law?

A sample of C4H10 occupies 79.466 L, experiencing a change in pressure from 118.22 kPa to 4.7353 atm. What is the new volume in liters?

According to Charles's law, if a sample of radon changes in volume from 99.565 L to 90.06 L and the initial temperature is 468.61C, what is the final temperature in degrees Celsius?

A gas occupies a volume of 10.0 L at 273 K and 1 atm. If the temperature is increased to 546 K and the pressure is increased to 2 atm, what is the new volume of the gas?

A closed container of fixed volume contains a mixture of nitrogen and oxygen gas. If the partial pressure of nitrogen is 60 kPa and the total pressure inside the container is 101.3 kPa, what is the partial pressure of the oxygen gas?

What would happen to the average kinetic energy of the molecules within a closed container if the absolute temperature is doubled?

How does increasing the intermolecular forces between gas molecules affect the deviation from ideal gas behavior?