What happens to the pressure of a gas sample when the volume is halved and its Kelvin temperature is doubled, assuming the amount of gas remains constant?

How many moles of O2 were yielded in an experiment if 3.85 L of O2 was gathered over water at 24 °C and a total pressure of 768.5 torr? Assume the partial pressure of water vapor at 24 °C is 22.4 torr. Use the ideal gas law (R = 0.0821 L·atm/mol·K).

Using the Ideal Gas Law, how many moles of gas were added to a balloon that initially contained 2.3 moles of gas and had a volume of 1.4 L, if the final volume of the balloon is 7.2 L and the temperature and pressure remain constant?

The gas is located in a closed container with a volume of 10.0 L at a pressure of 100,000.0 Pa and a temperature of 10.0°C. What would be the temperature of this gas in degrees Celsius if it was compressed to a new volume of 5.0 L and the pressure was decreased to 50,000.0 Pa?

The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at 1.33 atm is _______ °C. (Use R = 0.0821 L·atm/mol·K)

What is the density in g/L of laughing gas, dinitrogen monoxide (N₂O), at a temperature of 321 K and a pressure of 131 kPa, using the Ideal Gas Law?

What is the pressure (in torr) of 2.10 mol of gas in a 7.00 L container at 65.0 °C, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K, 1 atm = 760 torr)

What is the total pressure exerted by a mixture of gases in a 20.0 L container at 29.7°C if the mixture contains 0.400 mol O2, 0.700 mol CH4, and 0.500 mol SO2, assuming ideal gas behavior?

What is the pressure in a 13.0 L cylinder filled with 45.8 g of oxygen gas (O2) at a temperature of 318 K, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K)