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)

Using the Ideal Gas Law, how many moles of N2 (g) are present in 1.00 L of N2 (g) at 100.°C and 1.00 atm?

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?

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?

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?