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?

Using the Ideal Gas Law, calculate the pressure in atmospheres if 0.00245 mol of gas occupies 419 mL at 136°C.

Using the Ideal Gas Law, calculate the pressure in atmospheres if 0.00255 mol of gas occupies 413 mL at 138 °C. Assume 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).

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 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?