A sample of krypton gas at 3.50 atm is heated from 20.0 °C to 150.0 °C. If the volume remains constant, what is the final pressure?

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 °C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.80 atm and the temperature to 25 °C, assuming the amount of gas remains constant?

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112°C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.85 atm and the temperature is changed to 25°C, assuming the amount of gas remains constant?

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 °C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.80 atm and the temperature to 25 °C, assuming the amount of gas remains constant?

A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?

A sample of nitrogen gas is stored in a 490.7 mL flask at 108 kPa and 10.0°C. The gas is transferred to a 750.0 mL flask at 20.6°C. What is the pressure of nitrogen in the second flask?

A syringe contains 0.65 moles of He gas that occupy 900.0 mL. What volume (in L) will the syringe hold if 0.35 moles of Ne are added, assuming ideal gas behavior and constant temperature and pressure?

Using the Ideal Gas Law, calculate the number of moles of air in a car tire with an internal volume of 30.0 L, a temperature of 20°C, and a pressure of 3.50 atm.

A weather balloon is inflated to a volume of 27.3 L at a pressure of 747 mmHg and a temperature of 28.5 °C. The balloon rises in the atmosphere to an altitude where the pressure is 385 mmHg and the temperature is -13.4 °C. Assuming the balloon behaves as an ideal gas, what is the new volume of the balloon at the higher altitude?