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 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 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 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?

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?

According to Avogadro's Law, which of the following is true about the volume of a gas at a given temperature and pressure?

Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 °C. At what temperature does benzene boil when the external pressure is 410 torr?

Binary compounds of alkali metals and hydrogen react with water to produce H₂(g). The H₂ from the reaction of a sample of NaH with an excess of water fills a volume of 0.510 L above the water. The temperature of the gas is 35°C and the total pressure is 0.980 atm. Using the Ideal Gas Law, what is the number of moles of H₂ produced?