A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K, assuming ideal gas behavior?

If a student collects 2.50 L of hydrogen gas over water at a temperature of 25°C and a total pressure of 1.00 atm, what is the partial pressure of the hydrogen gas, given that the vapor pressure of water at 25°C is 0.0313 atm?

A cylinder contains 28.5 L of oxygen gas at a pressure of 1.8 atm and a temperature of 298 K. Using the Ideal Gas Law, how many moles of gas are in the cylinder?

A cylinder contains 30.0 L of oxygen gas at a pressure of 1.9 atm and a temperature of 307 K. How many moles of gas are in the cylinder?

A gas bottle initially contains 0.800 mol of gas at a pressure of 730 mm Hg. If the final pressure is increased to 1.15 atm, how many moles of gas were added to the bottle, assuming constant temperature and volume?

A sample of N2O gas has a density of 2.75 g/L at 298 K. What must be the pressure of the gas, assuming it behaves as an ideal gas?

A sample of argon gas has a volume of 0.240 L, a pressure of 0.900 atm, and a temperature of 27.0°C. At what temperature (°C) will the argon have a volume of 80.0 mL and a pressure of 3.20 atm?

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?