7. Gases

Using the Ideal Gas Law, calculate the pressure in atm of a 25.0 L metal tank containing 12.0 moles of hydrogen gas and 4.0 moles of nitrogen gas at a temperature of 298 K.

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the identity of the halogen?

A 1.20 L weather balloon on the ground has a temperature of 25.0 °C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.710 atm, the new volume is 1.80 L. What is the temperature (in °C) of the air at the elevation where the balloon rises?

A 10.0 mL container of helium is sealed at 22.0°C and 1.00 atm pressure. What pressure would be exerted by the helium if the container were heated to 220°C, assuming the volume remains constant?

A balloon filled with helium gas at 20°C occupies 6.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. Using the Ideal Gas Law, what is the volume of the balloon in the liquid nitrogen?

A capsule of gas has a volume of 550 L, a pressure of 1750 atm, and a temperature of 7500 degrees Celsius. It is broken, releasing the gas into an environment at STP. How many moles of gas are there in the capsule?

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 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?

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?