A gas is initially at 328 K, 842 torr, and occupies a volume of 5.43 L.  What volume will the gas occupy (in L) if the temperature and pressure decrease, respectively, to 7oC and 0.89 atm?

A sample of N2N2 gas has a volume of 19.0 L at a pressure of 1.50 atm and a temperature of 23 ∘C. What volume, in liters, will the gas occupy at 3.50 atm and 231 ∘C? Assume ideal behavior.

The density of 1.00 mol of an unknown gas at a temperature of -66oC and a pressure of 2,203 torr is 10.9 g/L.  Calculate the molar mass of the unknown gas.

45.0 L of an ideal gas at 288 K and 3.50 atm are heated to 373 K with a new pressure of 8.20 atm. What is the new volume (in L)?

A certain mass of nitrogen gas occupies a volume of 8.20 L at a pressure of 1.78 atm. At what pressure will the volume of this sample be 10.58 L? Assume constant temperature and ideal behavior.

For a gas sample whose total pressure is 740 torr, what are the partial pressures if the gas present consists of 1.0 mol of N₂, 0.23 mol of O2, and 0.051 mol of Ar? Partial pressure of N₂ Partial pressure of O₂ = Partial pressure of Ar = = = torr torr torr

The gas in a 1,528 mL balloon at sea level has a pressure of 762 mmHg, and 21.1 ℃. If the balloon rises to an altitude where its pressure is 135 mmHg and its temperature is -22.5 ℃, what is the volume (in L) of the balloon at the higher altitude?

If 1.50 L of a gas is at standard temperature and pressure is compressed to 556 mL, what is the new pressure of the gas in atm (hint, temperature stays the same)?

A 0.400 L sample of gas at - 55.0 degrees * C and a pressure of 2.15 atm is allowed to expand to double its original volume (i.e. L). Calculate the final pressure for the gas, in atm, if the temperature held constant.