A 3.00 L sample of a gas at a pressure of 4.00 atm is compressed to 2.00 L at a constant temperature. What is the pressure of the gas?

A sample of an ideal gas initially has a pressure of 0.775 atm at a temperature of 21.5°C. If the temperature of the gas increases to 97.5°C while volume is kept constant, what is the new pressure of the gas?

A flexible container at an initial volume of 7.14 L contains 9.51 mol of gas. More gas is then added to the container until it reaches a final volume of 12.1 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container. number of moles of gas: mol

A sample of gas at 62.0°C occupies a volume of 4.80 L at a pressure of 2.90 atm. How many moles of gas are contained in the sample?

A 1.50 mol sample of He occupies a volume of 2.50 L at a pressure of 14.7 atm. What will be the pressure of a 1.50 mol sample of H2 gas under the same conditions?

A sample of gas takes up 3.5 liters, at a pressure of 0.75 atmospheres and a temperature of 525 degrees Kelvin.  If the sample is cooled to 250 degrees and the pressure drops to 0.25 atmospheres, what is the new volume of the gas?

A sample of methane gas that occupies a volume of 22.4 L at a temperature of 0 °C and a pressure of 1 atm contains moles of gas.

A mixture of two gases, A and B, at a total pressure of 2.95 atm is found to contain 0.42 moles of gas A and 0.86 moles of gas B.  What is the partial pressure (in atm) of gas B?