The volume of 1 kg of helium in a piston–cylinder device is initially 5 m3. Now helium is compressed to 2 m3 while its pressure is maintained constant at 180 kPa. Determine the initial and final temperatures of helium as well as the work required to compress it, in kJ.

The equation for calculating the work performed when a piston in a cylinder expands against a constant pressure is w = −P ∙ΔV, where ΔV is the change in volume inside the cylinder. How much work is performed (in joules) when a piston pushes against a constant pressure of 1.21 atm, resulting in a volume change of 2.56 mL? (Hint: First determine the units that must be used for each term in the equation.)(101,325 Pa = 1 atm)

An industrial firm supplies compressed air cylinders of volume 0.25 m3 filled to a pressure of 20×106 Pa at 17 ºC. Calculate the number of moles of air in each cylinder.

A closed system consisting of 2 lb of a gas undergoes a process during which the relation between pressure and volume is pV" = constant. The process begins with p₁ = 25 lbf/in², V₁ = 13 ft³ and ends with p2 = 100 lbf/in². The value of n = 1.3. Determine the final volume, V₂, in ft3, and determine the specific volume at states 1 and 2, in ft³/lb.

A gas originally occupies a volume of 0.5m^3 at a pressure of kPa. It is slowly allowed to expand until the volume is 2.5m^3. Assuming the temperature is kept constant, calculate the final pressure of the gas.

A 0.75 m3 container of an ideal gas at atmospheric pressure is at a temperature of 40 oC and contains heat energy Q. The gas is heated so it now contains heat energy 1.75Q. The temperature of the gas is now