A quantity (0.0250 mol) of an ideal gas is expanded reversibly from 35.0 mL to 90.0 mL at a constant temperature of 30.0 °C inside of a frictionless piston. Calculate the amount of work, in J, done by the system.

One mole of an ideal monatomic gas is inititally at 300 K and 1010 J/L pressure inside a cylinder with a frictionless piston. the cylinder is an isolated (adiabatic) system. the gas expands against zero external pressure. when the volume expands to 24.7 L, a peg stopes the piston. calculate deltaU (the change in energy), q (the heat transferred to the system), and w (the work done by the system) when the expansion is isothermal and reversible.

Two moles of oxygen gas, which can be regarded as ideal with Cp=29.4 J/(K*mol) (independent of temperature), are initially at 298K in a volume of 12.5 dm^3. The gas is expanded reversibly to 353K at constant pressure. Calculate the final volume and q, w, delta U, and delta H.

Suppose that the gas in the previous question is reversibly compressed to half its volume at constant temperature (298K). Calculate the final pressure and q, w, delta U, and delta H.