One mole of an ideal gas at 300 K is reversibly and isothermally compressed from a volume of 20.0 L to a volume of 10.0 L. Because the water bath thermal reservoir in the surroundings is very large, T remains essentially constant at 300 K during the process. Calculate ΔS system in J/K.

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is

Two moles of an ideal gas originally at 380 torr and 298 K are compressed at constant temperature to a final pressure of 680 torr. Use the ideal gas law to calculate the volumes of gas at the initial and final pressures.(3pts)Initial volume (L), at 380 torr

10 mol of an ideal gas is expanded reversibly isothermally from 1 L to 10 L at 100 K. The work done during the process is:–1.91 kJ–0.95 kJ–19.1 kJ–38.2 kJ

1 mole of an ideal gas A(CV, m = 3R) and 2 mole of an ideal gas B are  taken in a container and expanded reversible and adiabatically from 1 litre to 4 litre starting from initial temperature of 320 K. ΔE or ΔU for the process is :

One mole of an ideal gas initially at a temperature of Ti = 1.0°C undergoes an expansion at a constant pressure of 1.00 atm to nine times its original volume.(a) Calculate the new temperature Tf of the gas. K(b) Calculate the work done on the gas during the expansion. kJ