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

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 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.

1 mole of an ideal gas at 25°C is subjected to expands reversibly 10 times of its initial volume. What is the change in entropy _________ JK-1

The molar specific heat at constant volume of an ideal gas is equal to 2.5 times the universal gas constant (8.314 J/mol.K). When the temperature increases by 100k, the change in molar specific enthalpy is ___ J/mol.: