Two moles of ideal gas at `27^(@)C` temperature is expanded reversibly from 2 litre to 20 liter. Find entropy change `(R=2cal//molK)` .

2 mol of an ideal gas at 27^(@)C temperature is expanded reversibly from 2L to 20L . Findk entropy change (R = 2 cal mol^(-1) K^(-1))

2 moles of ideal gas is expanded isothermally & reversibly from 1 litre to 10 litre. Find the enthalpy changes in KJ mol^(-1) .

Two moles of an ideal gas is expanded isothermally and reversibly from 2 litre to 20 litre at 300 K. The enthalpy change (in kJ) for the process is

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

One mole of an ideal gas at constant temperature 400K is expanded from 10 litre to 20 litre.The work done in the process is