`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 2 litre to 20 litre at 300 K. The enthalpy change (in kJ) for the process is

Two mole of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthapy 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

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The internal energy change (in kJ) for the process (R = 8.3J)

Two moles of an ideal gas expanded isothermally and reversibly from 1L to 10L at 300K . What is the enthalpy change?