Two moles of an ideal gas are expanded isothermally and reversible from 20 L to 30 L at 300 K. Calculate work done.(R=8.314`JK^(-1)mol^(-1)`)

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

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

5mol of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 6L to 60L . The work done in kJ 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

If x mole of ideal gas at 27^(@)C expands isothermally and reversibly from a volume of y to 10 y, then the work done is

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?

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