`6` moles of an ideal gas expand isothermally and reversibly from a volume of `1` litre to a volume of `10` litres at `27^(@)C`. What is the maximum work done.

6mole of an ideal gas expand isothermally and reversibly from a volume of 1 litre to a volume of 10 litre at 27° C .The maximum work is done

6 moles of an ideal gas expand isothermally and reversible from a volume of 1dm^(3) to a volme of 10dm^(3) at 27^(@)C . What is the maximum work done? Express your answer in joule.

Calculate the change in entropy when 1 mole nitrogen gas expands isothermally and reversibly from an initial volume of 1 litre to a final volume of 10 litre at 27^(@)C

2 mole of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 4 litre to 40 litre. The work done (in kJ) by the gas is

2 mole of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 4 litre to 40 litre. The work done (in kJ) by the gas is :