`5 mol` of an ideal gas expands reversibly from a volume of `8 dm^(3)` at a temperature of `27^(@)C`. Calculate the chngae in entropy.

Five moles of anideal gas expends reversily from a volume of 8dm^(3) at a temperature of 27^(@)C Calculate the change in entropy.

5 mol of an ideal gas expands reversibly from a volume of 8 dm^(3) to 80 dm^(3) at a temperature of 27^(@)C . Calculate the chngae in entropy.

5 mol of an ideal gas expand reversibly from a volume of 8 dm^(3) to 80 dm^(3) at an temperature of 27^(@)C . Calculate the change in entropy.

5 mol of an ideal gas expand reversibly from a volume of 8 dm^(3) to 80 dm^(3) at an temperature of 27^(@)C . Calculate the change in entropy.

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.

One mole of an ideal gas at 27^(@)C undergoes isothermal expansion reversible from a volume of 10 dm^(3) to a volume of 20 dm^(3) . Calculate the work done on the gas.

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.

One mole of an ideal gas expands reversibly and adiabatically from a temperature of 27^@C . If the work done during the process is 3 kJ, then final temperature of the gas is ( C_V = 20 J/K )