1 mol of an ideal gas undergoes reversible isothermal expansion from an initial volume `V_1` to final volume 10 `V_1` and does 10 kJ of work. The initial pressure was `1xx10^7` Pa, Calculate the value of `V_1`.

1 mole of an ideal gas undergoes reversible isothermal expansion from an initial volume V_1 to a final volume 10V_1 , and does 10 kJ of work. The initial pressure was 1 xx 10^7 Pa. If there were 2 mole of gas, what must its temperature would have been ?

1 mol of an ideal gas is expanded from volume V_(1) " to " 10 V_(1) . If work done by the gas is 10 kJ and the initial pressure of the gas is 1xx10^(7) Pa , then calculate V_(1) . What will be the temperature of the gas if the amount is 2 mol ?

1 mol of an ideal gas is expanded from its initial volume of 1 L to the final volume of 100 L at 25^(@)C . What will be the change in enthalpy for this process?

A 2.5 mol sample of an ideal gas is compressed in reversible isothermal process from a volume of 12L to a volume of 5 L at 27^(@)C . Calculate the work done on the gas.

Calculate entropy change when 10 moles of an ideal gas expands reversibly and isothermally from an initial volume of 10 litre to 100 litre at 300K.

One mole of an ideal gas at 300 K is expanded ‘ isothermally from an Initial volume of ( litre to 10 litre. What is the value of AE for this process ?

Work done during isothermal expension of one mole of an ideal gas from 10 atm to 1 atm at 300 K is

A 3 mol sample of an ideal gas at STP expands in an isothermal reversible process to atttain a final volume of 100 L. calculate the work done by the gas.

Calculate the entropy change involved in the isothermal expansion of 5 mol of ideal gas from a volume of 10 L to 100 L at 300 k