The `Delta S` for the vaporisation of 1 mol of water is 88.3 J/mole K. The value of `Delta S` for the condensation of 1 mole of water vapour will be

The Delta S for the vaporization of 1 mol of water is 88.3 J/mol K. The value of Delta S for the condensation of 1 mol of vapour will be ________ .

The Delta S for the vaporization of 1 mol of water is 88.3 J/mol K. The value of Delta S for the condensation of 1 mol of vapour will be ________ .

The enthalpy of vaporisation of water at 100^(@)C is 40.63 KJ mol^(-1) . The value Delta E for the process would be :-

The enthalpy of vaporisation of water at 100^(@)C is 40.63 KJ mol^(-1) . The value Delta E for the process would be :-

Assertion: The increase in internal energy (DeltaE) for the vaporisation of 1 mole of water at 1 atm and 373K is zero. Reason: For all isothermal processes DeltaE=0 .

Assertion: The increase in internal energy (DeltaE) for the vaporisation of 1 mole of water at 1 atm and 373K is zero. Reason: For all isothermal processes DeltaE=0 .

If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourisation of 1 mol of water at 1 bar and 100^(@)C is 41 KJ mol^(-1) . Calculate the internal energy, when i) 1 mol of water is vaporised at 1 bar pressure and 100^(@)C ii) 1 mole of water is converted into ice.