Calculate the work done for the vaporisation of 1 mole of water in calories :-(1 atm,`100^(@)C`)

Calculate the work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300 K

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.

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

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 .

Calculate w and DeltaU for the conversion of 1 mol of water at 100^(@)C to steam at 1 atm pressure.Heat of vaporisation of water at 100^(@)C is 40.670 kJ mol^(-1) .Assume ideal gas behaviour.

Calculate the work done when done when 1.0 mol of water at 373K vaporises against an atmosheric pressure of 1.0atm . Assume ideal gas behaviour.

Calculate the work done during isothermal reversible expansion of one mole ideal gas from 10 atm to 1 atm at 300 K .