Water boils at `95^(@)C` in Denver, the mile high city. Calculate the atomospheric pressure in Denver. `DeltaH_(Vap)` for `H_(2)O=40.67 KJ mol^(-1)`.

DeltaH^(@) " of " H_(2)O_((l)) is ………… KJ/mol.

When 1.8 g of steam at the normal boiling point of water is converted into water at the same temperature, enthalpy and entropy changes respectively will be (DeltaH_("vap") (for water) =40.8kJ"mol"^(-1) )

A swimmer coming out from a pool is covered with a film of water weighing about 18g. How much heat must be supplied to evaporate this water at 298 K? Calculate the internal energy of vaporisation at 100^@C . DeltaH_(vap)^@ for water at 373K = 40.66 kJ mol^(-1)

Is the vaporisation of water at 50^(@)C and 1 atm spontaneous? Given: For vaporisation of water at what temperature and pressure, DeltaH=40.67kJ*mol^(-1) and DeltaS=108.79J*K^(-1)*mol^(-1) .

Delta S for vapouization of 900g water (in KJ/K ) is Delta H_(Vap)=40KJ(mol)^-1

What is DeltaU when 2.0 mole of liquid water vaporise at 100^(@)C ? The heat of vaporistaion , DeltaH vap. of water at 100^(@)C is 40.66 kJ mol^(-1) .