The enthalpy change when 1.00 g of water freezes at `0^(@)C` and 1.00 atm is `(DeltaH_("fusion")=1.435 k.cal//mol)`

The enthalpy change when 1 g of water is frozen at 0^@C ( Delta_(fus) H^@=-1.435 kcal/mol) is __________ .

What is the enthalpy change when 1.0 g of water is frozen at 0^(@)C ? Delta_(fus) = H = 6.02 kJ "mol"^(-1) .

The enthalpy change in freezing 1 g of water ( Delta H "fusion "= 6.0 kJ mol^(-1) ) will be

Determine the change in enthalpy and internal energy when 1 mole of water completely vaporises at 100^(@)C and 1 atm pressure. [Latent heat of vaporisation of water=536 cal*g^(-1) ]