For a phase change:
`H_(2)O(l)hArrH_(2)O(s)`
`0^(@)C`, 1 bar

For a phase change H_2O(l)⇌H_2O(s) 0^@C ,1 bar

The molar enthalpy change for H_(2)O(l)hArrH_(2)O(g) at 373 K and 1 atm is 41 kJ/mol. Assume ideal behaviour, the internal energy change for vaporization of 1 mol of water at 373 K and 1 atm in KJ "mol"^(-1) is :

For the reaction H_(2)O_((s)) hArr H_(2)O_((l)) at ""^(@)C and normal pressure

Assertion : For the change, H_(2)O_((l))rarr H_(2)O_((s)),DeltaH=DeltaU . Reason : No enthalpy change is involved in this process.

Assertion : For the change, H_(2)O_((l))rarr H_(2)O_((s)),DeltaH=DeltaU . Reason : No enthalpy change is involved in this process.

Which of the followingk is true for the process H_(2) O (s) = H_(2) O (l) at 0^(@)C and 1 atm?

For the process H_(2)O(l)hArrH_(2)O(g),DeltaH=40.8kJ*mol^(-1) at the boiling poinit of water. Calculate molar entropy change for vaporisation from liquid phase.

For the reaction H_(2)O_((i))hArrH_(2)O_((g)) at 373 K and 1 atmospheric pressure