At 373 K, steam and water are in equilibrium and `DeltaH=40.98" kJ mol"^(-1)`. What will be `DeltaS` for conversion of water into system ?
`H_(2)O_((l))rarrH_(2)O_((g))`

At 0^@C , ice and water are in equilibrium and DeltaH = 6.0 kJ mol^(-1) for the process H_2O (s) hArr H_2O (l) What will be Delta S and DeltaG for the conversion of ice to liquid water?

At 0^(@)C ice and water are in equilibrium and DeltaH=6kJ" "mol^(-1) for this process: H_(2)OhArrH_(2)O(l) The values of DeltaS and DeltaG for conversion of ice into liquid water at 0^(@)C are:

If DeltaH_(f)^(0) " for" H_(2)O_(2(l)) and H_(2)O_((l)) " are " -188 kJ mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2(l)) rarr 2H_(2)O_((l)) + O_(2(g)) = ?

If DeltaH_(f)^(@) for H_(2)O_(2)(l) and H_(2)O(l) are -188kJ and mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2)(l)to2H_(2)O(l)+O_(2)(g) ?

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

In the equation 2H_(2)(g)+O_(2)(g)to2H_(2)O(L), DeltaH=-571.6KJ"mol"^(-1) What is the enthalpy of formation of a water molecule.