Calcualte the enthalpy change on freezing of 1.0 mole of water at `10.0^(@)C` to ice at `-10^(@)`C. `Delta_(fs)H=6.03 kJ mol^(-1)` at `0^(@)C`.
`C_(p)[H_(2)O(l)] = 75.3 J mol^(-1) K^(-1), C_(P)[H_(2)O(s)] = 36.8 Jmol^(-1)K^(-1)`

Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0^(@)C to ice at -10.0^(@)C . Delta_("fus")H=6.03 kJ mol^(-1) at 0^(@)C C_(p)[H_(2)O(l)]=75.3 J mol^(-1)K^(-1) C_(p)[H_(2)O(s)]=36.8 J mol^(-1)K^(-1)

The enthalpy change on freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C is : Delta_(fus). H^(@)=6.03 kJ mol^(-1) at 0^(@)C C_(p)[H_(2)O(l)]=75.3 J mol^(-1)K^(-1) C_(p)[H_(2)O(s)]=36.8 J mol^(-1) K^(-1)

Calculate the enthalpy change of freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C, Delta_(fus)H=6.03 kJ mol^(-1) at 0^(@)C . C_(P)[H_(2)O(l)]=75.3 J mol^(-1) K^(-1) C_(P)[H_(2)O(s)]=36.8 J mol^(-1) K^(-1)

Calculate enthalpy change on freezing 1 mol water at 10^(@)C to ice at -10^(@)C. Delta_("fus")H= 6.03 " kJ mol"^(-1) " at " 0^(@)C . C_(p)[H_(2)O(l)]= 75.3 " J. mol"^(-1). K^(-1) , C_(p)[H_(2)O(s)]= 36.8 " J mol"^(-1). K^(-1) .

The enthalpy change on freezing of 1 mol of water at 5^(@)C to ice at -5^(@) C is (Given Delta_("fus") H = 6 kJ mol^(-1) at 0^(@) C , C_(p) (H_(2) O , l) = 75.3 J mol^(-1) K^(-1) , C_(p) (H_(2) O , s) = 36.8 J mol^(-1) K^(-1))

Calculate the enthalpy change on freezing of '1.0 mol' of water at '10.0^circ C' to ice at '-10.0^circ C . Delta_( fus) H=6.03 kJ mol^(-1)' at '0^circ C .' 'C_p[H_2 O(t)]=7 5 . 3 J m o l^(-1) K^(-1)' 'C_p[H_2 O(s)]=36.8 J mol^(-1) K^(-1)'