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)`

Explanation

`triangle^(H)" cpdt "=C_(p) xx trianglet` 1 mole of water to freeze temperature down from `10^@C" to "0^@C`
=`75.3 xx 10`
`=753 J =0.753kJ`
`triangle_("fus")^H =6.03kJ`
1 mole of water taken to `-10^@C" from "0^@C`
`triangle^H=C_p, triangleT=36.8 xx -10 =-3685`
=0.368kJ
Total enthalpy =6.03+0.753 -0.368
=6.415kJ/mole