One mole of ice is converted into water at 273 K. The entropies of `H_(2)O(s)` and `H_(2)O(l)` are 38.20 and 60.01 J `mol^(-1)K^(-1)` respectively. Calculate the enthalpy change for this conversion a ?

Options

A. 59.59 J/mol
B. 595.95 J/mol
C. 5959.5 J/rnol
D. 595959.0 J/mol

Answer

D

Explanation

`H_(2)O(s)rarrH_(2)O(l)`, `DeltaS=S_l^0-S_s^0`
` = 60.03 - 38.20 = 21.83 Jk^(-1)mol^(-1)`
`DeltaH=TDeltaS=273xx21.83=5959.5 mol^(-1)`