Calculate the entropy change during the melting of one mole of ice into water at 0^@C Enthalpy of fustion of ice is 6008 J mol^(-1) (ii) Write the balanced chemical equation for K_(c) = ([CaO_((s))][CO_(2(g))])/([CaCO_(3(s)))

Calculate the entropy change during the melting of one mole of ice int

1.	Calculate the entropy change during the melting of one mole of ice into water at 0^@C Enthalpy of fustion of ice is 6008 J mol^(-1) (ii) Write the balanced chemical equation for K_(c) = ([CaO_((s))][CO_(2(g))])/([CaCO_(3(s)))
Answer» Solution :Given `DeltaS_("FUSION")=6008 J mol^(-1)` `T_(R) =0^@C = 273 K` `H_(2)O(S) overset(273K) rarr H_(2) O(l)` `Delta S_("fusion")= (Delta H_("fusion"))/(T_f)` `Delta S_("fusion")= (6008)/(273)` `Delta S_("funsion")=22.007 JK^(-1) mol ^(-1)` (ii) `CaCO_(3(s)) hArr CaO_((s))+CO_(2(g))`