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Calculate the enthalpy of hydration of anhydrous copper sulphate (CuSO_(4).5H_(2)O). Given that the enthalpies of solutions of anhydrous copper sulphate and hydrated copper sulphate are -66.5 and +11.7 KJ mol^(-1) respectively |
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Answer» Solution :We are given (i) `(CuSO_(4).5H_(2)O)` `Delta_("sol")H=-66.5KJmol^(-1)` (II) `CuSO_(4).5H_(2)O_((s))+aqrarrCuSO_(4)(aq)` `Delta_("sol")H=-66.5KJmol^(-1)` (ii) `CuSO_(4).5H_(2)O_((s))+aqrarrCuSO_(4)(aq)` `Delta_(sol)H=+11.7KJmol^(-1)` We need `CuSO_(4(s))+5H_(2)O_((l))rarrCuSO_(4).5H_(2)O_((s)),Delta_(hyd)H=?` Substracting equation (ii) from equation (i). we get `CuSO_(4(s))+5H_(2)O_((l))rarrCuSO_(4).5H_(2)O_((s))` `Delta_(hyd)H=-78.2KJmol^(-1)` |
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