The heat of solution of anhydrous CuSO_4 and CuSO_4 * 5 H_2 O are -70 kJ mol^-1 and +12 kJ mol^-1 respectively. The heat of hydration of CuSO_4 to CuSO_4 * 5 H_2 O is -x kJ. The value of x is ________. (nearest integer).

(I) CuSO_4 + aq -> CuSO_4 (sol) Delta H = -70 kJ \ (II) CuSO_4 * 5 H_2 O + aq -> CuSO_4 (sol) Delta H = +12 kJ [1em] Subtracting (II) from (I): \ CuSO_4 + 5 H_2 O -> CuSO_4 * 5 H_2 O \ Delta H = -70 - 12 = -82 kJ

The heat of solution of anhydrous CuSO4 and CuSO4 5 H2 ... | null (Chemistry)

\begin{aligned} & \text{(I)} \quad \mathrm{CuSO}_4 + \text{aq} \longrightarrow \mathrm{CuSO}_4 \text{(sol)} \\& \Delta H = -70 \mathrm{~kJ} \\\\ & \text{(II)} \quad \mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O} + \text{aq} \longrightarrow \mathrm{CuSO}_4 \text{(sol)} \\& \Delta H = +12 \mathrm{~kJ} \\[1em] & \text{Subtracting (II) from (I):} \\ & \mathrm{CuSO}_4 + 5 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O} \\ & \Delta H = -70 - 12 = -82 \mathrm{~kJ} \end{aligned}

Explanation

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