Zinc reacts with aqueous copper(II) sulfate, CuSO4(aq)\text{CuSO}_4\text{(aq)}CuSO4(aq), in a displacement reaction as shown below:
Zn(s)+CuSO4(aq)→ZnSO4(aq)+Cu(s)ΔH=−218 kJ mol−1 \text{Zn(s)} + \text{CuSO}_4\text{(aq)} \rightarrow \text{ZnSO}_4\text{(aq)} + \text{Cu(s)} \quad \Delta H = -218\text{ kJ mol}^{-1} Zn(s)+CuSO4(aq)→ZnSO4(aq)+Cu(s)ΔH=−218 kJ mol−1A student adds an excess of zinc powder to 75.0 cm3 of 0.600 mol dm-3 CuSO4(aq)\text{CuSO}_4\text{(aq)}CuSO4(aq). The initial temperature of the solution is 18.2 ∘C18.2\text{ }^\circ\text{C}18.2 ∘C.
Determine the maximum temperature reached in this reaction. Give your answer to 3 significant figures.
Assume that the specific heat capacity and density of the solution are the same as for water (c=4.18 J g−1 K−1c = 4.18\text{ J g}^{-1}\text{ K}^{-1}c=4.18 J g−1 K−1, and density = 1.00 g cm-3), and that there are no heat losses.
