Zinc reacts with aqueous silver nitrate, AgNO3(aq)\text{AgNO}_3\text{(aq)}AgNO3(aq), as shown below:
Zn(s)+2AgNO3(aq)→Zn(NO3)2(aq)+2Ag(s)ΔH=−364 kJ mol−1 \text{Zn(s)} + 2\text{AgNO}_3\text{(aq)} \rightarrow \text{Zn(NO}_3)_2\text{(aq)} + 2\text{Ag(s)} \quad \Delta H = -364\text{ kJ mol}^{-1} Zn(s)+2AgNO3(aq)→Zn(NO3)2(aq)+2Ag(s)ΔH=−364 kJ mol−1A student adds an excess of zinc powder to 250.0 cm3250.0\text{ cm}^3250.0 cm3 of 0.400 mol dm−30.400\text{ mol dm}^{-3}0.400 mol dm−3 AgNO3(aq)\text{AgNO}_3\text{(aq)}AgNO3(aq). The initial temperature of the solution is 20.2 ∘C20.2\text{ }^\circ\text{C}20.2 ∘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= 1.00\text{ g cm}^{-3}=1.00 g cm−3), and that there are no heat losses.
