The enthalpy changes for three reactions are provided below

CHEMISTRY · Single correct · A Level · Chemistry · Energetics · Energetics

Problem

The enthalpy changes for three reactions are provided below. 1. 2 Al(s)+32 O2(g)→Al2O3(s)2\,\text{Al}(s) + \tfrac{3}{2}\,\text{O}_2(g) \rightarrow \text{Al}_2\text{O}_3(s) ΔH1=−1675.7 kJ\Delta H_1 = -1675.7\,\text{kJ} 2. Al2O3(s)+3 H2SO4(aq)→Al2(SO4)3(aq)+3 H2O(l)\text{Al}_2\text{O}_3(s) + 3\,\text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3\,\text{H}_2\text{O}(l) ΔH2=−345.0 kJ\Delta H_2 = -345.0\,\text{kJ} 3. H2O(l)→H2(g)+12 O2(g)\text{H}_2\text{O}(l) \rightarrow \text{H}_2(g) + \tfrac{1}{2}\,\text{O}_2(g) ΔH3=+285.8 kJ\Delta H_3 = +285.8\,\text{kJ} Using these data, what is ΔH\Delta H (to three significant figures) for the reaction 2 Al(s)+3 H2SO4(aq)→Al2(SO4)3(aq)+3 H2(g)2\,\text{Al}(s) + 3\,\text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3\,\text{H}_2(g)? (a) −2.02×103 kJ-2.02 \times 10^{3}\,\text{kJ} (b) −1.16×103 kJ-1.16 \times 10^{3}\,\text{kJ} (c) −1.73×103 kJ-1.73 \times 10^{3}\,\text{kJ} (d) −2.88×103 kJ-2.88 \times 10^{3}\,\text{kJ}

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