Determine the heat of formation of sulfuric acid,H₂SO₄(l),from the following thermochemical equations: $\begin{array}{ll} \mathrm{S}_{8}(s)+8 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{2}(g) & \Delta H=-2374.6 \mathrm{~kJ} \ \mathrm{~S}_{8}(s)+12 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{3}(g) & \Delta H=-3165.8 \mathrm{~kJ} \ \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{3}(g) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(l) & \Delta H=-132.4 \mathrm{~kJ} \ 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H=-571.7 \mathrm{~kJ} \end{array}$

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Quizplus · Accepted Answer

The heat of formation of sulfuric acid can be determined by adding the enthalpies of the following reactions:$$\mathrm{S}_{8}(s)+8 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{2}(g) \quad \Delta H=-2374.6 \mathrm{~kJ}$$$$\mathrm{S}_{8}(s)+12 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{3}(g) \quad \Delta H=-3165.8 \mathrm{~kJ}$$$$8 \mathrm{SO}_{2}(g)+8 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{3}(g) \quad \Delta H=-791.2 \mathrm{~kJ}$$$$8 \mathrm{SO}_{3}(g)+8 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 8 \mathrm{H}_{2} \mathrm{SO}_{4}(l) \quad \Delta H=-1059.2 \mathrm{~kJ}$$The overall reaction is:$$\mathrm{S}_{8}(s)+12 \mathrm{O}_{2}(g)+8 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 8 \mathrm{H}_{2} \mathrm{SO}_{4}(l) \quad \Delta H=-814.0 \mathrm{~kJ}$$Therefore, the heat of formation of sulfuric acid is -814.0 kJ.

Determine the Heat of Formation of Sulfuric Acid,H2SO4(l),from the Following

Determine the Heat of Formation of Sulfuric Acid,H₂SO₄(l),from the Following