During Volcanic Eruptions, Hydrogen Sulfide Gas Is Given Off and Oxidized

During volcanic eruptions, hydrogen sulfide gas is given off and oxidized by air according to the following chemical equation: 2H₂S(g) + 3O₂(g) $\rarr$ 2SO₂(g) + 2H₂O(g)
Calculate the standard enthalpy change for the above reaction given: $\begin{array}{ll}3 \mathrm{~S}(\mathrm{~s}) +2 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) +\mathrm{SO}_{2}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=146.9 \mathrm{~kJ} / \mathrm{mol} \\\mathrm{~S}(\mathrm{~s}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{SO}_{2}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=-296.4 \mathrm{~kJ} / \mathrm{mol}\end{array}$

A) -1036.1 kJ/mol
B) -742.3 kJ/mol
C) -149.5 kJ/mol
D) 443.3 kJ/mol
E) 742.3 kJ/mol

Correct Answer:

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