We are asked to calculate ΔH˚_{rxn} for the following reaction: 2 H_{2}S(g) + 3 O_{2}(g) → 2 H_{2}O(l) + 2 SO_{2}(g)

$\overline{){\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

Note that we need to *multiply each ΔH˚ _{f} by the stoichiometric coefficient* since ΔH˚

Also, note that ΔH˚_{f} for elements in their standard state is 0.

Use standard enthalpies of formation to calculate ΔH˚_{rxn }for the following reaction: 2 H_{2}S(g) + 3 O_{2}(g) → 2 H_{2}O(l) + 2 SO_{2}(g)

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