We are asked to calculate ΔH˚_{rxn} for the following reaction: C(s) + H_{2}O(g) → CO(g) + H_{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: C(s) + H_{2}O(g) → CO(g) + H_{2}(g)

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