We are asked to calculate the value of ΔH˚ for N_{2}O_{4}(g) + 4 H_{2}(g) → N_{2}(g) + 4 H_{2}O(g)

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

Note that we need to *multiply each ΔH˚ by the stoichiometric coefficient* since ΔH˚ is in kJ/mol.

Balanced reaction : N_{2}O_{4}(g) + 4 H_{2}(g) → N_{2}(g) + 4 H_{2}O(g)

Using values from Appendix C in the textbook, calculate the standard enthalpy change for each of the following reactions.

N_{2}O_{4}(g) + 4 H_{2}(g) → N_{2}(g) + 4 H_{2}O(g)

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