We are asked to calculate ΔH˚_{rxn} for the following reaction: C_{2}H_{4}(g) + H_{2}(g) → C_{2}H_{6}(g).

The balanced reaction is:

C_{2}H_{4}(g) + H_{2}(g) → C_{2}H_{6}(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_{2}H_{4}(g) + H_{2}(g) → C_{2}H_{6}(g)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

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