# Problem: Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the following equation: N2H4(l) + N2O4(g) → 2 N2O(g) + 2 H2O(g). Calculate ΔH˚rxn for this reaction using standard enthalpies of formation.

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###### FREE Expert Solution

We’re being asked to determine the standard enthalpy change (ΔH˚rxn) for the balanced reaction

N2H4(l) + N2O4(g) → 2 N2O(g) + 2 H2O(g)

Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:

$\overline{){\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{\mathbf{f}\mathbf{,}\mathbf{products}}{\mathbf{-}}{\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{\mathbf{f}\mathbf{,}\mathbf{reactants}}}$

92% (483 ratings)
###### Problem Details

Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the following equation: N2H4(l) + N2O4(g) → 2 N2O(g) + 2 H2O(g). Calculate ΔH˚rxn for this reaction using standard enthalpies of formation.

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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Based on our data, we think this problem is relevant for Professor Stacey's class at University of Manitoba.

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