Question

Hydrazine (N₂H₄) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the following equation:

N₂H₄(l)+N₂O₄(g) → 2N₂O(g)+2H₂O(g)

Calculate ΔHrxn for this reaction using standard enthalpies of formation.

Answer 1

To calculate the standard enthalpy change (ΔHrxn) for the reaction, you need the standard enthalpies of formation for all reactants and products, which can be found in thermodynamic tables. The equation ΔHrxn° = ∑ ΔHf° (products) - ∑ ΔHf° (reactants) is used to determine the enthalpy change.

Step-by-step explanation:

To calculate the standard enthalpy change (ΔHrxn) for the oxidation of hydrazine (N₂H₄) with dinitrogen tetroxide (N₂O₄), you need the standard enthalpies of formation (ΔHf°) for all reactants and products involved in the balanced chemical equation. The provided information does not include the ΔHf° values needed, but these can be found in standard references such as thermodynamic tables.

The general formula to compute the standard enthalpy change of a reaction is:

ΔHrxn° = ∑ ΔHf° (products) - ∑ ΔHf° (reactants)

Once the ΔHf° values for hydrazine, dinitrogen tetroxide, nitrous oxide (N₂O), and water (H₂O) are obtained, you can plug them into the equation to get the ΔHrxn.