Question

Consider the reaction described by the following chemical equation. HN3(l) + 2NO(g) ⟶ H2O2(l) + 4N2(g)...

Consider the reaction described by the following chemical equation.

HN3(l) + 2NO(g) ⟶ H2O2(l) + 4N2(g)

What is the enthalpy change associated with the production of 1mol of H2O2 if a reaction that produces 2.50g of H2O2 releases 65.9kJ of heat?

-Assume the reaction occurs under conditions of constant pressure.

-Report the answer to three significant figures.

-Include a negative sign if appropriate.

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Homework Answers

Answer #1

Balanced equation:
2 NH3(l) + 6 NO(g) ====> 3 H2O2(l) + 4 N2(g)
Reaction type: double replacement

Molar mass of H2O2 =  34.0147 g/mol

Mass of H2O2 reacted = 2.5 gm

Moles of H2O2 reacted = 2.5 gm / 34.0147 g/mol = 0.073497 Moles

Amount of heat released = -65.9 Kj

Since energy is released the negative sign appears.

Enthalpy change associated with the production of 1mol H2O2 = -65.9 Kj / 0.073497 Mol = -896.627 Kilo Joules / Mole

Hence -896.627 Kilo Joules of heat will be released for 1 Mole of H2O2

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