The space shuttle orbiter utilizes the oxidation of methyl hydrazine by dinitrogentetroxide for propulsion. The reaction is 4 N2H3CH3(l) + 5 N2O4(l) ↔ 9 N2(g) + 12 H2O(g) + 4 CO2(g) What is ΔH°rxn for this reaction (in kilojoules)? N2H3CH3(l) ΔHfo = 54 kJ/mol. N2O4(l) ΔHfo = -19.5 kJ/mol. H2O(g) ΔHfo = -241.8 kJ/mol. CO2(g) ΔHfo = -393.5 kJ/mol.
we have:
Hof(N2H3CH3(l)) = 54.0 KJ/mol
Hof(N2O4(l)) = -19.5 KJ/mol
Hof(CO2(g)) = -393.5 KJ/mol
Hof(H2O(g)) = -241.8 KJ/mol
we have the Balanced chemical equation as:
4 N2H3CH3(l) + 5 N2O4(l) ---> 9 N2(g) + 4 CO2(g) + 12 H2O(g)
deltaHo rxn = 9*Hof(N2(g)) + 4*Hof(CO2(g)) + 12*Hof(H2O(g)) - 4*Hof( N2H3CH3(l)) - 5*Hof(N2O4(l))
deltaHo rxn = 9*0 + 4*(-393.5) + 12*(-241.8) - 4*(54.0) - 5*(-19.5)
deltaHo rxn = -4594.1 KJ
Answer: -4594.1 KJ
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