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Find Δ H∘ in kilojoules for the reaction of nitric oxide with oxygen, 2NO(g)+O2(g)⟶N2O4(g), given the...

Find Δ H∘ in kilojoules for the reaction of nitric oxide with oxygen, 2NO(g)+O2(g)⟶N2O4(g), given the following data: N2O4(g)⟶2NO2(g)ΔH∘=55.3kJNO(g)+1/2O2(g)⟶NO2(g)ΔH∘=−58.1kJ

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Homework Answers

Answer #1

Apply Hess Law

2NO(g)+O2(g)⟶N2O4(g)

Given

N2O4(g)⟶2NO2(g) ΔH∘=55.3kJ

NO(g)+1/2O2(g)⟶NO2(g)ΔH∘=−58.1kJ

invert(1) since we need N2O4 in the product side

2NO2(g)⟶N2O4(g) ΔH∘= -55.3kJ

NO(g)+1/2O2(g)⟶NO2(g)ΔH∘=−58.1kJ

Multiply (2) by 2x to calcal NO2

2NO2(g)⟶N2O4(g) ΔH∘= -55.3kJ

2NO(g)+O2(g)⟶2NO2(g)ΔH∘=2*(−58.1) = -116.2 kJ

Add both equations

2NO2(g)+2NO(g)+O2(g)⟶N2O4(g) + 2NO2(g) Hrxn =  -55.3 +  -116.2 = - 171.5 kJ

cnacel common terms

2NO(g)+O2(g)⟶N2O4(g) Hrxn = - 171.5 kJ

which is what we wanted

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