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ΔH = -746.6kJ

Explanation:

Using Hess's law we can find the ΔH of a reaction from the sum of similar reactions. From the reactions:

1. 2CO(g) + O2(g) → 2CO2 ΔH = -566.0kJ

2. N2(g) + O2(g) → 2NO(g) ΔH = 180.6kJ

The negative reaction of 2:

-2. 2NO(g) → N2(g) + O2(g) ΔH = -180.6kJ

The sum of 1 - 2:

2CO(g) + O2(g) + 2NO(g) → 2CO2  N2(g) + O2(g) ΔH = -566.0kJ + (-180.6kJ) =

ΔH = -746.6kJ

Subtracting the molecules that don't change:

2CO(g) + 2NO(g) → 2CO2  + N2(g) ΔH = -746.6kJ

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