Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the following reactions with known ΔG values: 2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ 2N2O(g)→2N2(g)+O2(g)ΔG∘rxn=−207.4kJ
N2O(g)+NO2(g) → 3NO(g) : ΔG = ? ------(1)
2NO(g)+O2(g) → 2NO2(g) : ΔG1 = −71.2kJ -----(2)
N2(g)+O2(g) → 2NO(g) : ΔG2 = +175.2kJ --------(3)
2N2O(g) → 2N2(g)+O2(g) : ΔG3 = −207.4kJ -------(4)
Equ(1) can be obtained from the remaining three equations as follows:
Eqn(1) = [(1/2) x reverse of Eqn(2) ]+Eqn(3) + [(1/2)xEqn(4)]
ΔG = [(1/2)x (-ΔG1 ) ] + ΔG2 + [(1/2) x ΔG3 ]
= [(1/2) x (-(-71.2 kJ))] + 175.2 kJ + [(1/2x(-207.4kJ)]
= +107.1 kJ
Therefore ΔG∘rxn for the reaction: N2O(g)+NO2(g) → 3NO(g) is +107.1 kJ
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