Consider the oxidation of no to no2: no (g) + 12o2 (g) →no2 (g) calculate δg∘rxn at 25∘c. express the free energy change in kilojoules to three significant figures

Given reaction is NO (g) + 1/2 O₂ (g) →NO₂ (g)

ΔGf⁰ [NO₂ (g) ] = 51.9 kJ/mol

ΔGf⁰ [NO (g) ] = 86.6 kJ/mol

ΔGf⁰ [O2 (g) ] = 0 kJ/mol

ΔG⁰rxn = ΔGf⁰ (products) - ΔGf⁰ (reactants)

= ΔGf⁰ [NO₂ (g) ] - {ΔGf⁰ [NO (g) ] + (1/2) ΔGf⁰ [O₂ (g) ]}

= 51.9 kJ/mol - { 86.6 kJ/mol + 0}

= - 34.7 kJ/mol

Therefore, ΔG⁰rxn = - 34.7 kJ/mol