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14 February, 02:17

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

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  1. 14 February, 05:40
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    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
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