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

The free energy change for the reaction has been -34.7 kJ/mol.

The oxidation has been defined as the loss of electrons by an atom. The change in the Gibbs free energy of the reaction has been given by:

The balanced equation has been given as:

The free energy for the compounds has been given in the image attached.

The change in the energy has been given as:

The free energy change for the reaction has been -34.7 kJ/mol.

Learn more about free energy change, here:

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