Question

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

Answer 1

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

Answer 2

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:

$\Delta G^\circ=\Delta G_{product}-\Delta G_{reactant}$

Computation for the Gibbs free energy of the reaction

The balanced equation has been given as:

$\rm NO\;+\;\dfrac{1}{2} \;O_2\rightarrow\;NO_2$

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

The change in the energy has been given as:

$\Delta G^\circ=\rm (NO_2)-(NO\;+\;\dfrac{1}{2}\;O_2 )\\\\ \Delta \textit G^\circ=51.9-(86.6+0)kJ/mol\\\\ \Delta \textit G^\circ=-34.7 \;kJ/mol$

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

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