For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO ( g ) + O 2 ( g ) − ⇀ ↽ − 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ G ° = − 69.0 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are P NO = 0.500 atm , P O 2 = 0.200 atm , and P NO 2 = 0.600 atm ?

The for the given reaction at 298 K is -64.11 kJ/mol

Explanation:

For the given chemical equation:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= Standard Gibbs free energy = -69.0 kJ/mol = -69000 J/mol   (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/K mol

T = Temperature = 298 K

= Ratio of partial pressure of products and reactants =

Putting values in above equation, we get:

Hence, the for the given reaction at 298 K is -64.11 kJ/mol

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