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

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

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