Question 24 of 69intermediate🔧 ApplyNumerical3 marks

Calculate a) ΔG∘\Delta G^\circ and b) the equilibrium constant for the formation of NO2_2 from NO and O2_2 at 298K

NO(g)+12O2(g)⇌NO2(g)NO (g) + \frac{1}{2} O_2 (g) \rightleftharpoons NO_2 (g)

where

ΔG∘(NO2)=52.0 kJ/mol\Delta G^\circ (NO_2) = 52.0 \text{ kJ/mol} ΔG∘(NO)=87.0 kJ/mol\Delta G^\circ (NO) = 87.0 \text{ kJ/mol} ΔG∘(O2)=0 kJ/mol\Delta G^\circ (O_2) = 0 \text{ kJ/mol}
(a)

Calculate ΔG∘\Delta G^\circ

Answer

ΔG∘=−35.0 kJ/mol\Delta G^\circ = -35.0 \text{ kJ/mol}

(b)

Calculate the equilibrium constant

Answer

K=1.36×106K = 1.36 \times 10^6

Explanation

To find the standard Gibbs free energy change (ΔG∘\Delta G^\circ) for the reaction, we use the standard Gibbs free energy of formation values for the products and reactants. For the equilibrium constant, we apply the relationship between ΔG∘\Delta G^\circ and the equilibrium constant KK.

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