Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO₂(g) 2NO(g) + O₂(g) $\Delta$H°_rxn = +114 kJ Under which reaction conditions would you expect to produce the largest amount of oxygen?

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Quizplus · Accepted Answer

According to Le Chatelier's principle, increasing temperature favors the endothermic reaction (the reaction with positive ΔH) to absorb heat and shift the equilibrium to the right to produce more products. Therefore, high temperature should be used to produce more oxygen. Additionally, decreasing pressure would favor the side with fewer moles of gas, but since both sides have the same number of gas molecules, pressure does not affect the equilibrium. Therefore, choice C (high temperature, low pressure) is the best option. The presence of a catalyst would increase the rate of the reaction, but would not affect the position of equilibrium or the amounts of products produced.

Nitrogen Dioxide Can Dissociate to Nitric Oxide and Oxygen Δ\DeltaΔ H°rxn = +114 KJ Under Which Reaction Conditions Would You

Nitrogen Dioxide Can Dissociate to Nitric Oxide and Oxygen $\Delta$ H°_rxn = +114 KJ
Under Which Reaction Conditions Would You