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The following reaction was carried out in a closed system:
N2(g) + O2(g) <--> 2NO(g)
Hrxn = -ve value
Which of the following will favor the production of NO?

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Correct Answer: D. Decreased temperature
Since the reaction is exothermic (negative enthalpy), heat can be considered a product in this reaction. A decrease in temperature will result in the equilibrium shifting to the right to bring heat to the system resulting in an increase in NO production, in accordance with Le Chatelier’s principle. A change in overall pressure of the system will not affect the equilibrium because there is an equal amount of moles of gas on both sides of the equation providing an even pressure. A catalyst affects the rate of a reaction not thermodynamic properties such as equilibrium.
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