Given the reaction: N2(g) +2O2(g) ⇌ 2NO2(g) The forward reaction is endothermic. Determine which of the following changes would result in more reactant being produced. I. Increase NO2 II. Increase O2 III. Add a catalyst IV. Increase the temperature V. Decrease the pressure A. I and V B. II and IV C. II, III, and V D. All

A. I and V

Explanation:

According to Le Chatelier's Principle, increasing the product side will cause the equilibrium to shift back towards the reactant side, so I is true.  By the same principle, II is false.

For gases, decreasing the pressure will cause the equilibrium to shift towards the side with higher number of moles.  So V is true.

The reaction is endothermic, so increasing the temperature will shift the equilibrium to the products, so IV is false.  And adding a catalyst has no effect on the equilibrium, so III is false.

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