Which of the following reactions is product favored by increasing the temperature of the reaction mixture?
I. 2 NO₂ (g) N₂(g) + 2 O₂(g) (exothermic)
II. 2 CO₂ (g) + 2 H₂ O (g) + heat C₂ H₄ (g) + 3 O₂(g)
III. 2 KCl (s) + 3 O₂(g) 2 KClO₃(s) ( D H 0)

Question

Which of the following reactions is product favored by increasing the temperature of the reaction mixture?
I. 2 NO₂ (g)

N₂(g) + 2 O₂(g) (exothermic)
II. 2 CO₂ (g) + 2 H₂ O (g) + heat Which of the following reactions is product favored by increasing the temperature of the reaction mixture? I. 2 NO₂ (g) N₂(g) + 2 O₂(g) (exothermic) II. 2 CO₂ (g) + 2 H₂ O (g) + heat C₂ H4 (g) + 3 O₂(g) III. 2 KCl (s) + 3 O₂(g) 2 KClO3(s) ( D H 0) A) I only B) II only C) I and III D) II and III E) All of these

C₂ H₄ (g) + 3 O₂(g)
III. 2 KCl (s) + 3 O₂(g) Which of the following reactions is product favored by increasing the temperature of the reaction mixture? I. 2 NO₂ (g) N₂(g) + 2 O₂(g) (exothermic) II. 2 CO₂ (g) + 2 H₂ O (g) + heat C₂ H4 (g) + 3 O₂(g) III. 2 KCl (s) + 3 O₂(g) 2 KClO3(s) ( D H 0) A) I only B) II only C) I and III D) II and III E) All of these

2 KClO₃(s) ( D H 0)

Quizplus · Accepted Answer

In reaction II, the production of C₂H₄ is favored by increasing the temperature because heat is a reactant in the forward reaction. Increasing the temperature will shift the equilibrium towards the products side in accordance with Le Chatelier's principle. In reaction I, the production of N₂ and O₂ is favored by decreasing the temperature because the reaction is exothermic. In reaction III, the production of KClO₃ is neither endothermic nor exothermic, so changing the temperature will not affect the equilibrium.

Which of the Following Reactions Is Product Favored by Increasing