Consider these two statements regarding the equation PCl5 (g) ⇌ PCl3 + Cl2 + heat: Statement 1: Adding heat to this reaction mixture would increase the reverse reaction. Statement 2: Cooling this reaction mixture would increase the forward reaction. A. Statements 1 and 2 are both true. B. Statement 1 is true, and statement 2 is false. C. Statements 1 and 2 are both false. D. Statement 1 is false, and statement 2 is true.

Question

Kamila Koch

Chemistry

1 June, 16:23

Consider these two statements regarding the equation PCl5 (g) ⇌ PCl3 + Cl2 + heat: Statement 1: Adding heat to this reaction mixture would increase the reverse reaction. Statement 2: Cooling this reaction mixture would increase the forward reaction. A. Statements 1 and 2 are both true. B. Statement 1 is true, and statement 2 is false. C. Statements 1 and 2 are both false. D. Statement 1 is false, and statement 2 is true.

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Answers (1)

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Abigayle Reese · Answer 1

Answer: - A. statements 1 and 2 are both true.

Explanations: - As per Le Chatelier's principle, a reaction shifts to the direction where it could oppose the change made to it at equilibrium. For example, if a reactant concentration is increased by adding it then the reaction shifts to the product side so that the added reaction could be used.

The reaction is exothermic in nature as heat is a product means the heat is released in the reaction.

So, if the heat is added then reaction must shift to the left side so that the added heat could be used.

Similarly, if the reaction mixture is cooled then reaction shifts to the right side so that the heat could be generated.

Hence, both the statements are true and A is the correct choice.