Problem: Consider the following reaction at equilibrium6A (s) + 7B (g) ⇌ 5C (g) + 8D (l)           ΔH = -3226.6 kJ/molWhich one of the following statements is correct?A. Increasing the temperature would shift the reaction right.B. Increasing the temperature would decrease the value of K.C. Increasing the total pressure on the system would cause the reaction to shift left. D. Adding a catalyst would favor the forward reaction, causing the reaction to shift right.E. Adding some A would cause the reaction to shift right.

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FREE Expert Solution

We’re being asked to identify the correct statement for the given reaction:

6 A(s) + 7 B(g)  5 C(g) + 8 D(l)       ΔH = –3226.6 kJ/mol


According to Le Chatelier’s Principle, if a system (chemical reaction) is at equilibrium and we disturb it, then the system will readjust to maintain its equilibrium state.



Since the reaction is exothermic, ΔH = (–), heat is given off as a product:

6 A(s) + 7 B(g)  5 C(g) + 8 D(l) + heat


Now, let’s look at each given statement.


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Problem Details

Consider the following reaction at equilibrium

6A (s) + 7B (g) ⇌ 5C (g) + 8D (l)           ΔH = -3226.6 kJ/mol

Which one of the following statements is correct?

A. Increasing the temperature would shift the reaction right.

B. Increasing the temperature would decrease the value of K.

C. Increasing the total pressure on the system would cause the reaction to shift left. 

D. Adding a catalyst would favor the forward reaction, causing the reaction to shift right.

E. Adding some A would cause the reaction to shift right.

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