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Select all the correct answers.

In this reaction, how does the rate of the forward reaction vary with the concentration of the product?

[tex]\[2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g)\][/tex]

A. It increases with an increase in the concentration of [tex]\(S_2(g)\)[/tex].

B. It decreases with a decrease in the concentration of [tex]\(H_2(g)\)[/tex].

C. It increases with a decrease in the concentration of [tex]\(H_2(g)\)[/tex].

D. It decreases with an increase in the concentration of [tex]\(S_2(g)\)[/tex].

E. It decreases with an increase in the concentration of [tex]\(H_2(g)\)[/tex].



Answer :

GinnyAnswer
Let's analyze the given reaction and how the rate of the forward reaction changes with variations in the concentration of products:

[tex]\[ 2 H_2 S (g) \rightleftharpoons 2 H_2(g) + S_2(g) \][/tex]

To determine how the rate of the forward reaction is influenced by the concentration of the products, we need to examine each statement carefully.

1. It increases with an increase in the concentration of [tex]\( S_2(g) \)[/tex]:
- This statement is incorrect. Increasing the concentration of [tex]\( S_2(g) \)[/tex] would shift the equilibrium towards the reactants (according to Le Chatelier's principle), thus decreasing the rate of the forward reaction.

2. It decreases with a decrease in the concentration of [tex]\( H_2(g) \)[/tex]:
- This statement is correct. A decrease in the concentration of [tex]\( H_2(g) \)[/tex] would shift the equilibrium towards the products to replace the lost [tex]\( H_2 \)[/tex], thus decreasing the rate of the forward reaction.

3. It increases with a decrease in the concentration of [tex]\( H_2(g) \)[/tex]:
- This statement is incorrect. A decrease in the concentration of [tex]\( H_2(g) \)[/tex] would shift the equilibrium towards the products, thereby not increasing but actually decreasing the rate of the forward reaction.

4. It decreases with an increase in the concentration of [tex]\( S_2(g) \)[/tex]:
- This statement is correct. Increasing the concentration of [tex]\( S_2(g) \)[/tex] would shift the equilibrium towards the reactants, thereby decreasing the rate of the forward reaction.

5. It decreases with an increase in the concentration of [tex]\( H_2(g) \)[/tex]:
- This statement is correct. Increasing the concentration of [tex]\( H_2(g) \)[/tex] would shift the equilibrium towards the reactants, thereby decreasing the rate of the forward reaction.

Hence, the correct answers are:
- It decreases with a decrease in the concentration of [tex]\( H_2(g) \)[/tex].
- It decreases with an increase in the concentration of [tex]\( S_2(g) \)[/tex].
- It decreases with increase in the concentration of [tex]\( H_2(g) \)[/tex].

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