Question

3) Given the equilibrium reaction:

Which reaction will be favored if each of the following changed (stresses) is applied to the system at equilibrium?
Favored reaction: forwards/reverse
Change
Addition of A
Addition of C
Removal of B
2A=B+2C

Answer 1

2A =B + 2C hope that helps

Step-by-step explanation:

Answer 2

Addition of A will favor the forward reaction.

Addition of C will favor the reverse reaction.

Removal of B will favor the forward reaction.

The equilibrium reaction provided is:

`\[ 2A \rightleftharpoons B + 2C \]`

According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change. Let's analyze each of the given changes:

1. Addition of A

Adding more reactant (A) to the system will result in the system trying to consume the excess A to re-establish equilibrium. Therefore, the equilibrium will shift to the right, favoring the forward reaction, to form more products (B and C).

2. Addition of C

Adding more product (C) to the system will result in the system trying to reduce the increased concentration of C. Thus, the equilibrium will shift to the left, favoring the reverse reaction, to convert C back into A

3. Removal of B

Removing a product (B) from the system will cause the equilibrium to shift towards the side where B is produced to replace it. Therefore, the equilibrium will shift to the right, favoring the forward reaction to produce more B (and also more C).