Question

Explain what happens as a reaction starts with ΔG < 0 (negative) and reaches the point where ΔG = 0.

A) The reaction starts with Q > K as the reaction proceeds, and Q decreases until equilibrium is reached (where Q = K).

B) The reaction starts with Q > K as the reaction proceeds, and Q increases until equilibrium is reached (where Q = K).

C) The reaction starts with Q < K as the reaction proceeds, and Q decreases until equilibrium is reached (where Q = K).

D) The reaction starts with Q < K as the reaction proceeds, and Q increases until equilibrium is reached (where Q = K).

Answer 1

If ΔG is less than zero, the reaction is spontaneous in the forward direction. As the reaction proceeds and reaches equilibrium, Q equals K. If Q is less than K at the start, it will decrease until equilibrium is reached. Correct option is C.

Step-by-step explanation:

If ΔG < 0 (negative), the reaction is spontaneous in the forward direction. As the reaction proceeds and reaches the point where ΔG = 0, the system is at equilibrium. At this point, Q = K, which means that the concentrations of reactants and products are at a ratio that satisfies the equilibrium constant.

If Q < K at the start of the reaction, it will decrease as the reaction proceeds until equilibrium is reached. Conversely, if Q > K at the start, it will increase until equilibrium is achieved.

So, the correct answer is option C) The reaction starts with Q < K as the reaction proceeds, and Q decreases until equilibrium is reached (where Q = K).