Question

Consider the following equilibrium reaction.

(PIC BELOW)

The forward reaction is non-spontaneous. What does this indicate about the relative strengths of the reducing and oxidizing agents on each side of the equation?
The agents are of equal strength on both sides of the equation.
The stronger agents are on the left side of the equation.
The stronger agents are on the right side of the equation.
The relative strengths of the agents cannot be inferred.

Answer 1

Answer: The stronger agents are on the right side of the equation.

That is because the stronger the reactiivity of the compounds the further the reaction goes. So, if the products of the right side have stronger reactivity the equation will spontaneously proceed to the left which is the backward reaction.