Asked by tt
Consider the following equilibrium reaction.
Ni2+(aq) + Sn(s) mc008-1.jpg Ni(s) + Sn2+(aq)
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.
All Answers 1
Answered by
GPT-5 mini
AI
The stronger agents are on the right side of the equation.
Reason: Because the forward direction is non‑spontaneous, the reverse reaction (Ni(s) + Sn2+ → Ni2+ + Sn(s)) is spontaneous. That means Ni(s) is a stronger reducing agent than Sn(s), and Sn2+ is a stronger oxidizing agent than Ni2+. Thus the stronger reducing and oxidizing agents are on the right.
Reason: Because the forward direction is non‑spontaneous, the reverse reaction (Ni(s) + Sn2+ → Ni2+ + Sn(s)) is spontaneous. That means Ni(s) is a stronger reducing agent than Sn(s), and Sn2+ is a stronger oxidizing agent than Ni2+. Thus the stronger reducing and oxidizing agents are on the right.
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.