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Which of these is/are TRUE about a spontaneous electrochemical reaction: i. Δg > 0 ii. Δg < 0 iii. -nfe⁰cell < 0 iv. E⁰cell < 0 v. They are not feasible and require electricity to proceed
Accepted Answer
Here are the TRUE statements about a spontaneous electrochemical reaction:
II. ΔG < 0: Spontaneous reactions have a negative Gibbs Free Energy change (ΔG), indicating they release energy.
III. -nFE⁰cell < 0: The equation ΔG = -nFE⁰cell relates Gibbs Free Energy to cell potential (E⁰cell). A negative ΔG means the cell potential (E⁰cell) must be positive.
Explanation:
I. ΔG > 0: This is incorrect. A positive ΔG indicates a non-spontaneous reaction that requires energy input.
IV. E⁰cell < 0: This is incorrect. A positive E⁰cell signifies a spontaneous reaction.
V. They are not feasible and require electricity to proceed: This is incorrect. Spontaneous reactions occur without external energy input; they release energy.
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