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Question
Assertion: When \[\ce{E{^{\circ}_{cell}}}\] is positive, the cell reaction is feasible and proceeds spontaneously.
Reason: When \[\ce{E{^{\circ}_{cell}}}\] is positive, ΔG° is negative which makes the cell reaction feasible.
Options
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
If both Assertion and Reason are CORRECT but Reason is not the CORRECT explanation of the Assertion.
If Assertion is CORRECT but Reason is INCORRECT.
If Assertion is INCORRECT but Reason is CORRECT.
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Solution
If both Assertion and Reason are CORRECT and Reason is the CORRECT explanation of the Assertion.
Explanation:
When \[\ce{E{^{\circ}_{cell}}}\] is positive, the standard Gibbs free energy change ΔG° is negative \[\ce{(\Delta G^\circ = -nFE{^{\circ}_{cell}})}\]. A negative ΔG° implies that the cell reaction is feasible and proceeds spontaneously.
