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.

पर्याय

• 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.

Answer 1

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.