E cell spontaneity

[Alondra Olmos 4C]

When E(cell) is less than 0, the reverse cell reaction is spontaneous. Is it valid to say that the “forward reaction is not spontaneous”

[LorenzoDuvergne3I]

Yes, it is. The forward reaction would be an electrolytic cell while the reverse would be a galvanic cell.

[Jayasuriya Senthilvelan 4I]

Yes it would be valid to say that. E cell > 0 (when we input it into -nFE) gives us a negative delta G meaning the forward reaction is spontaneous. When E cell < 0, the same equation will give us a positive delta G, meaning the forward reaction is not favored, but the reverse reaction is (the forward reaction is not spontaneous, but the reverse reaction is).

Hope that helps!

[Jonny Schindler 1A]

Is there a quick way to assume the sign of the Ecell?

[Saachi_Kotia_4E]

Is there a quick way to assume the sign of the Ecell?

if I understand your question correctly, you can determine the sign of Ecell depending on whether or not the reaction is spontaneous. so if G for the reaction is negative, Ecell is positive and vice versa. and if the reaction favors the products (K>1) then the Ecell is positive, and vice versa.

[Jennifer Su 2L]

Since deltaG=-nFE, the reaction is spontaneous in the forward direction when deltaG is negative, which happens when E is positive. On the other hand, the reaction is spontaneous in the reverse direction when deltaG is positive, which happens when E is negative.