## E cell spontaneity

Alondra Olmos 4C
Posts: 32
Joined: Fri Sep 28, 2018 12:21 am

### E cell spontaneity

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
Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

### Re: E cell spontaneity

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

Jayasuriya Senthilvelan 4I
Posts: 31
Joined: Thu Jan 10, 2019 12:17 am

### Re: E cell spontaneity

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
Posts: 30
Joined: Fri Sep 28, 2018 12:20 am

### Re: E cell spontaneity

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

Saachi_Kotia_4E
Posts: 68
Joined: Fri Sep 28, 2018 12:23 am

### Re: E cell spontaneity

Jonny Schindler 1A wrote: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
Posts: 47
Joined: Wed Nov 21, 2018 12:20 am

### Re: E cell spontaneity

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.