## Calculating standard cell potentials

Kate_Santoso_4F
Posts: 72
Joined: Fri Sep 28, 2018 12:29 am

### Calculating standard cell potentials

I thought that one of the half reactions must be reversed to form a redox reaction. Why is it that for a majority of the homework problems, the standard reduction potential for the anode, does not change signs when calculating the standard reduction potential for the cell? For example, for part a for Problem 14.13 in the Sixth edition, the standard reduction potential for Zn2+ (aq) + 2e- --> Zn(s) is -0.76V. When we calculate the standard reduction potential for the cell, why don't we flip the sign to +0.76V since you must reverse the anode reaction?

emily gao 1C
Posts: 61
Joined: Fri Sep 28, 2018 12:29 am

### Re: Calculating standard cell potentials

bc youre doing the method of e standard = e (cathode) - e (anode). the negative sign is built into the equation.

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