## 14.41b

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

Abigail Urbina 1K
Posts: 102
Joined: Thu Jul 27, 2017 3:01 am

### 14.41b

How do we know that the standard cell potential is 0 in this particular problem?

Tim Foster 2A
Posts: 73
Joined: Fri Sep 29, 2017 7:07 am

### Re: 14.41b

Hey! To find the standard cell potential, we extrapolate oxidation and reduction half reactions from the cell diagram, from the left and right sides, respectively. Once we have these half rxns, we can use our handy dandy chart in Appendix 2B to search for standard reduction potentials (subtracting the anode's from the cathode's). For 41 b, our oxidation and reduction half rxns are the same (only flipped) because both solely involve H2 and H+. Thus standard reduction potentials for the anode and the cathode are the same, and if Cathode = Anode Then Cathode - Anode = 0. It's also handy to know that the standard reduction potential of 2H+ => H2 is 0. The standard cell potential for this problem is equal to 0 - 0 (which , surprisingly enough, is still 0.) Hope this made at least a little sense!

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