# Nernst Equation Problem

• pzona
In summary, this problem is homework from a lab I did yesterday. Normally I would just ask my TA, but since it's homework I can't. I could email him, but I feel like I'll probably get a faster response if I post this here.f

#### pzona

This problem is homework from a lab I did yesterday. Normally I would just ask my TA, but since it's homework I can't. I could email him, but I feel like I'll probably get a faster response if I post this here

## Homework Statement

Use the Nernst equation to determine the cell potential for the cell involving Ag+. This is from a voltaic cell I made using a copper anode and CuSO4 solution and a silver cathode and AgNO3, with a KNO3 solution as a salt bridge. I used a multimeter to calculate the cell potentials for other cells I built (using other metal cathodes and relevant solutions) because their concentrations were 1M, standard conditions. The AgNO3 was 0.1M so I need to use the Nernst equation to calculate cell potential (assuming all other factors, ex. temperature were standard).

Measured potential for the cell: -0.390V
Given oxidation potential for the copper half reaction: +0.34V

## Homework Equations

The Nernst Equation:

E$$_{cell}$$ = E$$^{o}$$$$_{cell}$$ + 0.0592V(mol)/n * log$$_{10}$$Q

Half reaction at the cathode:

Ag+(aq) + e- -> Ag(s), since [Ag+] = 0.1M, Q and n will both be 0.1

## The Attempt at a Solution

Honestly, this comes down to me not understanding what the terms mean. I just started electrochemistry and I haven't been able to find a decent explanation of the terms online.

I'm not sure whether I need to solve for E$$^{o}$$$$_{cell}$$ (I did and got -0.982V) or E$$_{cell}$$ (I got +0.202V). Solving for E$$^{o}$$$$_{cell}$$ makes more sense, given my answer, since I know that silver is a poor reducing agent. It should give a negative answer of fairly high magnitude in relation to the other cells, which it did.

Basically what I'm asking is, E$$^{o}$$$$_{cell}$$ is the quantity I'm looking for...right? Is E$$_{cell}$$ the measured potential for a cell under non-standard conditions? Also, is my answer for E$$^{o}$$$$_{cell}$$ of a reasonable magnitude? Thanks.

EDIT: Looks like my subscripts were messed up somehow. I'm pretty sure you'll be able to figure out what I meant though.

No, you are looking for Ecell of a silver half cell. E0cell you can take from standard potential tables.

Q is 0.1, that's OK, but n is not.

Once you have Ecell of silver half cell, you can calculate E for whole cell.

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methods

Okay, so for the whole cell, n would be 1.1 mol then? My lab manual says that n is the total amount (in moles) of electrons transferred, so I just add the 0.1 to the 1 from the CuSO4, correct?

No, n is amount of electrons transferred in the half cell reaction. It is always an integer.

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Ah okay, looking back on it that makes a lot more sense than what I have. Thanks a lot for the help.