## equation for Q

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

Savannah Mance 4G
Posts: 107
Joined: Fri Aug 30, 2019 12:17 am

### equation for Q

Is the equation for Q from the cell diagram always going to be the anode over the electrode? Like for 6N.1 in the textbook with the rxn Mn(s)+Ti^2+---->Mn^2+ +Ti(s)? Or is it just like you'd normally do Q with products over reactants?

Aiden Metzner 2C
Posts: 104
Joined: Wed Sep 18, 2019 12:21 am

### Re: equation for Q

Yes for Q the anode is always over the cathode. It is very confusing because you would think it would be cathode over anode but in the case of the nernst equation it is the opposite

Lauren Tanaka 1A
Posts: 109
Joined: Sat Aug 17, 2019 12:18 am

### Re: equation for Q

It will always be the anode over the cathode since the equation for Q is products over reactants. The products of the equation will be the anode concentration and the cathode concentration will be the reactants.

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Re: equation for Q

And this is also the case since you do not consider solids for equilibrium?

Return to “Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)”

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