nernst equn and electrochemical cells

Murmur | 22:40 Sun 06th May 2012 | Science

3 Answers

Hello!
If you have and cell where both electrodes are Ag(s) and in one half there are 2M Ag+(aq) and on the other, .1M Ag+(aq), what is the cell potential at 298K?

I know
Ecell = Ecell{at STP} - [25.693mV{at 298K}/(mol e-)]Ln(Q)

but my problem is as follows:

Do I use the equation {Ag+(aq) + e- -> Ag(s) + .8V} or its opposite?

prev

George Foreman Grill Plates

next

Some become smarter as they age?

Answers

1 to 3 of 3

Best Answer

No best answer has yet been selected by Murmur. Once a best answer has been selected, it will be shown here.

For more on marking an answer as the "Best Answer", please visit our FAQ.

I have no idea what you are asking about but this might help

http://en.wikipedia.org/wiki/Nernst_equation

Murmur

Question Author

thanks- i do have the internet at my disposal already.

Murmur

Question Author

i think cells naturally create positive voltage, in which case Ag+ + e- -> Ag + .8V and E^0 is 1.6?

1 to 3 of 3

Do you know the answer?

nernst equn and electrochemical cells

Answer Question >>

Related Questions

Sorry, we can't find any related questions. Try using the search bar at the top of the page to search for some keywords, or choose a topic and submit your own question.