Kim W.

asked • 11/11/23

Nernst equation chemistry of electrochemical cell

Calculate the reaction constant of an electrochemical cell at 298K using the Nernst equation. All concentrations of ions are standard at 1.00M:


1.) Ca +Cu^+2 < Ca^+2 + Cu



( I am not sure which Nernst equation to use such as

Ecell= Eocell -0.0592/n log Q or Eocell = RT/nF lnK ?)

J.R. S.

tutor
The two equations you are considering using are the same. The first one has already included the Faraday constant and has converted natural log (lnQ) to base 10 log (log Q). Easiest to use the first one: Ecell = Eºcell - 0.0592/n log Q. Use K in place of Q since concentration is 1.00 M and solve for K. If you have a problem, reply to this message, and I&apos;ll help you.
Report

11/11/23

Anthony T.

At equilibrium, Ecell = 0, so the first equation becomes Eocell = 0.0592/n log K which is the second equation before converting to Log base 10.
Report

11/12/23

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