Question

What is the overall cell potential for this redox reaction?

Answer 1

$Eºcell = Eºcathode - Eºanode = -2.87 -(-2.90) = 0.03 V$

Answer 2

Explanation:

It is known that in an electrochemical cell, chemical reaction occurring at the electrodes generates a potential difference.

In an electrochemical cell, oxidation process occurs at anode and reduction process occurs at cathode.

For example, $Ba^{+} + Ca^{2+} \rightarrow Ba^{2+} + Ca$

Cathode: $Ca^{2+} + 2e^{-} \rightarrow Ca$

Anode : $2Ba^{+} \rightarrow Ba^{2+} + 2e^{-}$

Also, it is known that when more negative is the value of $E^{o}$ more easily an atom can lose electrons. Hence, oxidation will occur where $E^{o}$ value is more negative.

Thus, calculate the overall cell potential as follows.

                         $E^{o}$ = $E^{o}_{cathode}$ - $E^{o}_{anode}$

                               = [-2.87 - (-2.90)] V

                               = 0.03 V

Thus, we can conclude that overall cell potential for the given redox reaction is 0.03.