<P> where Q is the reaction quotient . This simplifies to </P> <Dl> <Dd> E half - cell = E 0 − 2.303 R T n F log 10 ⁡ (M n +) (\ displaystyle E_ (\ text (half - cell)) = E ^ (0) - 2.303 (\ frac (RT) (nF)) \ log _ (10) \ (M ^ (n+) \)) </Dd> </Dl> <Dd> E half - cell = E 0 − 2.303 R T n F log 10 ⁡ (M n +) (\ displaystyle E_ (\ text (half - cell)) = E ^ (0) - 2.303 (\ frac (RT) (nF)) \ log _ (10) \ (M ^ (n+) \)) </Dd> <P> where (M) is the activity of the metal ion in solution . The metal electrode is in its standard state so by definition has unit activity . In practice concentration is used in place of activity . The potential of the whole cell is obtained by combining the potentials for the two half - cells, so it depends on the concentrations of both dissolved metal ions . </P>

In an electrochemical cell the anode is quizlet