<P> where F is the Faraday constant, R is the gas constant and T is the temperature in kelvins . For the Daniell cell K is approximately equal to 1.5 × 10 . Thus, at equilibrium, a few electrons are transferred, enough to cause the electrodes to be charged . </P> <P> Actual half - cell potentials must be calculated by using the Nernst equation as the solutes are unlikely to be in their standard states, </P> <Dl> <Dd> E half - cell = E 0 − R T n F ln e ⁡ Q (\ displaystyle E_ (\ text (half - cell)) = E ^ (0) - (\ frac (RT) (nF)) \ ln _ (e) Q) </Dd> </Dl> <Dd> E half - cell = E 0 − R T n F ln e ⁡ Q (\ displaystyle E_ (\ text (half - cell)) = E ^ (0) - (\ frac (RT) (nF)) \ ln _ (e) Q) </Dd>

What happens to the anode in an electrochemical cell