<Dd> E half - cell = E 0 − 0.05918 V n log 10 ⁡ (M n +) (\ displaystyle E_ (\ text (half - cell)) = E ^ (0) - (\ frac (0.05918 V) (n)) \ log _ (10) (M ^ (n+))) </Dd> <P> These calculations are based on the assumption that all chemical reactions are in equilibrium . When a current flows in the circuit, equilibrium conditions are not achieved and the cell potential will usually be reduced by various mechanisms, such as the development of overpotentials . Also, since chemical reactions occur when the cell is producing power, the electrolyte concentrations change and the cell voltage is reduced . A consequence of the temperature dependency of standard potentials is that the voltage produced by a galvanic cell is also temperature dependent . </P> <P> Galvanic corrosion is a process that degrades metals electrochemically . This corrosion occurs when two dissimilar metals are located in contact with each other in the presence of an electrolyte, such as salt water, forming a galvanic cell . A cell can also be formed if the same metal is exposed to two different concentrations of electrolyte . The resulting electrochemical potential then develops an electric current that electrolytically dissolves the less noble material . </P> <Ul> <Li> Concentration cell </Li> <Li> Electrolytic cell </Li> <Li> Electrochemical cell </Li> <Li> Lemon battery </Li> <Li> Thermogalvanic cell </Li> </Ul>

Which one of the following is consistent with a galvanic cell