In a galvanic cell, electrons flow from the metal that is higher in the electrochemical series to the metal that is lower in the series. This flow of electrons results in the higher metal losing electrons (oxidation) and the lower metal gaining electrons (reduction).
In the case of a zinc-copper galvanic cell, zinc is higher in the electrochemical series than copper. Zinc has a greater tendency to lose electrons than copper, therefore, zinc undergoes oxidation and loses electrons in the galvanic cell. Copper, on the other hand, has a lower tendency to lose electrons compared to zinc, so copper does not lose electrons in this cell. Instead, copper undergoes reduction by gaining electrons.
As a result, in the galvanic cell, zinc acts as the anode (where oxidation occurs) and copper acts as the cathode (where reduction occurs). This flow of electrons from zinc to copper produces an electric current in the external circuit.
In galvanic cell,why Zinc lose electrons while cupper not
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