what is the cell reactions of dry cell

Dear student,

In the most common type of dry cell battery, the cathode is composed of a form of elemental carbon called graphite, which serves as a solid support for the reduction half-reaction. In an acidic dry cell, the reduction reaction occurs within the moist paste comprised of ammonium chloride (NH₄Cl) and manganese dioxide (MnO₂):

   2 NH4+  +  2 MnO2  +  2e-  ------>  Mn2O3  +  2 NH3  +  H2O

A thin zinc cylinder serves as the anode and it undergoes oxidation:

   Zn (s)  --------------->  Zn+2  +  2e-

This dry cell "couple" produces about 1.5 volts. ( These "dry cells" can also be linked in series to boost the voltage produced). In the alkaline version or "alkaline battery", the ammonium chloride is replaced by KOH or NaOH and the half-cell reactions are:

       Zn  +     2 OH-     ------->  ZnO    +  H2O    +  2e-
   2 MnO2  +  2e-  +  H2O  ------->  Mn2O3  +  2 OH-

The alkaline dry cell lasts much longer as the zinc anode corrodes less rapidly under basic conditons than under acidic conditions.

Other types of dry cell batteries are the silver battery in which silver metal serves as an inert cathode to support the reduction of silver oxide (Ag₂O) and the oxidation of zinc (anode) in a basic medium. The type of battery commonly used for calculators is the mercury cell. In this type of battery, HgO serves as the oxidizing agent (cathode) in a basic medium, while zinc metal serves as the anode. Another type of battery is the nickel/cadmium battery, in which cadmium metal serves as the anode and nickel oxide serves as the cathode in an alkaline medium. Unlike the other types of dry cells described above, the nickel/cadmium cell can be recharged like the lead-acid battery.