Answer
See the explanation
Work Step by Step
$Electrochemical- cell$
$(a)$ A Galvanic cell converts chemical energy into electrical energy.
$(b)$ The redox reaction is spontaneous and is responsible for the production of electrical energy.
$(c)$The two half-cells are set up in different containers, being connected through the salt bridge or porous partition.
$(d)$ The anode is negative and cathode is the positive electrode. The reaction at the anode is oxidation and that at the cathode is reduction.
$(e)$The electrons are supplied by the species getting oxidized. They move from anode to the cathode in the external circuit.
$Electrolytic-cell$
$(a)$ An electrolytic cell converts electrical energy into chemical energy.
$(b)$ The redox reaction is not spontaneous and electrical energy has to be supplied to initiate the reaction.
$(c)$ Both the electrodes are placed in a same container in the solution of molten electrolyte.
$(d)$ The anode is positive and cathode is the negative electrode. The reaction at the anode is oxidation and that at the cathode is reduction.
$(e)$ The external battery supplies the electrons. They enter through the cathode and come out through the anode.
