Consider the figure below and answer the following questions :

(i) Cell 'A' has `E_("cell") = 2V` and Cell 'B' has `E_("cell") = 1.1 V` which of the two cells 'A' or 'B' will act as an electrolytic cell. Which electrode reaction will occur in this cell?
(ii) If cell 'A' has `E_("cell") = 0.5 V` and cell 'B' has `E_("cell") =1.1 V` then what will be the reaction at anode and cathode?

Explanation

(i) Cell .B. will act as electrolytic cell as it has lower emf.
The electrode reactions will be :
`Zn^(2+) + 2e^(-) to Zn` at cathode
`Cu to Cu^(2+) + 2e^(-)` at anode.
(ii) Now cell .B. acts as galvanic cell as it has higher emf and will push electrons into cell .A.. The electrode reaction will be :
`{:("At anode", Zn to Zn^(2+) + 2e^(-)),("At cathode", Cu^(2+) + 2e^(-) to Cu):}`