Consider the figure and answer the following question.

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

Explanation

(i) Cell 'B' act as electrolytic cell due to its lesser value of emf.
The electrode reactions will be
At cathode `Zn^(2+)+2e^(-)rarrZn`
At anode `CurarrCu^(2+)+2e^(-)`
(ii) If cell 'B' are higher emf, it acts as galvanic cell. Now it will push electrons into cell 'A'
In this case, the reactions will be
`ZnrarrZn^(2+)+2e^(-)` (At anode)
`Cu^(2+)+2e^(-)rarrCu`(At cathode)