Consider the figure and answer the following questions.

(i) Cell 'A' has `E_(cell)2V and` cell 'B' has `E_(cell)=1.1V` which of the two cells '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 reaction at anode and cathode ?

Explanation

(i) Cell .B. will act as electrolytic cell as it has lower emf
`therefore` The electrode reactions will be:
Reduction at cathode : `Zn^(2+)+2e^(-) to Zn`
Oxidation at anode : `Cu to Cu^(2+) +2e^(-)`
(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 cahotde : `CutoCu^(2+)+2e^(-)`