Statement A: For the Daniell cell $Zn | {Zn}^{2 +} | | {Cu}^{2 +} | Cu$ with $E_{cell} = 1 .1 V$ ,
the application of opposite potential greater than 1.1 V results into flow of electron from Cu(cathode) to Zn(anode).
Statement B: Zn is deposited at anode and Cu is dissolved at cathode.

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Both Statement A and Statement B are false

Statement A is true but Statement B is false.

Statement A is false but Statement B is true.

Both Statement A and Statement B are true

answer is A.

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Detailed Solution

On applying an external voltage greater than 1.1 V in a Daniel cell,the current flows from Zn to Cu

and electrons flow from Cu to Zn

Zn is deposited at Zn electrode and Cu dissolves at Cu electrode.

The reaction is,

${Zn}^{+ 2} + Cu \to Zn + {Cu}^{+ 2}$

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