Question

Assertion :For a Daniell cell :
$Zn|Z{n}^{2+}||C{u}^{2+}|Cu$ with $E_{cell}=1.1V$
the application of opposite potential greater than 1.1 V results into the flow of electrons from cathode an anode. Reason: Zn is deposited at anode and Cu is dissolved at cathode.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Assertion is incorrect but Reason is correct

Answer 1

The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

Both (A) and (R) are correct but (R) is not the correct explanation of (A) .

Correct explanation: On applying an external voltage greater than 1.1 V in a Daniell cell, the current flows in the reverse direction i.e., from Zn to Cu (cathode to anode) and electrons flow from Cu and Zn.

Zn is deposited at Zn electrode and Cu dissolves at Cu electrode. The reaction is:
$Z{n}^{2+}+Cu\to Zn+C{u}^{2+}$