Question

Two statements are given about the galvanic cell shown below
Statement I: Current flows from Cu electrode to Zn electrode
Statement II: With increase in time the mass of Zn electrode increases and mass of Cu electrode decreases
Correct answer is

• A. Both statements I and II are correct
• B. Both statements I and II are not correct
• C. Statement I is correct and statement II is not correct
• D. Statement I is not correct and statement II is correct

Hint:

Remember:
If $E_{\text{ext}} \lt 1.1\text{ V}$, the cell acts as a galvanic cell (Zn is anode, Cu is cathode).
If $E_{\text{ext}} = 1.1\text{ V}$, no reaction occurs and no current flows.
If $E_{\text{ext}} \gt 1.1\text{ V}$, the cell reactions are reversed and it behaves as an electrolytic cell (Cu is anode, Zn is cathode).

Answer 1

The Correct Option is C

Step 1: Fix the anode and cathode first.
In this Zn-Cu cell, zinc gets oxidised at the anode, $\text{Zn} \to \text{Zn}^{2+} + 2e^-$, and copper gets reduced at the cathode, $\text{Cu}^{2+} + 2e^- \to \text{Cu}$.
Step 2: Track electrons before converting to current.
Electrons physically leave the zinc anode and travel through the external wire toward the copper cathode.
Step 3: Flip direction for conventional current.
Conventional current runs opposite to electron flow, so externally it travels from Cu to Zn, exactly matching Statement I, so that part is correct.
Step 4: Check the mass changes.
Zn keeps dissolving away, so its mass drops, while Cu keeps depositing fresh metal, so its mass rises, the reverse of what Statement II claims.
Final answer: Option 3, Statement I is correct and Statement II is not correct.