E°Cu2+/Cu = +0.34\ V; E°Zn2+/Zn = -0.76\ V Identify the incorrect statement from the options below for the above cell:

Strategy: Analyze the behavior of a Daniel cell under an \texternal opposing potential ($E_{\text{ext}}$). Transition from galvanic to equilibrium to electrolytic behavior at critical voltage levels.

Cell Analysis ($E^\circ = 1.1 \text{ V}$):

1. $E_{\text{ext}} < 1.1 \text{ V}$: Normal galvanic operation. Zn dissolves (Anode) and Cu deposits (Cathode). Statement (c) is correct.
2. $E_{\text{ext}} = 1.1 \text{ V}$: System at equilibrium. No chemical change or current. Statement (d) is correct.
3. $E_{\text{ext}} > 1.1 \text{ V}$: Electrolytic operation. The reaction reverses. Cu dissolves (now Anode) and Zn deposits (now Cathode). Electrons flow from Cu to Zn. Statement (a) is correct.

The Incorrect Statement: Statement (b) claims that if $E_{\text{ext}} > 1.1 \text{ V}$, Zn dissolves and Cu deposits. This is the forward (galvanic) reaction, not the reverse electrolytic one.

$\boxed{\text{Answer: (b) If } E_{\text{ext}} > 1.1\text{ V, Zn dissolves at Zn electrode and Cu deposits at Cu electrode}}$