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title: "A student constructs a galvanic cell under standard conditions at \\(298\\text{ K}\\) using the overall reaction shown below:  \\[ \\text{Zn(s)} + \\text{Cu}^{2+}\\text{(aq)} \\rightarrow \\text{Zn}^{2+}\\text{(aq)} + \\text{Cu(s)} \\quad E^\\circ_{\\text{cell}} = +1.10\\text{ V} \\]  The cell is initially operated with \\(100\\text{ mL}\\) of \\(1.0\\text{ M }\\text{Zn(NO}_3)_2\\text{(aq)}\\) in the anode compartment and \\(100\\text{ mL}\\) of \\(1.0\\text{ M }\\text{Cu(NO}_3)_2\\text{(aq)}\\) in the cathode compartment. The student then adds \\(100\\text{ mL}\\) of distilled water to the anode compartment while keeping the cathode compartment unchanged. Which of the following best predicts and justifies the effect of this modification on the cell potential, \\(E_{\\text{cell}}\\)?"
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url: "https://nerd-notes.com/ubq/121402/"
date_modified: "2026-08-23T05:02:06+00:00"
---

# A student constructs a galvanic cell under standard conditions at \(298\text{ K}\) using the overall reaction shown below:

\[ \text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)} \quad E^\circ_{\text{cell}} = +1.10\text{ V} \]

The cell is initially operated with \(100\text{ mL}\) of \(1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}\) in the anode compartment and \(100\text{ mL}\) of \(1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}\) in the cathode compartment. The student then adds \(100\text{ mL}\) of distilled water to the anode compartment while keeping the cathode compartment unchanged. Which of the following best predicts and justifies the effect of this modification on the cell potential, \(E_{\text{cell}}\)?

A student constructs a galvanic cell under standard conditions at \(298\text{ K}\) using the overall reaction shown below:

\[ \text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)} \quad E^\circ_{\text{cell}} = +1.10\text{ V} \]

The cell is initially operated with \(100\text{ mL}\) of \(1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}\) in the anode compartment and \(100\text{ mL}\) of \(1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}\) in the cathode compartment. The student then adds \(100\text{ mL}\) of distilled water to the anode compartment while keeping the cathode compartment unchanged. Which of the following best predicts and justifies the effect of this modification on the cell potential, \(E_{\text{cell}}\)?

- **A.** \(E_{\text{cell}}\) decreases because decreasing \([\text{Zn}^{2+}]\) shifts the equilibrium toward the reactants, which makes \(\Delta G\) less negative.
- **B.** \(E_{\text{cell}}\) decreases because diluting the anode compartment causes \(Q > 1\), which reduces the cell potential toward zero as the system approaches equilibrium.
- **C.** \(E_{\text{cell}}\) increases because decreasing \([\text{Zn}^{2+}]\) causes \(Q < 1\), which makes \(\Delta G\) more negative and increases the driving force for the forward reaction.
- **D.** \(E_{\text{cell}}\) increases because decreasing \([\text{Zn}^{2+}]\) increases the value of \(E^\circ_{\text{cell}}\), which increases the maximum electrical work the cell can perform under standard conditions.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121402/*