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title: "A galvanic cell is constructed at \\(298\\text{ K}\\) using a zinc electrode immersed in a \\(1.0\\text{ M }\\text{Zn(NO}_3)_2(aq)\\) solution and a copper electrode immersed in a \\(1.0\\text{ M }\\text{Cu(NO}_3)_2(aq)\\) solution. The overall cell reaction is represented below.  \\[\\text{Zn}(s) + \\text{Cu}^{2+}(aq) \\rightarrow \\text{Zn}^{2+}(aq) + \\text{Cu}(s) \\quad E^\\circ_{\\text{cell}} = +1.10\\text{ V}\\]  A student adds \\(100\\text{ mL}\\) of distilled water to the cathode compartment while keeping the anode compartment unchanged. Which of the following best predicts and explains the effect of this change on the cell potential, \\(E_{\\text{cell}}\\)?"
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date_modified: "2026-08-21T08:16:59+00:00"
---

# A galvanic cell is constructed at \(298\text{ K}\) using a zinc electrode immersed in a \(1.0\text{ M }\text{Zn(NO}_3)_2(aq)\) solution and a copper electrode immersed in a \(1.0\text{ M }\text{Cu(NO}_3)_2(aq)\) solution. The overall cell reaction is represented below.

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

A student adds \(100\text{ mL}\) of distilled water to the cathode compartment while keeping the anode compartment unchanged. Which of the following best predicts and explains the effect of this change on the cell potential, \(E_{\text{cell}}\)?

A galvanic cell is constructed at \(298\text{ K}\) using a zinc electrode immersed in a \(1.0\text{ M }\text{Zn(NO}_3)_2(aq)\) solution and a copper electrode immersed in a \(1.0\text{ M }\text{Cu(NO}_3)_2(aq)\) solution. The overall cell reaction is represented below.

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

A student adds \(100\text{ mL}\) of distilled water to the cathode compartment while keeping the anode compartment unchanged. Which of the following best predicts and explains the effect of this change on the cell potential, \(E_{\text{cell}}\)?

![A grayscale schematic diagram of a standard galvanic cell. On the left, a beaker labeled anode contains a submerged solid rectangle labeled Zn(s) in a liquid labeled 1.0 M Zn(NO3)2(aq). On the right, a beaker labeled cathode contains a submerged solid rectangle labeled Cu(s) in a liquid labeled 1.0 M Cu(NO3)2(aq). An inverted U-tube salt bridge connects the two solutions. A single wire connects the top of the Zn(s) electrode to the top of the Cu(s) electrode through a central circle labeled V. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787300218-cYYjjF.jpg)

- **A.** \(E_{\text{cell}}\) decreases because \([\text{Cu}^{2+}]\) decreases, which increases the value of \(Q\) and reduces the thermodynamic driving force for the forward reaction.
- **B.** \(E_{\text{cell}}\) increases because \([\text{Cu}^{2+}]\) decreases, which shifts the equilibrium toward the products to replace consumed ions.
- **C.** \(E_{\text{cell}}\) increases because adding water dilutes the solution and decreases the value of \(Q\), resulting in a larger cell voltage.
- **D.** \(E_{\text{cell}}\) remains unchanged because the standard reduction potentials of \(\text{Zn}^{2+}\) and \(\text{Cu}^{2+}\) depend only on the identity of the electrodes.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119880/*