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title: "A student constructs a galvanic cell at \\(298\\text{ K}\\) using the reaction represented below:  \\[ \\text{Ni(s)} + 2\\,\\text{Ag}^+\\text{(aq)} \\rightarrow \\text{Ni}^{2+}\\text{(aq)} + 2\\,\\text{Ag(s)} \\quad E^\\circ_{\\text{cell}} = +1.06\\text{ V} \\]  The cell is initially operated under standard conditions with \\([\\text{Ni}^{2+}] = 1.0\\text{ M}\\) and \\([\\text{Ag}^+] = 1.0\\text{ M}\\). The student then dilutes the solution in the anode compartment by adding distilled water until \\([\\text{Ni}^{2+}] = 0.010\\text{ M}\\), while maintaining \\([\\text{Ag}^+] = 1.0\\text{ M}\\) at \\(298\\text{ K}\\). Which of the following best predicts how the cell potential, \\(E_{\\text{cell}}\\), changes, and provides the correct justification?"
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date_modified: "2026-08-21T08:17:22+00:00"
---

# A student constructs a galvanic cell at \(298\text{ K}\) using the reaction represented below:

\[ \text{Ni(s)} + 2\,\text{Ag}^+\text{(aq)} \rightarrow \text{Ni}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]

The cell is initially operated under standard conditions with \([\text{Ni}^{2+}] = 1.0\text{ M}\) and \([\text{Ag}^+] = 1.0\text{ M}\). The student then dilutes the solution in the anode compartment by adding distilled water until \([\text{Ni}^{2+}] = 0.010\text{ M}\), while maintaining \([\text{Ag}^+] = 1.0\text{ M}\) at \(298\text{ K}\). Which of the following best predicts how the cell potential, \(E_{\text{cell}}\), changes, and provides the correct justification?

A student constructs a galvanic cell at \(298\text{ K}\) using the reaction represented below:

\[ \text{Ni(s)} + 2\,\text{Ag}^+\text{(aq)} \rightarrow \text{Ni}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]

The cell is initially operated under standard conditions with \([\text{Ni}^{2+}] = 1.0\text{ M}\) and \([\text{Ag}^+] = 1.0\text{ M}\). The student then dilutes the solution in the anode compartment by adding distilled water until \([\text{Ni}^{2+}] = 0.010\text{ M}\), while maintaining \([\text{Ag}^+] = 1.0\text{ M}\) at \(298\text{ K}\). Which of the following best predicts how the cell potential, \(E_{\text{cell}}\), changes, and provides the correct justification?

- **A.** \(E_{\text{cell}}\) decreases because \(Q > 1\), shifting the system closer to equilibrium and reducing the driving force for the forward reaction.
- **B.** \(E_{\text{cell}}\) decreases because diluting the electrolyte decreases the electrical conductivity of the half-cell, directly reducing \(E^\circ_{\text{cell}}\).
- **C.** \(E_{\text{cell}}\) increases because \(Q < 1\), which increases the thermodynamic driving force for the forward reaction relative to standard conditions.
- **D.** \(E_{\text{cell}}\) remains unchanged at \(+1.06\text{ V}\) because cell potential is an intensive property that depends only on the identities of the electrode materials.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119915/*