---
title: "A galvanic cell is constructed under standard conditions at \\(298\\text{ K}\\) based on the following balanced equation:  \\[ \\text{Cu(s)} + 2\\,\\text{Ag}^+\\text{(aq)} \\rightarrow \\text{Cu}^{2+}\\text{(aq)} + 2\\,\\text{Ag(s)} \\quad E^\\circ_{\\text{cell}} = +0.46\\text{ V} \\]  A student modifies the cell by adding an equal volume of distilled water to both half-cell compartments and stirring thoroughly. Which of the following statements 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/121473/"
date_modified: "2026-08-23T05:04:46+00:00"
---

# A galvanic cell is constructed under standard conditions at \(298\text{ K}\) based on the following balanced equation:

\[ \text{Cu(s)} + 2\,\text{Ag}^+\text{(aq)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +0.46\text{ V} \]

A student modifies the cell by adding an equal volume of distilled water to both half-cell compartments and stirring thoroughly. Which of the following statements best predicts and justifies the effect of this modification on the cell potential, \(E_{\text{cell}}\)?

A galvanic cell is constructed under standard conditions at \(298\text{ K}\) based on the following balanced equation:

\[ \text{Cu(s)} + 2\,\text{Ag}^+\text{(aq)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +0.46\text{ V} \]

A student modifies the cell by adding an equal volume of distilled water to both half-cell compartments and stirring thoroughly. Which of the following statements best predicts and justifies the effect of this modification on the cell potential, \(E_{\text{cell}}\)?

- **A.** \(E_{\text{cell}} > E^\circ_{\text{cell}}\), because diluting both solutions decreases the concentration of the product ion \(\text{Cu}^{2+}\text{(aq)}\), which makes \(Q < 1\).
- **B.** \(E_{\text{cell}} > E^\circ_{\text{cell}}\), because the stoichiometric coefficient of \(\text{Ag}^+\text{(aq)}\) is \(2\), so reducing its concentration creates a larger thermodynamic driving force for the forward reaction.
- **C.** \(E_{\text{cell}} < E^\circ_{\text{cell}}\), because halving the concentrations of both ions results in \(Q > 1\) due to the squared term for \([\text{Ag}^+]\) in the denominator of the reaction quotient.
- **D.** \(E_{\text{cell}} < E^\circ_{\text{cell}}\), because adding water increases the total electrolyte volume, which directly decreases the standard reduction potential \(E^\circ_{\text{cell}}\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121473/*