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AP Chemistry
9.10 Cell Potential Under Nonstandard Conditions
IntermediateMCQProportional AnalysisConceptual24.5k
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.
Galvanic cell constructed with zinc and copper half-cells at \(298\text{ K}\).
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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