AP Chemistry
9.10 Cell Potential Under Nonstandard Conditions
9.9 Cell Potential and Free Energy
9.8 Galvanic (Voltaic) and Electrolytic Cells
9.5 Free Energy and Equilibrium
9.3 Gibbs Free Energy and Thermodynamic Favorability
A galvanic cell is constructed under standard conditions at \(298\text{ K}\) using a nickel electrode immersed in a \(1.0\text{ M }\text{Ni(NO}_3)_2(aq)\) solution and a silver electrode immersed in a \(1.0\text{ M }\text{AgNO}_3(aq)\) solution, connected by a salt bridge and an external circuit. The overall cell reaction is represented by the following equation.
\[ \text{Ni}(s) + 2\text{Ag}^+(aq) \rightleftharpoons \text{Ni}^{2+}(aq) + 2\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]
As the cell operates and current flows through the circuit, the measured cell potential \(E_{\text{cell}}\) decreases over time until the voltmeter reads \(0.00\text{ V}\). Which of the following statements best explains why the cell potential reaches \(0.00\text{ V}\)?
\[ \text{Ni}(s) + 2\text{Ag}^+(aq) \rightleftharpoons \text{Ni}^{2+}(aq) + 2\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]
As the cell operates and current flows through the circuit, the measured cell potential \(E_{\text{cell}}\) decreases over time until the voltmeter reads \(0.00\text{ V}\). Which of the following statements best explains why the cell potential reaches \(0.00\text{ V}\)?
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