Questions: Which of the following statements is true concerning the hypothetical electrochemical cell depicted below? (M1 and M2 are differing metals)
M1M^2+(aq) M^+(aq)M2
M^2+(aq)+2e^- M1(s) ; E°=-2.91 V
M^2+(aq)+e^- M2(s) ; E°=-2.98 V
The cell reaction is spontaneous with a standard cell potential of 0.07 V.
The cell reaction is nonspontaneous with a standard cell potential of -0.07 V.
The cell reaction is spontaneous with a standard cell potential of 5.89 V.
The cell is at equilibrium.
The cell reaction is nonspontaneous with a standard cell potential of -5.89 V.
Transcript text: Which of the following statements is true concerning the hypothetical electrochemical cell depicted below? (M1 and M2 are differing metals)
\[
\begin{array}{l}
\mathrm{M} 1\left|\mathrm{M}^{2+}(a q) \| \mathrm{M}^{+}(a q)\right| \mathrm{M} 2 \\
\mathrm{M}^{2+}(a q)+2 \mathrm{e}^{-} \mathrm{M} 1(s) ; E^{\circ}=-2.91 \mathrm{~V} \\
\mathrm{M}^{2+}(a q)+\mathrm{e}^{-} \mathrm{M} 2(s) ; E^{\circ}=-2.98 \mathrm{~V}
\end{array}
\]
The cell reaction is spontaneous with a standard cell potential of 0.07 V .
The cell reaction is nonspontaneous with a standard cell potential of -0.07 V .
The cell reaction is spontaneous with a standard cell potential of 5.89 V .
The cell is at equilibrium.
The cell reaction is nonspontaneous with a standard cell potential of -5.89 V .
Solution
Solution Steps
Step 1: Identify the Half-Reactions and Their Potentials
The given half-reactions and their standard electrode potentials are: