Measurement of Electrode Potential — Prelims Questions

Which of the following statements about the Standard Hydrogen Electrode (SHE) is INCORRECT?

Given the standard reduction potentials: $E^\circ_{\text{Ag}^+/\text{Ag}} = +0.80\,\text{V}$ and $E^\circ_{\text{Cu}^{2+}/\text{Cu}} = +0.34\,\text{V}$. Calculate the standard cell potential ($E^\circ_{\text{cell}}$) for the galvanic cell formed by these two half-cells.

For the half-reaction $\text{Ni}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Ni}(\text{s})$, the standard electrode potential $E^\circ = -0.25\,\text{V}$. Calculate the electrode potential ($E$) at $298\,\text{K}$ when the concentration of $\text{Ni}^{2+}$ is $0.01\,\text{M}$. (Given: $\log(100) = 2$)

Consider the following standard reduction potentials: $\text{A}^{2+} + 2\text{e}^- \rightarrow \text{A} \quad E^\circ = -2.37\,\text{V}$ $\text{B}^{2+} + 2\text{e}^- \rightarrow \text{B} \quad E^\circ = -0.76\,\text{V}$ $\text{C}^{2+} + 2\text{e}^- \rightarrow \text{C} \quad E^\circ = +0.34\,\text{V}$ Which of the following metals is the strongest reducing agent?

A galvanic cell is constructed using a $\text{Zn}/\text{Zn}^{2+}$ half-cell and a $\text{Ag}/\text{Ag}^+$ half-cell. The standard reduction potentials are $E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76\,\text{V}$ and $E^\circ_{\text{Ag}^+/\text{Ag}} = +0.80\,\text{V}$. If the concentration of $\text{Zn}^{2+}$ is $0.1\,\text{M}$ and $\text{Ag}^+$ is $0.01\,\text{M}$ at $298\,\text{K}$, what is the cell potential ($E_{\text{cell}}$)? (Given: $\log(10) = 1$, $\log(100) = 2$)

Which of the following conditions is NOT considered a standard condition for measuring electrode potential?