Nernst Equation — MCQ Practice

Calculate the electrode potential of a zinc electrode dipped in $0.01\,\text{M}$ $ZnSO_4$ solution at $25^{\circ}\text{C}$. Given $E^{\circ}_{Zn^{2+}/Zn} = -0.76\,\text{V}$.

For the cell $Cu(s)|Cu^{2+}(aq, 0.1M)||Ag^+(aq, 0.01M)|Ag(s)$ at $298\,\text{K}$, calculate the cell potential. Given $E^{\circ}_{Cu^{2+}/Cu} = +0.34\,\text{V}$ and $E^{\circ}_{Ag^+/Ag} = +0.80\,\text{V}$.

At what concentration of $Cu^{2+}$ will the electrode potential of a copper electrode be $0.28\,\text{V}$ at $298\,\text{K}$? Given $E^{\circ}_{Cu^{2+}/Cu} = +0.34\,\text{V}$.

Which of the following statements about the Nernst equation is INCORRECT?

For the reaction $2Cr(s) + 3Cd^{2+}(aq) \rightarrow 2Cr^{3+}(aq) + 3Cd(s)$, if $E^{\circ}_{cell} = 0.34\,\text{V}$ and the concentrations are $[Cr^{3+}] = 0.1\,\text{M}$ and $[Cd^{2+}] = 0.001\,\text{M}$ at $298\,\text{K}$, what is the cell potential?

For a reaction, $E^{\circ}_{cell} = 0.0592\,\text{V}$ at $298\,\text{K}$ and $n=1$. What is the equilibrium constant ($K_{eq}$) for this reaction?

If the temperature of an electrochemical cell increases, how does the cell potential ($E_{cell}$) generally change according to the Nernst equation, assuming $Q > 1$ and $E^{\circ}_{cell}$ is positive?