EMF of a Cell — Prelims Questions

Given the standard reduction potentials: \n$E^\circ_{\text{Fe}^{3+}/\text{Fe}^{2+}} = +0.77 \text{ V}$ \n$E^\circ_{\text{Sn}^{4+}/\text{Sn}^{2+}} = +0.15 \text{ V}$ \nCalculate the standard EMF of the cell formed by combining these two half-cells and identify the anode and cathode.

For the reaction $2\text{Ag}^+(\text{aq}) + \text{Cd}(\text{s}) \rightarrow 2\text{Ag}(\text{s}) + \text{Cd}^{2+}(\text{aq})$, the standard cell potential $E_{\text{cell}}^\circ$ is $+1.20 \text{ V}$. What is the standard Gibbs free energy change ($\Delta G^\circ$) for this reaction? (Given: $F = 96485 \text{ C mol}^{-1}$)

For a galvanic cell, which of the following statements is TRUE regarding EMF?

A cell is constructed with two hydrogen electrodes. The first electrode has [H$^+$] = 1.0 M and $P_{\text{H}_2}$ = 1.0 atm. The second electrode has [H$^+$] = 0.1 M and $P_{\text{H}_2}$ = 1.0 atm. Calculate the EMF of this concentration cell at 298 K.

Which of the following factors does NOT affect the EMF of an electrochemical cell?

The EMF of a cell is related to the Gibbs free energy change ($\Delta G$) by the equation $\Delta G = -nFE_{\text{cell}}$. For a spontaneous reaction, which of the following conditions must be met?