Combine the equations $$ \Delta G^{\circ}=-n F \mathscr{C}^{\circ} \quad \text { and } \quad \Delta G^{\circ}=\Delta H^{\circ}-T \Delta S^{\circ} $$ to derive an expression for \(\mathscr{E}^{\circ}\) as a function of temperature. Describe how one can graphically determine \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) from measurements of \(\mathscr{E}^{\circ}\) at different temperatures, assuming that \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature. What property would you look for in designing a reference half-cell that would produce a potential relatively stable with respect to temperature?

Short Answer

Expert verified
The expression for \( \mathscr{E}^{\circ} \) as a function of temperature is \( \mathscr{E}^{\circ} = -\frac{\Delta H^{\circ}}{nF} + \frac{T \Delta S^{\circ}}{nF} \). To graphically determine \( \Delta H^{\circ} \) and \( \Delta S^{\circ} \) from measurements of \( \mathscr{E}^{\circ} \) at different temperatures, plot \( \mathscr{E}^{\circ} \) versus temperature (T) and fit the data points to a linear regression. The y-intercept is \( -\frac{\Delta H^{\circ}}{nF} \), and the slope is \( \frac{\Delta S^{\circ}}{nF} \). In designing a reference half-cell with a potential relatively stable with respect to temperature, one would look for a small value of \( \Delta S^{\circ} \) to minimize the temperature dependence of the electromotive force.

Step by step solution

01

Combining The Given Equations

We are given two equations: 1. \( \Delta G^{\circ}=-n F \mathscr{E}^{\circ} \) 2. \( \Delta G^{\circ}=\Delta H^{\circ}-T \Delta S^{\circ} \) To derive an expression for \( \mathscr{E}^{\circ} \), we will first equate the two expressions for \( \Delta G^{\circ} \): \( -n F \mathscr{E}^{\circ} = \Delta H^{\circ} - T \Delta S^{\circ} \) Now, we will solve for \( \mathscr{E}^{\circ} \):
02

Expression for Electromotive Force

Dividing both sides by \( -nF \) and isolating \( \mathscr{E}^{\circ} \), we get: \( \mathscr{E}^{\circ} = -\frac{\Delta H^{\circ}}{nF} + \frac{T \Delta S^{\circ}}{nF} \)
03

Graphically Determining \( \Delta H^{\circ} \) and \( \Delta S^{\circ} \)

To graphically determine \( \Delta H^{\circ} \) and \( \Delta S^{\circ} \) from the measurements of \( \mathscr{E}^{\circ} \) at different temperatures, we can rewrite the expression for \( \mathscr{E}^{\circ} \) in the form of a linear equation: \( \mathscr{E}^{\circ} = -\frac{\Delta H^{\circ}}{nF} + \Big(\frac{\Delta S^{\circ}}{nF}\Big) T \) Here, \( -\frac{\Delta H^{\circ}}{nF} \) is the y-intercept, and \( \frac{\Delta S^{\circ}}{nF} \) is the slope of the line. By plotting \( \mathscr{E}^{\circ} \) versus temperature (T) and fitting the data points to a linear regression, one can determine the slope and y-intercept of the line. With the values of slope and y-intercept, we can calculate \( \Delta H^{\circ} \) and \( \Delta S^{\circ} \) as follows: 1. \( \Delta H^{\circ} = -nF\times \text{y-intercept} \) 2. \( \Delta S^{\circ} = nF\times \text{slope} \)
04

Property for a Reference Half-Cell with Stable Potential

In designing a reference half-cell with a potential relatively stable with respect to temperature, one would look for a property that minimizes the temperature dependence of the electromotive force, \( \mathscr{E}^{\circ} \). From the derived expression: \( \mathscr{E}^{\circ} = -\frac{\Delta H^{\circ}}{nF} + \frac{T \Delta S^{\circ}}{nF} \) A relatively stable potential with respect to temperature could be achieved by minimizing the \( \frac{\Delta S^{\circ}}{nF} \) term, as it directly depends on temperature. So, a reference half-cell with a small value of \( \Delta S^{\circ} \) would lead to a more stable potential with respect to temperature.

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Most popular questions from this chapter

The equation \(\Delta G^{\circ}=-n F \mathscr{E}^{\circ}\) also can be applied to halfreactions. Use standard reduction potentials to estimate \(\Delta G_{\mathrm{f}}^{\circ}\) for \(\mathrm{Fe}^{2+}(a q)\) and \(\mathrm{Fe}^{3+}(a q) .\left(\Delta G_{\mathrm{f}}^{\circ}\right.\) for \(\left.\mathrm{e}^{-}=0 .\right)\)

You have a concentration cell with Cu electrodes and [Cu^{2+} ] \(=1.00 M\) (right side) and \(1.0 \times 10^{-4} M\) (left side). a. Calculate the potential for this cell at \(25^{\circ} \mathrm{C}\). b. The \(\mathrm{Cu}^{2+}\) ion reacts with \(\mathrm{NH}_{3}\) to form \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}{ }^{2+}\) by the following equation: \(\mathrm{Cu}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)\) \(K=1.0 \times 10^{13}\) Calculate the new cell potential after enough \(\mathrm{NH}_{3}\) is added to the left cell compartment such that at equilibrium \(\left[\mathrm{NH}_{3}\right]=2.0 \mathrm{M}\)

Consider the following galvanic cell at \(25^{\circ} \mathrm{C}\) : $$ \mathrm{Pt}\left|\mathrm{Cr}^{2+}(0.30 \mathrm{M}), \mathrm{Cr}^{3+}(2.0 \mathrm{M})\right|\left|\mathrm{Co}^{2+}(0.20 \mathrm{M})\right| \mathrm{Co} $$ The overall reaction and equilibrium constant value are $$ \begin{aligned} 2 \mathrm{Cr}^{2+}(a q)+\mathrm{Co}^{2+}(a q) & \longrightarrow & \\ 2 \mathrm{Cr}^{3+}(a q)+\mathrm{Co}(s) & K &=2.79 \times 10^{7} \end{aligned} $$ Calculate the cell potential, \(\mathscr{E}\), for this galvanic cell and \(\Delta G\) for the cell reaction at these conditions.

The following standard reduction potentials have been det mined for the aqueous chemistry of indium: $$ \begin{array}{cl} \mathrm{In}^{3+}(a q)+2 \mathrm{e}^{-} \longrightarrow \operatorname{In}^{+}(a q) & \mathscr{E}^{\circ}=-0.444 \mathrm{~V} \\ \mathrm{In}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \operatorname{In}(s) & \mathscr{E}^{\circ}=-0.126 \mathrm{~V} \end{array} $$ a. What is the equilibrium constant for the disproportionation reaction, where a species is both oxidized and reduced, shown below? $$ 3 \operatorname{In}^{+}(a q) \longrightarrow 2 \operatorname{In}(s)+\operatorname{In}^{3+}(a q) $$ b. What is \(\Delta G_{\mathrm{f}}^{\circ}\) for \(\operatorname{In}^{+}(a q)\) if \(\Delta G_{\mathrm{f}}^{\circ}=-97.9 \mathrm{~kJ} / \mathrm{mol}\) for \(\mathrm{In}^{3+}(a q) ?\)

Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are \(1.0 M\) and that all partial pressures are \(1.0 \mathrm{~atm}\).

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