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consider the galvanic cell constructed with the following materials $\mathrm{Zn}$ electrode, $\mathrm{Zn}$ (NO
3)2, Fe electrode, $\mathrm{Fe}(\mathrm{NO} 3) 3 \mathrm{a}$. sketch a diagram of the galvanic cell identifying each material and labeling the cathode and anode $b$ determine the overall cell reaction and calculate $E$ cell c calculate delta $G$ and $K$ for the cell reaction at 25 degrees celsius $\mathrm{d}$. calculate Ecell at 25 degrees celcius when $[\mathrm{Zn} 2+] 1.0$ times 10 to the $-2 \mathrm{M}$ and [Fe $2+$ ] 1.0 times 10 to the -4 th $M$
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Answer from Sia

Posted 4 months ago

Solution

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1 Answer

Diagram not provided, but the description of the galvanic cell components and their arrangement is given.

2 Answer

The overall cell reaction is $\mathrm{Zn} + \mathrm{Fe}^{3+} \rightarrow \mathrm{Zn}^{2+} + \mathrm{Fe}^{2+}$.

3 Answer

$E^\circ_{\text{cell}} = 1.53\ \text{V}$.

4 Answer

$\Delta G^\circ = -2 \times 96485\ \text{C/mol} \times 1.53\ \text{V} = -295,082\ \text{J/mol}$ and $K$ can be calculated from $\Delta G^\circ = -RT\ln K$.

5 Answer

$E_{\text{cell}}$ at the given concentrations can be calculated using the Nernst equation.

Key Concept

Galvanic cells convert chemical energy into electrical energy through redox reactions, and the cell potential can be calculated using standard potentials and the Nernst equation.

Explanation

The galvanic cell operates on the principle of spontaneous redox reactions, with the anode experiencing oxidation and the cathode experiencing reduction. The standard cell potential gives the voltage under standard conditions, while the Nernst equation allows for the calculation of cell potential under non-standard conditions.

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