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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.20 - ElectrochemistryProblema 36b
Capitolo 20, Problema 36b

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (b) By using data from Appendix E, determine E°red for the reaction involving Pd.

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Identify the half-reactions involved in the voltaic cell. The given overall reaction is: \[ \text{PdCl}_4^{2-} (aq) + \text{Cd} (s) \rightarrow \text{Pd} (s) + 4 \text{Cl}^- (aq) + \text{Cd}^{2+} (aq) \].
Write the oxidation and reduction half-reactions. The oxidation half-reaction is: \[ \text{Cd} (s) \rightarrow \text{Cd}^{2+} (aq) + 2e^- \]. The reduction half-reaction is: \[ \text{PdCl}_4^{2-} (aq) + 2e^- \rightarrow \text{Pd} (s) + 4 \text{Cl}^- (aq) \].
Use the standard cell potential equation: \[ E^\circ_{\text{cell}} = E^\circ_{\text{red}} (\text{cathode}) - E^\circ_{\text{red}} (\text{anode}) \]. Here, \( E^\circ_{\text{cell}} = +1.03 \text{ V} \).
Look up the standard reduction potential for the cadmium half-reaction from Appendix E: \( E^\circ_{\text{red}} (\text{Cd}^{2+}/\text{Cd}) \).
Rearrange the equation to solve for \( E^\circ_{\text{red}} (\text{PdCl}_4^{2-}/\text{Pd}) \): \[ E^\circ_{\text{red}} (\text{PdCl}_4^{2-}/\text{Pd}) = E^\circ_{\text{cell}} + E^\circ_{\text{red}} (\text{Cd}^{2+}/\text{Cd}) \].

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Voltaic Cell

A voltaic cell, also known as a galvanic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte. The flow of electrons from the anode to the cathode generates an electric current, and the cell potential (E°) is a measure of the driving force behind the reaction.
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The Electrolytic Cell

Standard Reduction Potential (E°red)

Standard reduction potential (E°red) is a measure of the tendency of a chemical species to gain electrons and be reduced, measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C). Each half-reaction has a specific E°red value, which can be used to calculate the overall cell potential of a voltaic cell. A higher E°red indicates a greater likelihood of reduction occurring.
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Standard Reduction Potentials

Nernst Equation

The Nernst equation relates the cell potential of an electrochemical cell to the concentrations of the reactants and products involved in the redox reaction. It allows for the calculation of the cell potential under non-standard conditions and is expressed as E = E° - (RT/nF)ln(Q), where Q is the reaction quotient. Understanding this equation is crucial for analyzing how changes in concentration affect the cell potential.
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Domanda del libro di testo

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow

Domanda del libro di testo

(c) Why is it impossible to measure the standard reduction potential of a single half-reaction?

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A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions.

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Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (a) Cl21g2 + 2 I-1aq2 ¡ 2 Cl-1aq2 + I21s2

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Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (b) Ni1s2 + 2 Ce4+1aq2 ¡ Ni2+1aq2 + 2 Ce3+1aq2

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