Ch.19 - Electrochemistry

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McMurry 8th Edition

Ch.19 - Electrochemistry

Problema 59

Capitolo 19, Problema 59

Write the shorthand notation for a galvanic cell that uses the following cell reaction. Include inert electrodes if necessary. 2 Fe1s2 + Cr2O72-1aq2 + 14 H+1aq2¡2 Fe3+1aq2 + 2 Cr3+1aq2 + 7 H2O1l2

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Identify the oxidation and reduction half-reactions from the given overall cell reaction.

Write the oxidation half-reaction: \( 2 \text{Fe}^{2+} \rightarrow 2 \text{Fe}^{3+} + 2e^- \).

Write the reduction half-reaction: \( \text{Cr}_2\text{O}_7^{2-} + 14 \text{H}^+ + 6e^- \rightarrow 2 \text{Cr}^{3+} + 7 \text{H}_2\text{O} \).

Balance the number of electrons transferred in both half-reactions by multiplying the oxidation half-reaction by 3 and the reduction half-reaction by 1.

Combine the balanced half-reactions and write the cell notation: \( \text{Pt(s)} | \text{Fe}^{2+}(aq), \text{Fe}^{3+}(aq) || \text{Cr}_2\text{O}_7^{2-}(aq), \text{H}^+(aq), \text{Cr}^{3+}(aq) | \text{Pt(s)} \).

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Galvanic Cell Notation

Galvanic cell notation is a shorthand way to represent the components and reactions occurring in an electrochemical cell. It typically follows the format: anode | anode solution || cathode solution | cathode. The anode is where oxidation occurs, and the cathode is where reduction takes place, with the double vertical line indicating the salt bridge separating the two half-cells.

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01:08

The Galvanic Cell

Oxidation and Reduction

Oxidation and reduction are fundamental processes in electrochemistry. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. In the given reaction, iron (Fe) is oxidized to Fe3+, and chromium (Cr) is reduced from Cr2O7^2- to Cr3+, illustrating the transfer of electrons between the reactants.

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01:53

Oxidation and Reduction Reactions

Inert Electrodes

Inert electrodes, such as platinum or graphite, are used in electrochemical cells when the reactants or products are not solid. They provide a surface for the electron transfer without participating in the chemical reaction. In the context of the given cell reaction, an inert electrode may be necessary if either the oxidation or reduction half-reaction involves ions in solution rather than solid reactants.

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04:44

Electron Geometry

Pratica correlata

Domanda del libro di testo

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (b) Write balanced equations for the electrode and overall cell reactions.

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Domanda del libro di testo

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

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Domanda del libro di testo

Describe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b)

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Domanda del libro di testo

Write a balanced equation for the overall cell reaction in the following galvanic cell, and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br-(aq) | Br2(l2) || Cl2(g) | Cl-(aq) || Pt(s)

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Domanda del libro di testo

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (c) Give the shorthand notation for the cell.