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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.20 - ElectrochemistryProblema 12c
Capitolo 20, Problema 12c

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (c) Recall that in an electrolytic cell the anode is given the + sign and the cathode is given the – sign, which is the opposite of what we see in batteries. What half-reaction occurs at the anode in this electrolytic cell?
Diagram of an electrolytic cell showing carbon and steel electrodes in an electrolyte with chlorine gas output.

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Identify the anode and cathode in the electrolytic cell. The anode is the carbon electrode connected to the positive terminal, and the cathode is the steel electrode connected to the negative terminal.
Determine the species present in the electrolyte. The electrolyte contains molten salt, which includes magnesium ions (Mg2+) and chloride ions (Cl-).
Recall that oxidation occurs at the anode. Therefore, the half-reaction at the anode involves the loss of electrons by chloride ions.
Write the oxidation half-reaction for chloride ions at the anode: 2Cl- -> Cl2(g) + 2e-.
Confirm that chlorine gas (Cl2) is produced at the anode, as indicated by the diagram showing Cl2(g) out.

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Electrolytic Cell

An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction. In this setup, an external voltage source is applied to facilitate the movement of ions in the electrolyte, leading to the oxidation and reduction reactions at the electrodes. The anode is positively charged, where oxidation occurs, while the cathode is negatively charged, where reduction takes place.
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The Electrolytic Cell

Half-Reaction

A half-reaction is a representation of either the oxidation or reduction process occurring in an electrochemical cell. It shows the species involved, their charges, and the electrons exchanged. In the context of the electrolytic cell described, the half-reaction at the anode involves the oxidation of chloride ions (Cl-) to form chlorine gas (Cl2), which is released as a product.
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First-Order Half-Life

Electrode Reactions

Electrode reactions are the chemical processes that occur at the electrodes of an electrochemical cell. At the anode, oxidation occurs, where electrons are lost, while at the cathode, reduction occurs, where electrons are gained. Understanding these reactions is crucial for predicting the products of electrolysis, such as the formation of chlorine gas at the anode in this specific electrolytic cell.
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Electron Capture & Positron Emission Reaction Example
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Domanda del libro di testo

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (b) Chlorine gas is evolved as voltage is applied in the cell. Knowing this, identify the electrolyte.

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Domanda del libro di testo

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.

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Domanda del libro di testo

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (a) What is the most common oxidation number for Mg when it is part of a salt?

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Domanda del libro di testo

(b) On which side of an oxidation half-reaction do the electrons appear?

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Domanda del libro di testo

Bars of iron are put into each of the three beakers as shown here. In which beaker—A, B, or C—would you expect the iron to show the most corrosion ? [Section 20.8]

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