Skip to main content
Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.20 - ElectrochemistryProblema 75a
Capitolo 20, Problema 75a

Heart pacemakers are often powered by lithium–silver chromate 'button' batteries. The overall cell reaction is 2 Li(s) + Ag2CrO4(s) → Li2CrO4(s) + 2 Ag(s) (a) Lithium metal is the reactant at one of the electrodes of the battery. Is it the anode or the cathode?

Guida verificata passo dopo passo
1
Identify the role of lithium in the cell reaction: \(2 \text{Li}_{(s)} + \text{Ag}_2\text{CrO}_4_{(s)} \rightarrow \text{Li}_2\text{CrO}_4_{(s)} + 2 \text{Ag}_{(s)}\).
Determine which species is oxidized and which is reduced. Lithium goes from \(0\) to \(+1\) oxidation state, indicating oxidation.
Recall that oxidation occurs at the anode. Therefore, the electrode where lithium is oxidized is the anode.
Understand that the anode is where the oxidation reaction takes place, and electrons are released.
Conclude that since lithium is oxidized, it is the anode in this electrochemical cell.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
6m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Electrochemical Cells

Electrochemical cells convert chemical energy into electrical energy through redox reactions. They consist of two electrodes: the anode, where oxidation occurs, and the cathode, where reduction takes place. Understanding the flow of electrons and the reactions at each electrode is crucial for analyzing battery function.
Video consigliato:
Percorso guidato
02:46
Electrochemical Cells

Oxidation and Reduction

Oxidation is the loss of electrons, while reduction is the gain of electrons. In the context of batteries, the anode undergoes oxidation, releasing electrons that flow through the circuit to the cathode, where reduction occurs. Identifying which species is oxidized or reduced helps determine the roles of the electrodes.
Video consigliato:
Percorso guidato
01:53
Oxidation and Reduction Reactions

Lithium in Batteries

Lithium is commonly used in batteries due to its high electrochemical potential and light weight. In the given reaction, lithium metal is oxidized to lithium ions at the anode, providing a source of electrons. This characteristic makes lithium an essential component in the design and function of lithium-based batteries.
Video consigliato:
Percorso guidato
01:21
The Electrolytic Cell
Pratica correlata
Domanda del libro di testo

During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery. (b) How many coulombs of electrical charge are transferred from Zn to MnO2?

778
views
1
rank
Domanda del libro di testo

During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery. (a) What mass of MnO2 is reduced at the cathode during this discharge?

Domanda del libro di testo

Heart pacemakers are often powered by lithium–silver chromate 'button' batteries. The overall cell reaction is 2 Li(s) + Ag2CrO4(s) → Li2CrO4(s) + 2 Ag(s) (b) Choose the two half-reactions from Appendix E that most closely approximate the reactions that occur in the battery. What standard emf would be generated by a voltaic cell based on these half-reactions?

840
views