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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.20 - Electrochemistry문제 79a
20장, 문제 79a

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?

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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.

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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.
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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.
추천 영상:
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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.
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01:21
The Electrolytic Cell
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In some applications nickel–cadmium batteries have been replaced by nickel–zinc batteries. The overall cell reaction for this relatively new battery is: 2 H2O(l) + 2 NiO(OH)(s) + Zn(s) → 2 Ni(OH)2(s) + Zn(OH)2(s) (c) A single nickel–cadmium cell has a voltage of 1.30 V. Based on the difference in the standard reduction potentials of Cd2+ and Zn2+, what voltage would you estimate a nickel–zinc battery will produce? (d) Would you expect the specific energy density of a nickel–zinc battery to be higher or lower than that of a nickel–cadmium battery?

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교과서 질문

During a period of discharge of a lead–acid battery, 402 g of Pb from the anode is converted into PbSO4(s). (b) How many coulombs of electrical charge are transferred from Pb to PbO2?

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교과서 질문

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?

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교과서 질문

During a period of discharge of a lead–acid battery, 402 g of Pb from the anode is converted into PbSO4(s). (a) What mass of PbO2(s) is reduced at the cathode during this same period?

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교과서 질문

In some applications nickel–cadmium batteries have been replaced by nickel–zinc batteries. The overall cell reaction for this relatively new battery is: 2 H2O(l) + 2 NiO(OH)(s) + Zn(s) → 2 Ni(OH)2(s) + Zn(OH)2(s) (b) What is the anode half-reaction?

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교과서 질문

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?

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