/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 76 (a) The nonrechargeable lithium ... [FREE SOLUTION] | 91影视

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Chapter 20: Problem 76

(a) The nonrechargeable lithium batteries used for photography use lithium metal as the anode. What advantages might be realized by using lithium rather than zinc, cadmium, lead, or nickel? (b) The rechargeable lithiumion battery does not use lithium metal as an electrode material. Nevertheless, it still has a substantial advantage over nickel-based batteries. Suggest an explanation.

Short Answer

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Lithium anodes in nonrechargeable batteries are advantageous due to their lightweight nature, high electrochemical potential, and high specific capacity. These properties result in lighter batteries with higher energy density and longer-lasting power. Rechargeable lithium-ion batteries, despite not using lithium metal as an electrode, still have advantages over nickel-based batteries due to their efficient working mechanism, higher energy density, and better charge retention.

Step by step solution

01

Advantages of Lithium Anodes in Nonrechargeable Batteries

There are a few key properties of lithium that make it advantageous over other metals like zinc, cadmium, lead, or nickel when used as an anode material in nonrechargeable batteries. These include: 1. **Lightweight:** Lithium is the lightest metal in the periodic table. This means that using lithium in batteries results in lighter batteries, which is particularly important for applications like photography that often require portable power sources. 2. **High electrochemical potential:** Lithium has a high electrochemical potential, which means that it can release a higher voltage upon discharge relative to other common anode materials. This high voltage results in higher energy density, enabling a lithium-based battery to provide more energy for the same volume of battery material. 3. **High specific capacity:** Lithium has a high specific capacity, which means that it can store a large amount of charge per unit mass. This allows for a longer-lasting battery, as it can store more energy in a smaller and lighter package.
02

Rechargeable Lithium-ion Batteries vs. Nickel-based Batteries

Rechargeable lithium-ion batteries do not use lithium metal as an electrode material, but they still have advantages over nickel-based batteries. There are a few reasons for this, including: 1. **Working mechanism:** Unlike other batteries that rely on metallic electrodes, lithium-ion batteries work based on the movement of lithium ions between positive and negative electrodes through an electrolyte. This allows for a more efficient transfer of charge, resulting in higher energy efficiency and longer cycle life for the battery. 2. **Higher energy density:** Lithium-ion batteries generally have a higher energy density than nickel-based batteries due to the efficient working mechanism mentioned above. This means that they can store more energy within a smaller and lighter battery, making them preferable for applications that require portable power sources or devices with limited space. 3. **Better charge retention:** Lithium-ion batteries tend to retain their charge better when not in use compared to nickel-based batteries. This means that they have a lower self-discharge rate, allowing them to hold onto their stored energy for more extended periods without significant losses. Overall, these advantages make rechargeable lithium-ion batteries a suitable choice over nickel-based batteries for many applications, despite not using lithium metal as an electrode material.

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Most popular questions from this chapter

A voltaic cell utilizes the following reaction and operates at \(298 \mathrm{~K}\) : $$ 3 \mathrm{Ce}^{4+}(a q)+\mathrm{Cr}(s)-\rightarrow 3 \mathrm{Ce}^{3+}(a q)+\mathrm{Cr}^{3+}(a q) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when \(\left[\mathrm{Ce}^{4+}\right]=3.0 M\), \(\left[\mathrm{Ce}^{3+}\right]=0.10 \mathrm{M}\), and \(\left[\mathrm{Cr}^{3+}\right]=0.010 \mathrm{M} ?\) (c) What is the emf of the cell when \(\left[\mathrm{Ce}^{4+}\right]=0.10 \mathrm{M},\left[\mathrm{Ce}^{3+}\right]=1.75 \mathrm{M}\), and \(\left[\mathrm{Cr}^{3+}\right]=2.5 \mathrm{M} ?\)

A voltaic cell is constructed that uses the following halfcell reactions: $$ \begin{gathered} \mathrm{Cu}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Cu}(s) \\ \mathrm{I}_{2}(s)+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{I}^{-}(a q) \end{gathered} $$ The cell is operated at \(298 \mathrm{~K}\) with \(\left[\mathrm{Cu}^{+}\right]=0.25 \mathrm{M}\) and \(\left[\mathrm{I}^{-}\right]=3.5 \mathrm{M}\). (a) Determine \(E\) for the cell at these concentrations. (b) Which electrode is the anode of the cell? (c) Is the answer to part (b) the same as it would be if the cell were operated under standard conditions? (d) If \(\left[\mathrm{Cu}^{+}\right]\) was equal to \(0.15 \mathrm{M}\), at what concentration of \(\mathrm{I}^{-}\) would the cell have zero potential?

Some years ago a unique proposal was made to raise the Titanic. The plan involved placing pontoons within the ship using a surface-controlled submarine-type vessel. The pontoons would contain cathodes and would be filled with hydrogen gas formed by the electrolysis of water. It has been estimated that it would require about \(7 \times 10^{8} \mathrm{~mol}\) of \(\mathrm{H}_{2}\) to provide the buoyancy to lift the ship (J. Chem. Educ., Vol. \(50,1973,61\) ). (a) How many coulombs of electrical charge would be required? (b) What is the minimum voltage required to generate \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) if the pressure on the gases at the depth of the wreckage ( \(2 \mathrm{mi}\) ) is \(300 \mathrm{~atm} ?\) (c) What is the minimum electrical energy required to raise the Titanic by electrolysis? (d) What is the minimum cost of the electrical energy required to generate the necessary \(\mathrm{H}_{2}\) if the electricity costs 85 cents per kilowatt-hour to generate at the site?

(a) Why is it impossible to measure the standard reduction potential of a single half-reaction? (b) Describe how the standard reduction potential of a half-reaction can be determined.

(a) What is the difference between a battery and a fuel cell? (b) Can the "fuel" of a fuel cell be a solid? Explain.
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