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Chapter 20: Problem 124

Construct a concept map illustrating the relationship between batteries and electrochemical ideas.

Short Answer

Expert verified
A concept map can illustrate that electrochemistry is a field that studies the movement of electrons and includes topics like redox reactions and electrochemical cells. Batteries, which utilize these principles, convert chemical energy to electrical energy. The whole process involves the flow of electrons from the anode to the cathode, aided by the movement of cations and anions.

Step by step solution

01

Identifying Main Concepts

The first step towards creating a concept map is identifying the main concepts that must be included: Batteries, Electrochemistry, Redox reactions, Cations and Anions, Electrochemical cells, Anode, Cathode, and Electron flow.
02

Establish Relationship between Concepts

Next, describe how these concepts are connected. For example, Electrochemistry is the overarching concept studying chemical processes that cause electrons to move. This involves Redox reactions which are reactions where oxidation and reduction occur simultaneously. Batteries are a practical application of these principles. They convert chemical energy to electrical energy through a process that occurs in an electrochemical cell.
03

Arrange the Concepts

Now, arrange the concepts in the concept map. Start with the broad topic like 'Electrochemistry' and then branch out to smaller, detailed concepts such as 'Redox reactions', 'Electrochemical cells' and 'Batteries' and explain their relations.
04

Draw the Connections

Finally, draw the connections between the concepts. These can be shown as arrows or lines between concepts. Each connection should be labelled with linking phrases or words that describe the relationship between the concepts. For example, an arrow pointing from 'Redox reactions' to 'Batteries' could be labelled with 'occur in'.

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Most popular questions from this chapter

The following voltaic cell registers an \(E_{\text {cell }}=0.108 \mathrm{V}\) What is the pH of the unknown solution? $$\operatorname{Pt}\left|\mathrm{H}_{2}(\mathrm{g}, 1 \mathrm{atm})\right| \mathrm{H}^{+}(x \mathrm{M}) \| \mathrm{H}^{+}(1.00 \mathrm{M}) |$$ $$\mathrm{H}_{2}(\mathrm{g}, 1 \mathrm{atm}) | \mathrm{Pt}$$

\(\mathrm{Ni}^{2+}\) has a more positive reduction potential than \(\mathrm{Cd}^{2+}\) (a) Which ion is more easily reduced to the metal? (b) Which metal, Ni or Cd, is more easily oxidized?

Your task is to determine \(E^{\circ}\) for the reduction of \(\mathrm{CO}_{2}(\mathrm{g})\) to \(\mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{g})\) in two different ways and to explain why each gives the same result. (a) Consider a fuel cell in which the cell reaction corresponds to the complete combustion of propane gas. Write the half-cell reactions and the overall reaction. Determine \(\Delta G^{\circ}\) and \(E_{\text {cell }}^{\circ}\) for the reaction, then obtain \(E_{\mathrm{CO}_{2} / \mathrm{C}_{3} \mathrm{H}_{8}^{*}}^{\circ}\) (b) Without considering the oxidation that occurs simultaneously, obtain \(E_{\mathrm{CO}_{2} / \mathrm{C}_{3} \mathrm{H}_{8}}^{\circ}\) directly from tabulated thermodynamic data for the reduction half-reaction.

$$E_{\text {cathode }}^{\circ}=(2.71-2.310) V=+0.40 V$$VVV

Only a tiny fraction of the diffusible ions move across a cell membrane in establishing a Nernst potential (see Focus On 20: Membrane Potentials), so there is no detectable concentration change. Consider a typical cell with a volume of \(10^{-8} \mathrm{cm}^{3},\) a surface area \((A)\) of \(10^{-6} \mathrm{cm}^{2},\) and a membrane thickness \((l)\) of \(10^{-6} \mathrm{cm}\) Suppose that \(\left[\mathrm{K}^{+}\right]=155 \mathrm{mM}\) inside the cell and \(\left[\mathrm{K}^{+}\right]=4 \mathrm{mM}\) outside the cell and that the observed Nernst potential across the cell wall is \(0.085 \mathrm{V}\). The membrane acts as a charge-storing device called a capacitor, with a capacitance, \(C,\) given by $$C=\frac{\varepsilon_{0} \varepsilon A}{l}$$ where \(\varepsilon_{0}\) is the dielectric constant of a vacuum and the product \(\varepsilon_{0} \varepsilon\) is the dielectric constant of the membrane, having a typical value of \(3 \times 8.854 \times 10^{-12}\) \(\mathrm{C}^{2} \mathrm{N}^{-1} \mathrm{m}^{-2}\) for a biological membrane. The SI unit of capacitance is the firad, \(1 \mathrm{F}=1\) coulomb per volt \(=1 \mathrm{CV}^{-1}=1 \times \mathrm{C}^{2} \mathrm{N}^{-1} \mathrm{m}^{-1}\) (a) Determine the capacitance of the membrane for the typical cell described. (b) What is the net charge required to maintain the observed membrane potential? (c) How many \(\mathrm{K}^{+}\) ions must flow through the cell membrane to produce the membrane potential? (d) How many \(\mathrm{K}^{+}\) ions are in the typical cell? (e) Show that the fraction of the intracellular \(K^{+}\) ions transferred through the cell membrane to produce the membrane potential is so small that it does not change \(\left[\mathrm{K}^{+}\right]\) within the cell.
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