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Chapter 18: Problem 19

What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.

Short Answer

Expert verified
Electrochemistry is the study of chemical reactions involving electron transfer, usually in redox reactions. Redox reactions are chemical reactions where oxidation states change due to electron transfer, with one species being reduced and the other being oxidized. A galvanic cell converts chemical energy into electrical energy through a spontaneous redox reaction, whereas an electrolytic cell uses electrical energy to drive a non-spontaneous redox reaction, like in electrolysis or electroplating. The key differences are energy conversion, spontaneity, direction of electron flow, and applications.

Step by step solution

01

Define Electrochemistry

Electrochemistry is a branch of chemistry that deals with the study of chemical reactions involving the transfer of electrons between different chemical species, usually in the form of a redox reaction. It encompasses the processes and technologies in which the interconversion of electrical energy and chemical energy takes place, such as batteries and electrolysis.
02

Define Redox Reactions

Redox reactions, short for reduction-oxidation reactions, are chemical reactions where the oxidation states of the elements involved change due to the transfer of electrons. In a redox reaction, one element or species is reduced (gains electrons) while the other is oxidized (loses electrons).
03

Explain Galvanic Cells

A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts the chemical energy produced by a spontaneous redox reaction (meaning it occurs naturally, without any external input) into electrical energy. In a galvanic cell, the reactants are two different metals or metal ions, each in contact with an electrolyte solution. The two reactants form a redox pair, and the electrons flow from the more oxidized species (anode) to the less oxidized species (cathode) through an external circuit, generating electrical current.
04

Explain Electrolytic Cells

An electrolytic cell is an electrochemical cell where electrical energy is used to drive a non-spontaneous redox reaction (meaning it does not occur naturally and requires an external energy source). In an electrolytic cell, an external voltage source (a battery or a power supply) forces the electrons to flow in the opposite direction of the natural redox reaction. Electrolysis is the most common application of electrolytic cells, and it is used to split compounds into their constituent elements or to plate one metal onto another.
05

Highlight the Differences between Galvanic and Electrolytic Cells

The main differences between galvanic and electrolytic cells are as follows: 1. Energy Conversion: A galvanic cell converts chemical energy into electrical energy, while an electrolytic cell converts electrical energy into chemical energy. 2. Spontaneity: Redox reactions in galvanic cells are spontaneous, while those in electrolytic cells are non-spontaneous and need an external energy source to occur. 3. Direction of Electron Flow: In a galvanic cell, electrons flow from the anode to the cathode (in a direction that is favourable for the redox reaction), while in an electrolytic cell, they flow in the opposite direction (forced from the cathode to the anode). 4. Applications: Galvanic cells are used in batteries and other energy storage devices, while electrolytic cells are applied in processes like electrolysis and electroplating.

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Most popular questions from this chapter

What is the maximum work that can be obtained from a hydrogen-oxygen fuel cell at standard conditions that produces \(1.00 \mathrm{~kg}\) water at \(25^{\circ} \mathrm{C} ?\) Why do we say that this is the maximum work that can be obtained? What are the advantages and disadvantages in using fuel cells rather than the corresponding combustion reactions to produce electricity?

The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing \(\mathrm{Mn}^{2+}\) ions. These ions are then oxidized to the deeply colored \(\mathrm{MnO}_{4}^{-}\) ions by periodate ion \(\left(\mathrm{IO}_{4}^{-}\right)\) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate \(\mathscr{C}^{\circ}\) and \(\Delta G^{\circ}\) at \(25^{\circ} \mathrm{C}\) for each reaction.

Nerve impulses are electrical "signals" that pass through neurons in the body. The electrical potential is created by the differences in the concentration of \(\mathrm{Na}^{+}\) and \(\mathrm{K}^{+}\) ions across the nerve cell membrane. We can think about this potential as being caused by a concentration gradient, similar to what we see in a concentration cell (keep in mind that this is a very simple explanation of how nerves work; there is much more involved in the true biologic process). A typical nerve cell has a resting potential of about \(-70 \mathrm{mV}\). Let's assume that this resting potential is due only to the \(\mathrm{K}^{+}\) ion concentration difference. In nerve cells, the \(\mathrm{K}^{+}\) concentration inside the cell is larger than the \(\mathrm{K}^{+}\) concentration outside the cell. Calculate the \(\mathrm{K}^{+}\) ion concentration ratio necessary to produce a resting potential of \(-70 . \mathrm{mV}\). $$\frac{\left[\mathrm{K}^{+}\right]_{\text {inside }}}{\left[\mathrm{K}^{+}\right]_{\text {outside }}}=?$$

A zinc-copper battery is constructed as follows at \(25^{\circ} \mathrm{C}:\) $$\mathrm{Zn}\left|\mathrm{Zn}^{2+}(0.10 \mathrm{M}) \| \mathrm{Cu}^{2+}(2.50 \mathrm{M})\right| \mathrm{Cu}$$ The mass of each electrode is \(200 . \mathrm{g}\). a. Calculate the cell potential when this battery is first connected. b. Calculate the cell potential after \(10.0 \mathrm{~A}\) of current has flowed for \(10.0 \mathrm{~h}\). (Assume each half-cell contains \(1.00 \mathrm{~L}\) of solution.) c. Calculate the mass of each electrode after \(10.0 \mathrm{~h}\). d. How long can this battery deliver a current of \(10.0 \mathrm{~A}\) before it goes dead?

Consider the following galvanic cell at \(25^{\circ} \mathrm{C}\) : $$\mathrm{Pt}\left|\mathrm{Cr}^{2+}(0.30 M), \mathrm{Cr}^{3+}(2.0 M)\right|\left|\mathrm{Co}^{2+}(0.20 M)\right| \mathrm{Co}$$ The overall reaction and equilibrium constant value are $$2 \mathrm{Cr}^{2+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow{2 \mathrm{Cr}^{3+}(a q)+\mathrm{Co}(s)} \quad K=2.79 \times 10^{7}$$ Calculate the cell potential, \(\mathscr{E}\), for this galvanic cell and \(\Delta G\) for the cell reaction at these conditions.
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