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Chapter 19: Problem 4

Describe the basic features of a galvanic cell. Why are the two components of the cell separated from each other?

Short Answer

Expert verified
A galvanic cell, also known as a voltaic cell, is an electrochemical cell that derives electrical energy from spontaneous redox reactions occurring within the cell. It has two half-cells, each containing an electrode immersed in a solution of its own ions. The separation of the Anode and Cathode is essential to prevent a rapid, uncontrolled direct reaction between the two. A salt bridge completes the circuit, allowing the flow of ions and maintaining cell neutrality.

Step by step solution

01

Describe a Galvanic Cell

A galvanic cell, also known as a voltaic cell, is a device in which a redox reaction spontaneously occurs and produces an electric current. It consists of two half-cells, each containing an electrode (which can be a metal) immersed in a solution of its own ions.
02

Name the components of a Galvanic Cell

There are two primary components in a galvanic cell: the Anode, which is the electrode where oxidation occurs, and the Cathode, where reduction happens. It also includes an electrolyte, which allows the flow of ions, and a salt bridge that completes the circuit.
03

Discuss the separation of the cell components

The anode (negative electrode) and the cathode (positive electrode) must be separate from each other to prevent a direct reaction between the two, which would occur rapidly and not produce a controlled electrical current. The separation ensures a sustained, controlled chemical reaction leading to a steady flow of electric current between the two.
04

Explain the purpose of the salt bridge

The salt bridge completes the electrical circuit and allows the flow of ions between the half-cells. It is pivotal to maintain the cell neutrality, i.e., to prevent the solutions in the half-cells from becoming too negatively charged at the cathode or too positively charged at the anode.

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Most popular questions from this chapter

Calculate the amounts of \(\mathrm{Cu}\) and \(\mathrm{Br}_{2}\) produced in \(1.0 \mathrm{~h}\) at inert electrodes in a solution of \(\mathrm{CuBr}_{2}\) by a current of 4.50 A.

What is the difference between a galvanic cell (such as a Daniell cell) and an electrolytic cell?

Gold will not dissolve in either concentrated nitric acid or concentrated hydrochloric acid. However, the metal does dissolve in a mixture of the acids (one part \(\mathrm{HNO}_{3}\) and three parts \(\mathrm{HCl}\) by volume ), called aqua regia. (a) Write a balanced equation for this reaction. (Hint: Among the products are \(\mathrm{HAuCl}_{4}\) and \(\mathrm{NO}_{2} .\) ) (b) What is the function of \(\mathrm{HCl} ?\)

Use the standard reduction potentials to find the equilibrium constant for each of the following reactions at \(25^{\circ} \mathrm{C}\): (a) \(\operatorname{Br}_{2}(l)+2 \mathrm{I}^{-}(a q) \rightleftharpoons 2 \mathrm{Br}^{-}(a q)+\mathrm{I}_{2}(s)\) (b) \(2 \mathrm{Ce}^{4+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons$$\mathrm{Cl}_{2}(g)+2 \mathrm{Ce}^{3+}(a q)\) (c) \(5 \mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q) \rightleftharpoons\) \(\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)+5 \mathrm{Fe}^{3+}(a q)\)

Explain why most useful galvanic cells give voltages of no more than 1.5 to \(2.5 \mathrm{~V}\). What are the prospects for developing practical galvanic cells with voltages of \(5 \mathrm{~V}\) or more?
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