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Chapter 18: Problem 45

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

Short Answer

Expert verified
The main difference between a galvanic cell and an electrolytic cell is that a galvanic cell converts chemical energy into electrical energy through a spontaneous reaction, while an electrolytic cell uses electrical energy to drive a non-spontaneous reaction. Also, the flow of electrons in a galvanic cell is natural from anode to cathode, while in an electrolytic cell, it's forced from cathode to anode.

Step by step solution

01

Introduction and Definition of Galvanic Cell

A galvanic cell (such as a Daniell cell) is an electrochemical cell that converts the energy released by a spontaneous redox reaction into electrical energy. In other words, the chemical reaction happens naturally and is capable of producing an electric current.
02

Introduction and Definition of Electrolytic Cell

In contrast, an electrolytic cell is a type of electrochemical cell where electrical energy is used to drive a non-spontaneous redox reaction. This means that an external power source is necessary to push the reaction.
03

Comparison of Electrolyte Flow

In a galvanic cell, the electrons flow from the anode (where oxidation occurs) to the cathode (where reduction occurs). The opposite happens in an electrolytic cell: the electrons are forced to flow from the cathode (where reduction occurs) to the anode (where oxidation occurs), against their natural direction.
04

Comparison of Energy Source

The galvanic cell relies on the natural, spontaneous reaction to generate electricity, while the electrolytic cell relies on an external power source to induce the reactions.
05

Comparison of Applications

Galvanic cells are typically used in batteries to provide electrical energy to a circuit. On the other hand, electrolytic cells are used in processes such as electroplating or electrolysis, where an electric current is used to drive a chemical change.

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Most popular questions from this chapter

For each of the following redox reactions, (i) write the half-reactions, (ii) write a balanced equation for the whole reaction, (iii) determine in which direction the reaction will proceed spontaneously under standard-state conditions: (a) \(\mathrm{H}_{2}(g)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{H}^{+}(a q)+\mathrm{Ni}(s)\) (b) \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow\) \(\quad \mathrm{Mn}^{2+}(a q)+\mathrm{Cl}_{2}(g)\) (in acid solution) \(\begin{array}{ll}\text { (c) } \mathrm{Cr}(s)+\mathrm{Zn}^{2+}(a q) & \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Zn}(s)\end{array}\)

A sample of iron ore weighing \(0.2792 \mathrm{~g}\) was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required \(23.30 \mathrm{~mL}\) of \(0.0194 \mathrm{M} \mathrm{KMnO}_{4}\) for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore.

Show a sketch of a galvanic concentration cell. Each compartment consists of a Co electrode in a \(\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}\) solution. The concentrations in the compartments are \(2.0 \mathrm{M}\) and \(0.10 \mathrm{M}\), respectively. Label the anode and cathode compartments. Show the direction of electron flow. (a) Calculate the \(E_{\text {cell }}\) at \(25^{\circ} \mathrm{C}\). (b) What are the concentrations in the compartments when the \(E_{\text {cell }}\) drops to 0.020 V? Assume volumes to remain constant at \(1.00 \mathrm{~L}\) in each compartment.

What is a cell diagram? Write the cell diagram for a galvanic cell consisting of an \(\mathrm{Al}\) electrode placed in a \(1 M\) Al(NO \(_{3}\) ) \(_{3}\) solution and a Ag electrode placed in a \(1 M \mathrm{AgNO}_{3}\) solution.

The oxidation of \(25.0 \mathrm{~mL}\) of a solution containing \(\mathrm{Fe}^{2+}\) requires \(26.0 \mathrm{~mL}\) of \(0.0250 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) in acidic solution. Balance the following equation and calculate the molar concentration of \(\mathrm{Fe}^{2+}\) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{Fe}^{2+}+\mathrm{H}^{+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{Fe}^{3+}\)
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