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Chapter 18: Problem 3

Define the following terms: anode, cathode, cell voltage, electromotive force, and standard reduction potential.

Short Answer

Expert verified
Anode is the electrode where oxidation takes place, cathode is where reduction occurs. Cell voltage is the electric potential difference between the two electrodes. Electromotive force is the energy provided per charge that pushes the flow of electrons. Standard reduction potential measures a species' tendency to gain electrons.

Step by step solution

01

Defining Anode

An anode is the electrode where oxidation takes place. In a galvanic (voltaic) cell, it's the negative electrode, while in an electrolytic cell, it's the positive electrode.
02

Defining Cathode

A cathode is the electrode where reduction occurs. In a galvanic (voltaic) cell, it's the positive electrode, while in an electrolytic cell, it's the negative electrode.
03

Defining Cell Voltage

Cell voltage, also known as cell potential, is the force that pushes electric charges through a circuit. It's equal to the difference in electric potential between the two electrodes of a cell, often measured in volts.
04

Defining Electromotive Force

Electromotive force (EMF) is the energy provided per unit charge that drives the flow of electrons around a circuit. It is the maximum potential difference between two electrodes of a cell.
05

Defining Standard Reduction Potential

Standard reduction potential is a measure of the tendency for a chemical species to be reduced. Each species has its own intrinsic reduction potential; the more positive the potential, the greater the species' ability to gain electrons and be reduced.

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Most popular questions from this chapter

The zinc-air battery shows much promise for electric cars because it is lightweight and rechargeable: The net transformation is \(\mathrm{Zn}(s)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnO}(s)\) (a) Write the half-reactions at the zinc-air electrodes and calculate the standard emf of the battery at \(25^{\circ} \mathrm{C}\). (b) Calculate the emf under actual operating conditions when the partial pressure of oxygen is 0.21 atm. (c) What is the energy density (measured as the energy in kilojoules that can be obtained from \(1 \mathrm{~kg}\) of the metal) of the zinc electrode? (d) If a current of \(2.1 \times 10^{5} \mathrm{~A}\) is to be drawn from a zinc-air battery system, what volume of air (in liters) would need to be supplied to the battery every second? Assume that the temperature is \(25^{\circ} \mathrm{C}\) and the partial pressure of oxygen is 0.21 atm.

Describe the electrolysis of an aqueous solution of \(\mathrm{KNO}_{3}\)

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 \(\mathrm{HCl} ?\)

Based on the following standard reduction potentials: $$ \begin{aligned} \mathrm{Fe}^{2+}(a q)+2 e^{-} & \longrightarrow \mathrm{Fe}(s) & & E_{1}^{\circ}=-0.44 \mathrm{~V} \\ \mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q) & & E_{2}^{\circ}=& 0.77 \mathrm{~V} \end{aligned} $$ calculate the standard reduction potential for the half-reaction $$ \mathrm{Fe}^{3+}(a q)+3 e^{-} \longrightarrow \mathrm{Fe}(s) \quad E_{3}^{\circ}=? $$

The \(E_{\text {cell }}^{\circ}\) for the following cell is \(1.54 \mathrm{~V}\) at \(25^{\circ} \mathrm{C}\) : $$\mathrm{U}(s) \mid \mathrm{U}^{3+}(a q)\left\|\mathrm{Ni}^{2+}(a q)\right\| \mathrm{Ni}(s)$$ Calculate the standard reduction potential for the \(\mathrm{U}^{3+} / \mathrm{U}\) half-cell.
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