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Chapter 5: Problem 2

Define the following terms: (a) Oxidation (b) Standard electrod potential (c) Overpotential (d) Redox couple

Short Answer

Expert verified
(a) Oxidation is a process where a substance loses electrons. (b) Standard electrode potential is a measure of the individual potential of a reversible electrode at standard state. (c) Overpotential is the potential difference between the equilibrium potential and the potential at which the electrochemical reaction is actually observed to occur. (d) A Redox couple refers to a pair of substances that are involved in a Redox reaction, where one member undergoes oxidation, while the other undergoes reduction.

Step by step solution

01

Definition of Oxidation

Oxidation in chemistry refers to a process where a substance loses electrons. This is often associated with the reaction of a substance with oxygen, hence the term. However, oxidation doesn’t necessarily need to involve oxygen. It is one half of a Redox (reduction-oxidation) reaction, the other half being reduction.
02

Definition of Standard Electrode Potential

Standard electrode potential, also known as electrochemical potential, is the measure of the individual potential of a reversible electrode at standard state, i.e., a temperature of 298.15 K, a solute concentration of 1 mol\(^{-1}\) and a pressure of 1 atm. It can be viewed as the measure of the tendency of a chemical species to acquire electrons and thereby be reduced or, alternatively, lose electrons and be oxidised.
03

Definition of Overpotential

Overpotential is defined as the potential difference between the equilibrium potential and the potential at which the electrochemical reaction is actually observed to occur. It represents the extra energy required to make a chemical reaction occur at an electrode.
04

Definition of Redox Couple

A Redox couple refers to a pair of substances that are involved in an oxidation/reduction (Redox) reaction. One member of the couple undergoes oxidation while the other undergoes reduction during the reaction.

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Most popular questions from this chapter

Determine the reduction potential \(E_{\mathrm{Sn}^{4+} / \mathrm{sn}}^{\circ}\) if \(E_{\mathrm{Sn}^{2+} / \mathrm{Sn}}^{\circ}=-0.136 \mathrm{~V}\) and \(E_{\mathrm{Sn}^{4+} / \mathrm{sn}^{2+}}^{\circ}=0.15 \mathrm{~V}\). Also draw the corresponding Latimer diagram.

Discuss electrochemical cell in detail with the help of a suitable example.

Calculate the equilibrium constant for the possible reaction between \(\mathrm{Fe}^{2+}(\mathrm{aq})\) ions and \(\mathrm{Ce}^{4+}(\mathrm{aq})\) ions \(\mathrm{f} E_{\mathrm{Ce}^{4+} / \mathrm{ce}^{3+}}=1.44 \mathrm{~V}\) and \(E_{\mathrm{Fe}^{\circ} / \mathrm{Fe}^{2+}}^{\circ}=0.68 \mathrm{~V}\). Also comment on the spontaneity of the reaction.

Discuss the Pourbaix diagram for iron in detail.

Draw a Frost diagram for mercury in acid solution and comment on the tendency of the involved species to undergo disproportionation. Given \(E_{\mathrm{Hg}^{2+} / \mathrm{Hg}_{2}^{2+}}=0.911 \mathrm{~V}\) and \(E_{\mathrm{H}_{2}^{2+} / \mathrm{Hg}}^{\circ}=0.796 \mathrm{~V}\)
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