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Chapter 5: Problem 3

What do you mean by electrochemical series? Discuss its important applications.

Short Answer

Expert verified
The Electrochemical series, also known as the reactivity series, is a list of metals ordered by their reactivity. It is based on the reduction potential of metals, with a higher reduction potential indicating a higher reactivity. The series has several applications, including determining the direction of current in an electrochemical cell, predicting the feasibility of chemical reactions, calculating the e.m.f. of a cell, and is essential in processes like corrosion and metallurgy.

Step by step solution

01

Define Electrochemical Series

The electrochemical series, also known as the reactivity series, is a list of metals arranged in order of their reactivity - from most reactive to least reactive. It is a tabulation of standard electrode potentials (or reduction potentials) which enables the relative reactivity of different metals to be determined.
02

Explain the Working of Electrochemical Series

The working is based on the concept of reduction potential. The higher the reduction potential of the metal in the series, the greater is its ability to get reduced (gain electrons), and thus, the higher is its reactivity. For instance, if two metals are placed in a solution and the one with the higher reduction potential will displace the other.
03

Discuss Applications of Electrochemical Series

The electrochemical series have several significant applications. Some of which are: 1. Determining the direction of flow of current in an electrochemical cell. 2. Predicting the feasibility of a chemical reaction. 3. Calculating the e.m.f. of a cell. It also plays a significant role in corrosion, metallurgical processes, and in creating batteries.

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Most popular questions from this chapter

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.

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.

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 \(E_{\mathrm{H}_{2}^{2+} / \mathrm{Hg}}^{\circ}=0.796 \mathrm{~V}\)

Write short notes on (a) Redox stability field of water (b) Hydrogen overpotential (c) Nernst equation(d) Disproportionation

Discuss the Pourbaix diagram for iron in detail.
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