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Chapter 22: Problem 19

Show by calculation whether the disproportionation of chlorine gas to chlorate and chloride ions will occur under standard-state conditions in an acidic solution.

Short Answer

Expert verified
The disproportionation of chlorine gas to chlorate and chloride ions will not occur under standard-state conditions in an acidic solution since the value of E˚Cell is negative (-0.11 V).

Step by step solution

01

Write Half-Reactions

Separate the overall redox reaction into two half-reactions. Chlorine is both oxidized and reduced in this process, forming chloride and chlorate ions. The half reactions are: \n 1. \(Cl2(g) + 2e^- ⟶ 2Cl^-(aq)\) (Reduction)\n 2. \(Cl2(g) + 6H2O (l) ⟶ 2ClO3^-(aq) + 12H^+ (aq) + 10e^-\) (Oxidation)
02

Determine the Reduction Potential

The standard reduction potential, E˚, can be obtained from standard reduction tables for each of the half-reactions. These are: \n 1. E˚(Cl2/Cl-) = +1.36 V \n 2. E˚(Cl2/ClO3-) = +1.47 V
03

Apply the Nernst Equation

According to the Nernst equation, the overall cell potential, E˚cell, is calculated as follows: \( E˚cell = E˚(Reduction) - E˚(Oxidation) \). Since chlorine is being reduced to chloride and oxidized to chlorate, we substitute the corresponding E˚s. \( E˚Cell = E˚(Cl2/Cl-) - E˚(Cl2/ClO3-) = +1.36 V - (+1.47 V)\
04

Determine Spontaneity of Reaction

The sign of E˚Cell tells us whether the reaction is spontaneous or not. A positive E˚Cell indicates a spontaneous redox reaction, while a negative E˚Cell indicates a non-spontaneous redox reaction. Hence, calculate E˚Cell. If our calculated E˚Cell is less than 0; the reaction is not spontaneous under standard conditions.

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Most popular questions from this chapter

Peroxonitrous acid is an unstable intermediate formed in the oxidation of \(\mathrm{HNO}_{2}\) by \(\mathrm{H}_{2} \mathrm{O}_{2}\). It has the same formula as nitric acid, HNO \(_{3}\). Show how you would expect peroxonitrous and nitric acids to differ in structure.

The heavier halogens (Cl, Br, and I) form compounds in which the central halogen atom, \(X\), is bonded directly to oxygen and to fluorine. Several examples are known, including those with formulas of the type \(\mathrm{FXO}_{2}, \mathrm{FXO}_{3, \text { and } \mathrm{F}_{3} \mathrm{XO} . \text { The structures of these }}\) molecules are all consistent with the VSEPR model. Draw Lewis structures and predict the geometries of (a) chloryl fluoride, \(\mathrm{FClO}_{2}\); (b) perchloryl fluoride, \(\mathrm{FClO}_{3} ;(\mathrm{c}) \mathrm{F}_{3} \mathrm{ClO}\).

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