What are the oxidation and reduction half-reactions and the balanced overall reaction for each of the following processes: (a) Conversion of HOC1+ HS- to Cl- + S042-(b) Conversion of CH3OH + O2(ag) to CO2(g) + H2O(1)(c) Conversion of MnO4- + Mn²+ to MnO2(s)

Answered: What are the oxidation and reduction…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What are the oxidation and reduction half-reactions and the balanced overall reaction for each of the following processes:

(a) Conversion of HOC1+ HS- to Cl- + S042-
(b) Conversion of CH3OH + O2(ag) to CO2(g) + H2O(1)
(c) Conversion of MnO4- + Mn²+ to MnO2(s)

Expert Solution

Step 1

The oxidation-reduction half reaction method are to be written for the given reactions and balanced them.

In redox reaction one of the element gets oxidised and another gets reduced. That means oxidation and reduction reactions occur simultaneously. The element whose oxidation number increased in the chemical equation is said to be oxidized. The element whose oxidation number decreased in the chemical equation is said to be reduced. The oxidation number is the total number of electrons that atom either gains or losses in order to form a chemical bond with another atom.

The oxidation number is the total number of electrons that atom either gains or losses in order to form a chemical bond with another atom.

Rules to assign oxidation number:

The oxidation number of an element in its pure form is 0.
The general oxidation state of oxygen is -2.
The general oxidation state of hydrogen is +1
The total oxidation state of all atoms in a neutral species is 0 and in an ion is equal to the ion charge.
The oxidation number of halogens is -1.

Step 2

(a) Conversion of HOCl + HS^- to Cl^- + SO₄^2-

The reaction equation is,

HOCl + HS^- $\to$ Cl^- + SO₄^2-

Assign the oxidation states to each element in the given reaction equation,

HOCl

HS^-

→

Cl^-

SO₄^2-

H = +1

O = -2

Cl = +1

H = +1

S = -2

Cl = -1

S = +6

O = -2

The oxidation number of chlorine has decreased from +1 to -1. Therefore, HOCl have reduced.

The oxidation number of sulfur has increased from -2 to +6. Therefore, HS^- has oxidized.

The half reactions are:

HOCl $\to$ Cl^- (reduction half reaction)

HS^- $\to$ SO₄^2- (oxidation half reaction)

Balance O atoms by adding H₂O:

HOCl $\to$ Cl^- + H₂O

HS^- + 4 H₂O $\to$ SO₄^2-

Balance H atoms by adding H⁺:

HOCl + H⁺ $\to$ Cl^- + H₂O

HS^- + 4 H₂O $\to$ SO₄^2- + 9H⁺

Balance charge by adding electrons to more positive side:

HOCl + H⁺ +2 e^- $\to$ Cl^- + H₂O

HS^- + 4 H₂O $\to$ SO₄^2- + 9H⁺ + 8 e^-

Multiply reduction half reaction by 4 to balance electrons,

4 HOCl + 4 H⁺ +8 e^- $\to$ 4 Cl^- + 4 H₂O

HS^- + 4 H₂O $\to$ SO₄^2- + 9H⁺ + 8 e^-

Add two half reactions,

4 HOCl + HS^- $\to$ 4 Cl^- + SO₄^2- + 5H⁺

This is the balanced equation.

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