Explanation Add both equations (1) and (2) to get the overall reaction as follows: I 2 + 2 e − + F e → F e 2 + + 2 e − + 2 I − The overall balanced reaction is I 2 + F e → F e I 2 Write oxidation states of all the atoms and identify the oxidation and reduction half-reactions. C l 2 + H 2 O 2 → C l − + O 2 0 + 1 , − 1 − 1 0 Here, chlorine gains electrons (reduction) and oxygen loses electrons (oxidation). The half-reaction is as follows: C l 2 → C l − H 2 O 2 → O 2 Balance both the reactions by using protons in water. In acidic medium, the hydrogen and the oxygen atoms are balanced. The balanced reactions are as follows: C l 2 → 2 C l − H 2 O 2 → O 2 + 2 H + Use electrons to balance the change on both sides. C l 2 + 2 e − → 2 C l − ........... ( 1 ) H 2 O 2 → O 2 + 2 H + + 2 e − .......... ( 2 ) Given half-reactions are balanced and have equal number electrons. Now, add both the equations to get overall reaction as follows: C l 2 + 2 e − + H 2 O 2 → 2 C l − + O 2 + 2 H + + 2 e − The overall balanced reaction is C l 2 + H 2 O 2 → 2 C l − + O 2 + 2 H + Write oxidation states of all the atoms to identify the oxidation and reduction half-reactions. H g 2 + + H 2 → H g + H 2 O + 2 0 0 + 1 , − 2 Here, H g 2 + gains electrons (reduction) and hydrogen loses electrons (oxidation). The half-reaction is as follows: H g 2 + → H g H 2 → H 2 O Balance both the reactions. Use hydroxide ions and water to balance hydrogen and oxygen atoms (for basic medium). The balanced reactions are as follows: H g 2 + → H g H 2 + 2 O H − → H 2 O + H 2 P Use electrons to balance the change on both sides: H g 2 + + 2 e − → H g

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Chapter 19, Problem 142QGW

Interpretation Introduction

To balance the given redox reactions:-

a) I2+Fe→FeI2

b) Cl2+H2O2→Cl−+O2

c) Hg2++H2→Hg +H2O

d) CH3OH+O2→CO2 + H2O

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Chapter 19, Problem 141E

Chapter 19, Problem 143DIA

Chapter 19 Solutions

Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition

Ch. 19 - Prob. 1SAQ Ch. 19 - Q2. Which statement is true for voltaic cells? a)...Ch. 19 - Prob. 3SAQ Ch. 19 - Prob. 4SAQ Ch. 19 - Prob. 5SAQ Ch. 19 - Prob. 6SAQ Ch. 19 - Prob. 7SAQ Ch. 19 - Prob. 8SAQ Ch. 19 - Prob. 9SAQ Ch. 19 - Prob. 10SAQ

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Balancing Redox Reactions in Acidic and Basic Conditions; Author: Professor Dave Explains;https://www.youtube.com/watch?v=N6ivvu6xlog;License: Standard YouTube License, CC-BY

To balance the given redox reactions: - a) I 2 + F e → F e I 2 b) C l 2 + H 2 O 2 → C l − + O 2 c) H g 2 + + H 2 → H g + H 2 O d) C H 3 O H + O 2 → C O 2 + H 2 O

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To balance the given redox reactions:- a) I2+Fe→FeI2 b) Cl2+H2O2→Cl−+O2 c) Hg2++H2→Hg +H2O d) CH3OH+O2→CO2 + H2O

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Chapter 19 Solutions

To balance the given redox reactions:-

a) I2+Fe→FeI2

b) Cl2+H2O2→Cl−+O2

c) Hg2++H2→Hg +H2O

d) CH3OH+O2→CO2 + H2O