Interpretation Introduction Interpretation: Each of the given redox reaction that occurs in aqueous acidic medium is to be balanced. Explanation We have the following redox reaction: I − ( a q ) + N O 2 − → I 2 ( s ) + N O ( g ) Step 1: Separate the overall reaction into two half-reactions: one for oxidation and one for reduction. O x i d a t i o n : I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) → N O ( g ) Step 2: Balance the elements, excluding H, O. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) → N O ( g ) Step 3: Balance the elements H, O. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) Reduction : N O 2 − ( s ) + 2 H + ( a q ) → N O ( g ) + H 2 O ( l ) In these half-reactions, all elements are balanced, including H, O. Hence, in the next step we need to balance the charge. Step 4: Balance each half-reaction with respect to charge by adding electrons. O x i d a t i o n : 2 I − ( a q ) → I 2 ( s ) + 2 e − Reduction : N O 2 − ( s ) + 2 H + ( a q ) + 1 e − → N O ( g ) + H 2 O ( l ) Step 5: Make the number of electrons in both half-reactions equal by multiplying one or both half reactions by a small whole number. O x i d a t i o n : [ 2 I − ( a q ) → I 2 ( s ) + 2 e − ] × 1 Reduction : [ N O 2 − ( s ) + 2 H + ( a q ) + 1 e − → N O ( g ) + H 2 O ( l ) ] × 2 Add these two reactions to get the balanced reaction. 2 N O 2 − ( s ) + 4 H + ( a q ) + 2 I − ( a q ) → 2 N O ( g ) + 2 H 2 O ( l ) + I 2 ( s ) We have the following redox reaction: C l O 4 − ( a q ) + C l − ( a q ) → C l O 3 − ( a q ) + C l 2 ( g ) Step 1: Separate the overall reaction into two half-reactions: one for oxidation and one for reduction. O x i d a t i o n : C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) → C l O 3 − ( a q ) Step 2: Balance the elements, excluding H, O. O x i d a t i o n : 2 C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) → C l O 3 − ( a q ) Step 3: Balance the elements H, O. O x i d a t i o n : 2 C l − ( a q ) → C l 2 ( s ) Reduction : C l O 4 − ( a q ) + 2 H + ( a q ) → C l O 3 − ( a q ) + H 2 O ( l ) In these half-reactions, all elements are balanced, including H, O

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Chapter 19, Problem 40E

Interpretation Introduction

Interpretation: Each of the given redox reaction that occurs in aqueous acidic medium is to be balanced.

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Chapter 19, Problem 39E

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Chemistry: A Molecular Approach (4th 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