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Consider the following unbalanced, net ionic, reduction-oxidation expression MnO4- (aq) + Cl2 (g) --> Mn2+ (aq) + ClO- (aq) A) Balance the Mn containing half-reaction in acidic solution. (You do not need to include the state symbols.) MnO4-                           -->                        Mn2+       B) Balance the Cl containing half-reaction in acidic solution. (You do not need to include the state symbols.)   Cl2                                       -->                             ClO-

Consider the following unbalanced, net ionic, reduction-oxidation expression MnO4- (aq) + Cl2 (g) --> Mn2+ (aq) + ClO- (aq) A) Balance the Mn containing half-reaction in acidic solution. (You do not need to include the state symbols.) MnO4-                           -->                        Mn2+       B) Balance the Cl containing half-reaction in acidic solution. (You do not need to include the state symbols.)   Cl2                                       -->                             ClO-

Chemistry
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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Consider the following unbalanced, net ionic, reduction-oxidation expression

MnO4- (aq) + Cl2 (g) --> Mn2+ (aq) + ClO- (aq)

A) Balance the Mn containing half-reaction in acidic solution. (You do not need to include the state symbols.)

MnO4-                           -->                        Mn2+    

 

B) Balance the Cl containing half-reaction in acidic solution. (You do not need to include the state symbols.)

 

Cl2                                       -->                             ClO-

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