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Balance the redox reactions using the half-reaction method. Identify the reducing agent (Substance Oxidized) and oxidizing agent (Substance Reduced). (From: Principles of Chemistry Laboratory Manual) 1. S2O3 2- + I2 → I - + S4O6 2- (in acidic medium) 2. MnO4 - + I- → MnO2 + I2 (in basic medium)

Balance the redox reactions using the half-reaction method. Identify the reducing agent (Substance Oxidized) and oxidizing agent (Substance Reduced). (From: Principles of Chemistry Laboratory Manual) 1. S2O3 2- + I2 → I - + S4O6 2- (in acidic medium) 2. MnO4 - + I- → MnO2 + I2 (in basic medium)

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Chemistry
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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
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Balance the redox reactions using the half-reaction

method. Identify the reducing agent (Substance Oxidized) and

oxidizing agent (Substance Reduced). (From: Principles of

Chemistry Laboratory Manual)

1. S2O3

2- + I2 → I

- + S4O6

2-

(in acidic medium)

2. MnO4

- + I- → MnO2 + I2 (in basic medium)

Exercise 1: Balance the redox reactions using the half-reaction method. Identify the reducing agent (Substance Oxidized) and oxidizing agent (Substance Reduced). (From: Principles of Chemistry Laboratory Manual) 1. S2032- + 12 →I+ S4O6² (in acidic medium) 2. MnO4 + l → MnO2 + 12 (in basic medium)
Transcribed Image Text:Exercise 1: Balance the redox reactions using the half-reaction method. Identify the reducing agent (Substance Oxidized) and oxidizing agent (Substance Reduced). (From: Principles of Chemistry Laboratory Manual) 1. S2032- + 12 →I+ S4O6² (in acidic medium) 2. MnO4 + l → MnO2 + 12 (in basic medium)
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