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Ex: Balance the oxidation of Fe2+ to Fe3+ by Cr2O72- in acid solution. Cr3+ is the reduction product. 1. Write the unbalanced equation. Fe2+ + Cr2O72- Fe3+ + Cr3+ 2. Separate the equation into two half-reactions: Oxidation: Reduction: +6 +2 Fe2+ 11 Cr2O72- +3 Fe3+ +3 Cr3+ 3. Balance the atoms other than O and H in each half-reaction. +2 Fe2+ 11 Cr₂O2-- +3 Fe3+ 2 Cr3+

Ex: Balance the oxidation of Fe2+ to Fe3+ by Cr2O72- in acid solution. Cr3+ is the reduction product. 1. Write the unbalanced equation. Fe2+ + Cr2O72- Fe3+ + Cr3+ 2. Separate the equation into two half-reactions: Oxidation: Reduction: +6 +2 Fe2+ 11 Cr2O72- +3 Fe3+ +3 Cr3+ 3. Balance the atoms other than O and H in each half-reaction. +2 Fe2+ 11 Cr₂O2-- +3 Fe3+ 2 Cr3+

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter20: Electrochemistry
Section: Chapter Questions
Problem 30A
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Ex: Balance the oxidation of Fe2+ to Fe3+ by Cr2O72- in acid solution. Cr3+ is the reduction product. 1. Write the unbalanced equation. Fe2+ + Cr2O72- Fe3+ + Cr3+ 2. Separate the equation into two half-reactions: Oxidation: Reduction: +6 +2 Fe2+ 11 Cr2O72- +3 Fe3+ +3 Cr3+ 3. Balance the atoms other than O and H in each half-reaction. +2 Fe2+ 11 Cr₂O2-- +3 Fe3+ 2 Cr3+
Transcribed Image Text:Ex: Balance the oxidation of Fe2+ to Fe3+ by Cr2O72- in acid solution. Cr3+ is the reduction product. 1. Write the unbalanced equation. Fe2+ + Cr2O72- Fe3+ + Cr3+ 2. Separate the equation into two half-reactions: Oxidation: Reduction: +6 +2 Fe2+ 11 Cr2O72- +3 Fe3+ +3 Cr3+ 3. Balance the atoms other than O and H in each half-reaction. +2 Fe2+ 11 Cr₂O2-- +3 Fe3+ 2 Cr3+
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