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: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
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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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