The following balanced equations represent reactions that occur in aqueous acid. Break them down into balanced oxidation and reduction half-equations. (a) 2 H;O*(aq) +H;O2(aq) + 2 Fe²* (aq) - 2 Fe** (aq) + 4 H2O(€) (b) H3O*(aq) + H2O(€) + 2 MnO (aq) + 5 SO2(aq) (aq) + 5 HSO, (aq) 2 Mn²+ (c) 5 CIO (aq) + 4 H;O* (aq) 4 CIO2(g) + CI¯(aq) + 6 H2O(e)

The following balanced equations represent reactions that occur in aqueous acid. Break them down into balanced oxidation and reduction half-equations. (a) 2 H;O(aq) +H;O2(aq) + 2 Fe² (aq) - 2 Fe** (aq) + 4 H2O(€) (b) H3O(aq) + H2O(€) + 2 MnO (aq) + 5 SO2(aq) (aq) + 5 HSO, (aq) 2 Mn²+ (c) 5 CIO (aq) + 4 H;O (aq) 4 CIO2(g) + CI¯(aq) + 6 H2O(e)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.108QE: At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction...

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At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
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