Guidelines for Balancing Redox Equations:Determine the oxidation states of each species.Write each half reaction and for each:Balance atoms that change oxidation state.Determine number of electrons gained or lostBalance charges by using H+ (in acidic solution) or OH- (in basic solution).Balance the rest of the atoms (H's and O's) using H2O.Balance the number of electrons transferred for each half reaction using the appropriate factor so that the electrons cancel.Add the two half-reactions together and simplify if necessary. Balance the following redox reactions.1. Hg₂²+ (aq) + Sn²+ (aq) → Hg() +2. Al(s) +2H* (aq)+ 2Cl → Al³+ (aq)3. HN2NNH2 +103 + CI™4. Ti³+ + Fe(CN)6³-→5. Ag(s) + I + Sn4+TiO²+ +Sn4+ (aq)+ H2(g) +N2 (8) + ICI₂Fe(CN)64-Sn²+Agl(s) +2Cl(aq)

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Answered: Balance the following redox reactions.…

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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Guidelines for Balancing Redox Equations:

Determine the oxidation states of each species.
Write each half reaction and for each:
1. Balance atoms that change oxidation state.
2. Determine number of electrons gained or lost
3. Balance charges by using H⁺ (in acidic solution) or OH^- (in basic solution).
4. Balance the rest of the atoms (H's and O's) using H₂O.
Balance the number of electrons transferred for each half reaction using the appropriate factor so that the electrons cancel.
Add the two half-reactions together and simplify if necessary.

Balance the following redox reactions.
1. Hg₂²+ (aq) + Sn²+ (aq) → Hg() +
2. Al(s) +
2H* (aq)
+ 2Cl → Al³+ (aq)
3. HN2NNH2 +
103 + CI™
4. Ti³+ + Fe(CN)6³-→
5. Ag(s) + I + Sn4+
TiO²+ +
Sn4+ (aq)
+ H2(g) +
N2 (8) + ICI₂
Fe(CN)64-
Sn²+
Agl(s) +
2Cl(aq)

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