Using the steps below how do you balance the oxidation/reduction reaction In Acidic solution:H2C204 (ag) + Mno, (aq)Mn2* (ag) + Co3 (g)(acidic)1.Write the two half- reactions (Oxidation and reduction reaction)2.Balance the atoms undergoing oxidation and reduction/ all other atoms other than"о" and "H"3.Balance atoms and charges in each half-reaction.Use H20 to balance o atoma.a.b.Use H* to balance H atomsC.Use e to balance positive charges4. Multiply each half-reaction by some integer so the the number of e-lost in theOxidation half-reaction equals the number of e gained in the Reduction half-reaction5.Add the half - reactions together, canceling species that appear on both sides.The e must completely cancel and not be present in the end.

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Answered: Using the steps below how do you…

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Using the steps below how do you balance the oxidation/reduction reaction

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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Concept explainers

Redox Reactions

Redox reactions are considered to be the chemical reactions involving both oxidation and reduction processes. They are actually oxidation-reduction reactions. The term redox is made from two words where “red” comes from reduction and “ox” comes from oxidation. During a redox reaction electron transfer takes place in such a way that one chemical compound gets reduced and the other one gets oxidized.

Question

Using the steps below how do you balance the oxidation/reduction reaction

In Acidic solution:
H2C204 (ag) + Mno, (aq)
Mn2* (ag) + Co3 (g)
(acidic)
1.
Write the two half- reactions (Oxidation and reduction reaction)
2.
Balance the atoms undergoing oxidation and reduction/ all other atoms other than
"о" and "H"
3.
Balance atoms and charges in each half-reaction.
Use H20 to balance o atoma.
a.
b.
Use H* to balance H atoms
C.
Use e to balance positive charges
4. Multiply each half-reaction by some integer so the the number of e-lost in the
Oxidation half-reaction equals the number of e gained in the Reduction half-
reaction
5.
Add the half - reactions together, canceling species that appear on both sides.
The e must completely cancel and not be present in the end.

Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.

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