
. Iodide ion, I- , is one of the most easily oxidized species. Balance each of the following
a.

(a)
Interpretation:
The given oxidation-reduction reaction should be balanced using the half-reaction method.
Concept Introduction:
The oxidation-reduction reaction is also known as a redox reaction. In this reaction, one reactant is oxidized and other is reduced. In balancing an oxidation-reduction reaction they must be first divided into two half reactions: one is oxidation reaction and other is reduction reaction.
The balancing of redox reaction is complicated as compared to simple balancing. It is necessary to determine the half reactions of reactants undergoing oxidation and reduction. On adding the two half-reactions, net total equation can be obtained. This method of balancing redox reaction is known as half equation method.
The following rules must be followed in balancing redox reaction by half equation method:
- Initially, redox reaction is separated into two half equations; oxidation and reduction.
- Atoms other than hydrogen and oxygen are balanced first in the unbalanced half equations.
- Oxygen atoms are balanced by addition of water on either side of the reaction.
- Hydrogen ion/s is added to balance the hydrogen atom.
- Electrons are added to balance the charge.
- Half reactions are added to get the net total equation.
- The further addition of hydroxide ion takes place on both side of the reaction, if the solution is basic in nature to neutralise the hydrogen ion present in the solution.
Answer to Problem 47QAP
Explanation of Solution
The given reaction is as follows:
The above reaction can be separated into two half reactions as follows:
Here,
To balance the reaction (1), give coefficient 2 to
Now, oxygen atom can be balanced by adding 6 water molecules to right thus,
Next step is to balance hydrogen atoms by adding 12 hydrogen ions to the left:
The last step is to balance the charge thus, 4 electrons are added to left thus,
Now, balance reaction (2) by given coefficient 2 to
Now, charge can be balanced by adding 2 electrons to the right thus,
To get the net reaction, add reaction (3) and (4) as follows:
Thus, the balanced chemical reaction is as follows:

(b)
Interpretation:
The given oxidation-reduction reaction should be balanced using the half-reaction method.
Concept Introduction:
The oxidation-reduction reaction is also known as a redox reaction. In this reaction, one reactant is oxidized and other is reduced. In balancing an oxidation-reduction reaction they must be first divided into two half reactions: one is oxidation reaction and other is reduction reaction.
The balancing of redox reaction is complicated as compared to simple balancing. It is necessary to determine the half reactions of reactants undergoing oxidation and reduction. On adding the two half-reactions, net total equation can be obtained. This method of balancing redox reaction is known as half equation method.
The following rules must be followed in balancing redox reaction by half equation method:
- Initially, redox reaction is separated into two half equations; oxidation and reduction.
- Atoms other than hydrogen and oxygen are balanced first in the unbalanced half equations.
- Oxygen atoms are balanced by addition of water on either side of the reaction.
- Hydrogen ion/s is added to balance the hydrogen atom.
- Electrons are added to balance the charge.
- Half reactions are added to get the net total equation.
- The further addition of hydroxide ion takes place on both side of the reaction, if the solution is basic in nature to neutralise the hydrogen ion present in the solution.
Answer to Problem 47QAP
Explanation of Solution
The given reaction is as follows:
The two reactions can be separated into half reactions as follows:
And,
Reaction (1) can be balanced by giving coefficient 2 to
Add 7 water molecules to the right to balance oxygen atoms thus,
Hydrogen atom can be balanced by adding 14 hydrogen ions to the left
Last step is to balance the charge, the net charge on left side is + 12 and on right side is + 6 thus, 6 electrons are added to left to balance the charge thus,
In reaction (2), iodine atom is balanced by giving coefficient 2 to
Next step is to balance the charge; two electrons are added to the right to balance the two negative charges on left side:
To get the net reaction, add reaction (3) and (4) as follows:
Thus, the balanced chemical reaction is as follows:

(c)
Interpretation:
The given oxidation-reduction reaction should be balanced using the half-reaction method.
Concept Introduction:
The oxidation-reduction reaction is also known as a redox reaction. In this reaction, one reactant is oxidized and other is reduced. In balancing an oxidation-reduction reaction they must be first divided into two half reactions: one is oxidation reaction and other is reduction reaction.
The balancing of redox reaction is complicated as compared to simple balancing. It is necessary to determine the half reactions of reactants undergoing oxidation and reduction. On adding the two half-reactions, net total equation can be obtained. This method of balancing redox reaction is known as half equation method.
The following rules must be followed in balancing redox reaction by half equation method:
- Initially, redox reaction is separated into two half equations; oxidation and reduction.
- Atoms other than hydrogen and oxygen are balanced first in the unbalanced half equations.
- Oxygen atoms are balanced by addition of water on either side of the reaction.
- Hydrogen ion/s is added to balance the hydrogen atom.
- Electrons are added to balance the charge.
- Half reactions are added to get the net total equation.
- The further addition of hydroxide ion takes place on both side of the reaction, if the solution is basic in nature to neutralise the hydrogen ion present in the solution.
Answer to Problem 47QAP
Explanation of Solution
The given reaction is as follows:
The above reaction can be separated into two half reactions as follows:
And,
In reaction (1), charge can be balanced by adding electrons. Since, there is + 1 charge on left thus, 1 electron is added to left:
Now, in reaction (2), iodine atom can be balanced by giving coefficient 2 to
The charge can be balanced by adding 2 electrons to the right thus,
To get the net reaction, add reaction (3) and (4) as follows:
Thus, the balanced chemical reaction is as follows:
Want to see more full solutions like this?
Chapter 18 Solutions
Introductory Chemistry: A Foundation
- The molecule PYRIDINE, 6th electrons and is therefore aromatre and is Assigned the Following structure contering Since aromatk moleculoy undergo electrophilic anomatic substitution, Pyridine shodd undergo The Following reaction + HNO3 12504 a. write all of the possible Mononitration Products that could Result From this reaction 18. Bared upon the reaction mechanison determime which of these producty would be the major Product of the hegetionarrow_forwarda. Explain Why electron withdrawing groups tend to be meta-Directors. Your answer Should lyclude all apropriate. Resonance contributing Structures fo. Explain why -ll is an outho -tura drccton even though chlorine has a very High Electronegativityarrow_forward9. Write Me product as well as the reaction Mechanism For each of the Following Vanctions +H₂504 4.50+ T C. +212 Fellz 237 b. Praw the potential energy Diagrams For each OF Mese Rauctions and account For any differences that appear in the two potential Puergy Diagrams which of here two reactions 19 Found to be Reversable, Rationalice your answer based upon the venation mechanisms and the potential energy diagrams.arrow_forward
- 9. Write Me product as well as the reaction Mechanism For each of the Following Veritious +H2504 4.50+ + 1/₂ Felly ◎+ 7 b. Praw he potential energy Diagrams For each OF Mese Ronctions and account for any differences that appeak in the two potential Puergy Diagramsarrow_forwardDraw the major product of this reaction. Ignore inorganic byproducts. Incorrect, 3 attempts remaining 1. excess Br2, NaOH 2. neutralizing workup Qarrow_forwardGiven the electrode Pt | Ag | Ag+ (aq), describe it.arrow_forward
- At 25°C, the reaction Zn2+ + 2e ⇄ Zn has a normal equilibrium potential versus the saturated calomel electrode of -1.0048 V. Determine the normal equilibrium potential of Zn versus the hydrogen electrode.Data: The calomel electrode potential is E° = 0.2420 V versus the normal hydrogen electrode.arrow_forwardElectrochemistry. State the difference between E and E0.arrow_forwardIn an electrolytic cell, the positive pole is always assumed to be on the right side of the battery notation. Is that correct?arrow_forward
- In an electrolytic cell, the positive pole is always assumed to be on the right side of the battery. Is that correct?arrow_forwardCalculate the free energy of formation of 1 mol of Cu in cells where the electrolyte is 1 mol dm-3 Cu2+ in sulfate solution, pH 0. E° for the Cu2+/Cu pair in this medium is +142 mV versus ENH.Assume the anodic reaction is oxygen evolution.Data: EH2 = -0.059 pH (V) and EO2 = 1.230 - 0.059 pH (V); 2.3RT/F = 0.059 Varrow_forwardIf the normal potential for the Fe(III)/Fe(II) pair in acid at zero pH is 524 mV Hg/Hg2Cl2 . The potential of the saturated calomel reference electrode is +246 mV versus the NHE. Calculate E0 vs NHE.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning





