
(a)
Interpretation:
The given
Concept Introduction:
The
(a)

Answer to Problem 16QRT
The
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The carbon atoms in the given redox reaction are balanced. The oxygen atoms are balanced by putting
The above balanced reaction is multiplied by
Thus, the balanced chemical reaction is shown below.
The oxidation number of carbon atom in
The oxidation number of oxygen atom in
(b)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(b)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The hydrogen atoms and chlorine atoms are balanced by putting
The above balanced reaction is multiplied by
Thus, the balanced chemical reaction is shown below.
The oxidation number of hydrogen atom in
The oxidation number of chlorine atom in
(c)
Interpretation:
The given redox reaction is to be balanced in acidic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(c)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of titanium atom in
The oxidation number of oxygen atom in
The given unbalanced redox reaction is shown below.
The oxidation number of titanium atom in
The oxidation number of oxygen atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(d)
Interpretation:
The given redox reaction is to be balanced in acidic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(d)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of chlorine atom in
The oxidation number of manganese atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since the electron gain is not equivalent to electron lost. Thus, multiply the oxidation half reaction by
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(e)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(e)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of iron atom in
The oxidation number of oxygen atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The iron atom and sulphur atoms are balanced by putting
Oxidation:
Reduction:
The given reaction is to be balanced in acidic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, now hydrogen atoms are balanced by adding protons
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Since the electron gain is not equivalent to electron lost. Thus, multiply the oxidation half reaction by
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
(f)
Interpretation:
The given redox reaction is to be balanced and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(f)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given redox reaction is shown below.
The given redox reaction is already balanced and there are equal numbers of each atom both the sides.
The oxidation number of nitrogen atom in
The oxidation number of oxygen atom in
(g)
Interpretation:
The given redox reaction is to be balanced in basic medium and the oxidizing agent and reducing agent are to be identified.
Concept Introduction:
Same as part (a).
(g)

Answer to Problem 16QRT
The balanced redox reaction is shown below.
In this reaction,
Explanation of Solution
The given unbalanced redox reaction is shown below.
The oxidation number of zinc atom in
The oxidation number of mercury atom in
Therefore, the unbalanced half reactions are shown below.
Oxidation:
Reduction:
The given reaction is to be balanced in basic medium. Therefore, oxygen atoms are balanced by adding water molecules to the deficient side.
Oxidation:
Reduction:
After balancing oxygen atoms, hydrogen atoms are balanced by adding water molecules
Oxidation:
Reduction:
The charge is on both sides is balanced by adding electrons to the more positive side of the half- reaction to equal the less positive side of the half- reaction.
Oxidation:
Reduction:
Now, there is the equal loss and gain of electron in the above two half-cell reactions. Therefore, the overall cell reaction is get by addition the above two half-cell reactions.
The simplified chemical equation after removing the chemical species of the similar kind is shown below.
Thus, the balanced chemical reaction is shown below.
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Chapter 17 Solutions
Bundle: Chemistry: The Molecular Science, 5th, Loose-Leaf + OWLv2 with Quick Prep 24-Months Printed Access Card
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