(a)
Interpretation: Whether silver in the reaction is oxidized or reduced is to be determined.
Concept Introduction: The species that involves the loss of electrons are said to be oxidized while the one that involves the gain of electrons is said to be reduced.
(a)
Answer to Problem 56A
Silver is oxidized in the reaction.
Explanation of Solution
In the reaction,
The half-reactions involved are,
Oxidation:
Reduction:
The removal of electrons is taking place in
(b)
Interpretation: The oxidizing and reducing agents in the given reaction,
Concept Introduction: The species that undergo reduction is identified as an oxidizing agent while the one that undergoes oxidation is identified as a reducing agent.
(b)
Answer to Problem 56A
Reducing agent is
Explanation of Solution
In the reaction,
The half-reactions involved are,
Oxidation:
Reduction:
The removal of electrons is taking place in
So, the reducing agent is
(c)
Interpretation: The given chemical equation,
Concept Introduction: The
- First, the given redox reaction is divided into half reactions one oxidation and the other reduction.
- Based on mass and charge the half-reactions are balanced.
- The electrons on both sides of the reaction are equalized.
- Then add the half-reactions together and the common one is eliminated to get the balanced equation.
(c)
Answer to Problem 56A
The balanced chemical equation is,
Explanation of Solution
In the reaction,
The half-reactions involved are,
Oxidation:
Reduction:
The half-reaction can be balanced first by multiplying 2 by Ag.
So the equation becomes,
All the other chemical species are equal. So the balanced equation is,
Chapter 20 Solutions
Chemistry 2012 Student Edition (hard Cover) Grade 11
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