Chapter 19, Problem 83A

Interpretation Introduction

(a)

Interpretation:

Oxidation number of each element is to determine in the reaction.

Concept introduction:

Oxidation number: It is defined as charge the atom would have if electrons are not shared but transfer completely.

Answer to Problem 83A

$\begin{array}{l}\stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+4}{N}{\stackrel{-2}{O}}_2\to \stackrel{0}{N_2}+2{\stackrel{+}{H}}_2\stackrel{-2}{O}\\ \stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+5}{N}{\stackrel{-2}{O}}_3\to \stackrel{+2}{N}\stackrel{-2}{O}+2{\stackrel{+}{H}}_2\stackrel{-2}{O}\end{array}$

Explanation of Solution

The given reactions are:

$\begin{array}{l}N{H}_{4}N{O}_2\to N_2+2H_{2}O\\ N{H}_{4}N{O}_3\to NO+2H_{2}O\end{array}$

Oxidation number of elements is:

$\begin{array}{l}\stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+4}{N}{\stackrel{-2}{O}}_2\to \stackrel{0}{N_2}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\\ \stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+5}{N}{\stackrel{-2}{O}}_3\to \stackrel{+2}{N}\stackrel{-2}{O}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\end{array}$

Change in oxidation number in reaction 1:

N in NH₄=3

N in NO₂ = (-4)

Change in oxidation number in reaction 2:

N in NH₄=+5

N in NO₂ = (-3)

Interpretation Introduction

(b)

Interpretation:

The elements which are oxidized and reduced are to determine in the reaction.

Concept introduction:

Oxidation number: It is defined as charge the atom would have if electrons are not shared but transfer completely.

Answer to Problem 83A

In both reactions nitrogen is oxidized as well as reduced.

Explanation of Solution

The given reactions are:

$\begin{array}{l}N{H}_{4}N{O}_2\to N_2+2H_{2}O\\ N{H}_{4}N{O}_3\to NO+2H_{2}O\end{array}$

Oxidation number of elements is:

$\begin{array}{l}\stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+4}{N}{\stackrel{-2}{O}}_2\to \stackrel{0}{N_2}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\\ \stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+5}{N}{\stackrel{-2}{O}}_3\to \stackrel{+2}{N}\stackrel{-2}{O}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\end{array}$

Change in oxidation number in reaction 1:

N in NH₄=3

N in NO₂ = (-4)

Change in oxidation number in reaction 2:

N in NH₄=+5

N in NO₂ = (-3)

Thus in both reactions nitrogen is oxidized as well as reduced.

Interpretation Introduction

(c)

Interpretation:

The elements which are oxidizing and reducing agents are to determine in the reaction.

Concept introduction:

Oxidation number: It is defined as charge the atom would have if electrons are not shared but transfer completely.

Answer to Problem 83A

In both reactions nitrogen is oxidizing as well as reducing agent.

Explanation of Solution

The given reactions are:

$\begin{array}{l}N{H}_{4}N{O}_2\to N_2+2H_{2}O\\ N{H}_{4}N{O}_3\to NO+2H_{2}O\end{array}$

Oxidation number of elements is:

$\begin{array}{l}\stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+4}{N}{\stackrel{-2}{O}}_2\to \stackrel{0}{N_2}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\\ \stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+5}{N}{\stackrel{-2}{O}}_3\to \stackrel{+2}{N}\stackrel{-2}{O}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\end{array}$

Change in oxidation number in reaction 1:

N in NH₄=3

N in NO₂ = (-4)

Change in oxidation number in reaction 2:

N in NH₄=+5

N in NO₂ = (-3)

Thus in both reactions nitrogen is oxidizing as well as reducing agent.

Interpretation Introduction

(d)

Interpretation:

Difference in electron transfer of given reaction is to be determined.

Concept introduction:

Oxidation number: It is defined as charge the atom would have if electrons are not shared but transfer completely.

Answer to Problem 83A

In reaction:

$2AgN{O}_3+Zn\to Zn{\left(N{O}_3\right)}_2+2Ag$

Oxidizing and reducing agents are different but in the following reaction Nitrogen is oxidizing as well as reducing agent.

Explanation of Solution

The given reactions are:

$\begin{array}{l}N{H}_{4}N{O}_2\to N_2+2H_{2}O\\ N{H}_{4}N{O}_3\to NO+2H_{2}O\end{array}$

Oxidation number of elements is:

$\begin{array}{l}\stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+4}{N}{\stackrel{-2}{O}}_2\to \stackrel{0}{N_2}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\\ \stackrel{-3}{N}{\stackrel{+1}{H}}_4\stackrel{+5}{N}{\stackrel{-2}{O}}_3\to \stackrel{+2}{N}\stackrel{-2}{O}+2{\stackrel{+1}{H}}_2\stackrel{-2}{O}\end{array}$

Change in oxidation number in reaction 1:

N in NH₄=3

N in NO₂ = (-4)

Change in oxidation number in reaction 2:

N in NH₄=+5

N in NO₂ = (-3)

Thus in both reactions nitrogen is oxidizing as well as reducing agent.

In Reaction:

$2AgN{O}_3+Zn\to Zn{\left(N{O}_3\right)}_2+2Ag$

Zn is reducing agent and Ag is oxidizing agent.