Chapter 6, Problem 6.24P

(a)

Interpretation Introduction

Interpretation:

The chemical formula and balanced chemical equation of carbon dioxide from carbon monoxide and oxygen has to be written.

Concept Introduction:

1. 1) The chemical formula of binary compound from a pair of its constituent ion has to be written.
2. 2) The coefficients of the ions with the magnitude of the charge on each of the ions have to be crossed multiplied.  This is done to neutralize charge on the binary compound.
3. 3) The oxidation state of the metal is written in roman numbers in the brackets

Answer to Problem 6.24P

The chemical formula is ${\text{CO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{CO}}_{\text{2(g)}}\text{.}$

The balanced chemical equation is ${\text{2CO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{2CO}}_{\text{2(g)}}\text{.}$

Explanation of Solution

Carbon monoxide and oxygen exists as gas in nature.  They react with each other to form carbon dioxide.  The chemical reaction is written as,

  ${\text{CO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{CO}}_{\text{2(g)}}$

Two moles of carbon monoxide are required in the reactant side and two moles of carbon dioxide are required in the product side to make the reaction a balanced one.  The balanced equation is,

  ${\text{2CO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{2CO}}_{\text{2(g)}}$

(b)

Interpretation Introduction

Interpretation:

The chemical formula and balanced chemical equation of cesium bromide from cesium and bromine has to be written.

Concept Introduction:

Refer to part (a).

Answer to Problem 6.24P

The chemical formula is ${\text{Cs}}_{\left(\text{s}\right)}{\text{+Br}}_{\text{2(l)}}\stackrel{}{\to }{\text{CsBr}}_{\text{(s)}}.$

The balanced chemical equation is ${\text{2Cs}}_{\left(\text{s}\right)}{\text{+Br}}_{\text{2(l)}}\stackrel{}{\to }{\text{2CsBr}}_{\text{(s)}}.$

Explanation of Solution

Cesium has a monopositive charge $\left({\text{Cs}}^{\text{+}}\right)$ and bromine belongs to the group 17 and forms a mononegative anion $\left({\text{Br}}^{\text{-}}\right)$ known as bromide.  The chemical formula is,

  ${\text{Cs}}^{\text{+}}{\text{+Br}}^{\text{-}}\stackrel{}{\to }\text{CsBr}$

But bromine in nature exists as ${\text{Br}}_{\text{2}}\text{.}$  The equation becomes,

  ${\text{Cs}}_{\left(\text{s}\right)}{\text{+Br}}_{\text{2(l)}}\stackrel{}{\to }{\text{CsBr}}_{\text{(s)}}$

Two moles of cesium and two moles of cesium bromide are required in the reactant side and product side respectively to make the reaction a balanced one.  The balanced equation is,

  ${\text{Cs}}_{\left(\text{s}\right)}{\text{+Br}}_{\text{2(l)}}\stackrel{}{\to }{\text{CsBr}}_{\text{(s)}}$

(c)

Interpretation Introduction

Interpretation:

The chemical formula and balanced chemical equation of nitrogen dioxide from nitrogen monoxide and oxygen has to be written.

Concept Introduction:

Refer to part (a).

Answer to Problem 6.24P

The chemical formula is ${\text{NO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{NO}}_{\text{2}\left(\text{g}\right)}\text{.}$

The balanced chemical equation is ${\text{2NO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{2NO}}_{\text{2}\left(\text{g}\right)}\text{.}$

Explanation of Solution

Nitrogen monoxide and oxygen exists as gas in nature.  They react with each other to form nitrogen dioxide.  The chemical reaction is written as,

  ${\text{NO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{NO}}_{\text{2}\left(\text{g}\right)}$

Two moles of nitrogen monoxide are required in the reactant side and two moles of nitrogen dioxide are required in the product side to make the reaction a balanced one.  The balanced equation is,

  ${\text{2NO}}_{\left(\text{g}\right)}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{2NO}}_{\text{2}\left(\text{g}\right)}$

(d)

Interpretation Introduction

Interpretation:

The chemical formula and balanced chemical equation of nitrogen monoxide and water from ammonia and oxygen has to be written.

Concept Introduction:

Refer to part (a).

Answer to Problem 6.24P

The chemical formula is ${\text{NH}}_{\text{3(g)}}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{NO}}_{\text{(g)}}{\text{+H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}.$

The balanced chemical equation is ${\text{4NH}}_{\text{3(g)}}{\text{+5O}}_{\text{2(g)}}\stackrel{}{\to }{\text{4NO}}_{\text{(g)}}{\text{+6H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}.$

Explanation of Solution

Ammonia and oxygen exists as gas in nature.  They react with each other to form nitrogen monoxide and water.  The chemical reaction is written as,

  ${\text{NH}}_{\text{3(g)}}{\text{+O}}_{\text{2(g)}}\stackrel{}{\to }{\text{NO}}_{\text{(g)}}{\text{+H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

Four moles of ammonia and five moles of oxygen in the reactant side and four moles of nitrogen monoxide and six moles of water are required to make the reaction a balanced one.  The balanced equation is,

  ${\text{4NH}}_{\text{3(g)}}{\text{+5O}}_{\text{2(g)}}\stackrel{}{\to }{\text{4NO}}_{\text{(g)}}{\text{+6H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$