Chapter 19, Problem 35E

Interpretation Introduction

(a)

Interpretation:

A balanced equation for the reaction ${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to$ is to be stated.

Concept introduction:

The reaction of hydrocarbon in the presence of oxygen to give carbon dioxide and water is known as combustion reaction. Complete combustion of any hydrocarbons always gives oxide of carbon and hydrogen. The reason for this is that hydrocarbons consist of hydrogen and carbon.

Answer to Problem 35E

A balanced equation for the reaction ${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+3{\text{O}}_{\text{2}}\to 2{\text{CO}}_{\text{2}}+{\text{2H}}_{\text{2}}\text{O}$

Explanation of Solution

The given reaction is a combustion reaction. Complete combustion of any hydrocarbons always gives carbon dioxide and water as final product. The alkenes react with oxygen forms carbon dioxide and water. The corresponding reaction is shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to {\text{CO}}_{\text{2}}+{\text{H}}_{\text{2}}\text{O}$

In the above reaction, the number of carbon atoms on the reactant side is two and on the product side is one. The number of hydrogen atoms on the reactant side is four and on the product side is two. Therefore, the number of carbon and hydrogen atoms is balanced as shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to 2{\text{CO}}_{\text{2}}+2{\text{H}}_{\text{2}}\text{O}$

Now, the number of oxygen atoms on the reactant side is two and on the product side are six. Therefore, the number of oxygen atoms is balanced as shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+3{\text{O}}_{\text{2}}\to 2{\text{CO}}_{\text{2}}+2{\text{H}}_{\text{2}}\text{O}$

Therefore, the balanced equation for the reaction ${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+3{\text{O}}_{\text{2}}\to 2{\text{CO}}_{\text{2}}+2{\text{H}}_{\text{2}}\text{O}$

Conclusion

A balanced equation for the reaction ${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+{\text{O}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{2}}={\text{CH}}_{\text{2}}+3{\text{O}}_{\text{2}}\to 2{\text{CO}}_{\text{2}}+{\text{2H}}_{\text{2}}\text{O}$

Interpretation Introduction

(b)

Interpretation:

A balanced equation for the reaction ${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to$ is to be stated.

Concept introduction:

The reaction of hydrocarbon in the presence of oxygen to give carbon dioxide and water is known as combustion reaction. Complete combustion of any hydrocarbons always gives oxide of carbon and hydrogen. The reason for this is that hydrocarbons consist of hydrogen and carbon.

Answer to Problem 35E

A balanced equation for reaction ${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to {\text{CH}}_{\text{3}}-{\text{CH}}_2-{\text{CH}}_{\text{3}}$

Explanation of Solution

The reaction of alkenes with hydrogen gives alkanes as the final product. This reaction is known as reduction reaction. The reaction of propene with hydrogen is shown below.

${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to {\text{CH}}_{\text{3}}-{\text{CH}}_2-{\text{CH}}_{\text{3}}$

In the above reaction, the number of carbon and hydrogen atoms is same on the both sides. Therefore, the above reaction is balanced. The balanced equation for reaction ${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to {\text{CH}}_{\text{3}}-{\text{CH}}_2-{\text{CH}}_{\text{3}}$

Conclusion

A balanced equation for reaction ${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to$ is shown below.

${\text{CH}}_{\text{3}}-\text{CH}={\text{CH}}_{\text{2}}+{\text{H}}_{\text{2}}\to {\text{CH}}_{\text{3}}-{\text{CH}}_2-{\text{CH}}_{\text{3}}$