Chapter 19, Problem 20E

Interpretation Introduction

(a)

Interpretation:

The balanced equation for the complete combustion of ethane is to be stated.

Concept introduction:

Combustion means the reaction of any substance with atmospheric oxygen. The process of combustion is an exothermic reaction that is energy is transferred to the surroundings. Combustion of alkane forms water and carbon dioxide as a byproduct.

Answer to Problem 20E

The balanced equation for the complete combustion of ethane is stated below.

${\text{2C}}_2{\text{H}}_6+7{\text{O}}_{\text{2}}\to 4{\text{CO}}_{\text{2}}+6{\text{H}}_{\text{2}}\text{O}$

Explanation of Solution

The general reaction for the combustion of an alkane is shown below.

${\text{C}}_{\text{n}}{\text{H}}_{\text{2n+2}}+\left(\frac{\text{3n+1}}{\text{2}}\right){\text{O}}_{\text{2}}\to {\text{nCO}}_{\text{2}}+\left(\text{n}+\text{1}\right){\text{H}}_{\text{2}}\text{O}$

Where

• n is the number of carbon atoms.

The number of carbon atom present in ethane is $2$. Therefore, the value of $\text{n}$ is $2$. Substitute $\text{n}=2$ in the above reaction. Multiply the whole reaction by a coefficient $2$ to convert the atoms of ${\text{O}}_{\text{2}}$ into a whole number.

The balanced chemical reaction of combustion of ethane is stated below.

${\text{2C}}_2{\text{H}}_6+7{\text{O}}_{\text{2}}\to 4{\text{CO}}_{\text{2}}+6{\text{H}}_{\text{2}}\text{O}$

Conclusion

The balanced equation of ethane is stated above.

Interpretation Introduction

(b)

Interpretation:

The balanced equation for the complete combustion of butane is to be stated.

Concept introduction:

Combustion means the reaction of any substance with atmospheric oxygen. The process of combustion is an exothermic reaction that is energy is transferred to the surroundings. Combustion of alkane forms water and carbon dioxide as a byproduct.

Answer to Problem 20E

The balanced equation for the complete combustion of butane is stated below.

${\text{2C}}_4{\text{H}}_{10}+13{\text{O}}_{\text{2}}\to 8{\text{CO}}_{\text{2}}+10{\text{H}}_{\text{2}}\text{O}$

Explanation of Solution

The general reaction for the combustion of an alkane is shown below.

${\text{C}}_{\text{n}}{\text{H}}_{\text{2n+2}}+\left(\frac{\text{3n+1}}{\text{2}}\right){\text{O}}_{\text{2}}\to {\text{nCO}}_{\text{2}}+\left(\text{n}+\text{1}\right){\text{H}}_{\text{2}}\text{O}$

Where

• n is the number of carbon atoms.

The number of carbon atom present in butane is $4$. Therefore, the value of $\text{n}$ is $4$. Substitute $\text{n}=4$ in the above reaction. Multiply the whole reaction by a coefficient $2$ to convert the atoms of ${\text{O}}_{\text{2}}$ into a whole number.

The balanced chemical reaction of combustion of butane is stated below.

${\text{2C}}_4{\text{H}}_{10}+13{\text{O}}_{\text{2}}\to 8{\text{CO}}_{\text{2}}+10{\text{H}}_{\text{2}}\text{O}$

Conclusion

The balanced equation of butane is stated above.

Interpretation Introduction

(c)

Interpretation:

The balanced equation for the complete combustion of pentane is to be stated.

Concept introduction:

Combustion means the reaction of any substance with atmospheric oxygen. The process of combustion is an exothermic reaction that is energy is transferred to the surroundings. Combustion of alkane forms water and carbon dioxide as a byproduct.

Answer to Problem 20E

The balanced equation for the complete combustion of pentane is stated below.

${\text{2C}}_5{\text{H}}_{12}+16{\text{O}}_{\text{2}}\to 10{\text{CO}}_{\text{2}}+12{\text{H}}_{\text{2}}\text{O}$

Explanation of Solution

The general reaction for the combustion of an alkane is shown below.

${\text{C}}_{\text{n}}{\text{H}}_{\text{2n+2}}+\left(\frac{\text{3n+1}}{\text{2}}\right){\text{O}}_{\text{2}}\to {\text{nCO}}_{\text{2}}+\left(\text{n}+\text{1}\right){\text{H}}_{\text{2}}\text{O}$

Where

• n is the number of carbon atoms.

The number of carbon atom present in pentane is $5$. Therefore, the value of $\text{n}$ is $5$. Substitute $\text{n}=5$ in the above reaction. Multiply the whole reaction by a coefficient $2$ to convert the atoms of ${\text{O}}_{\text{2}}$ into a whole number.

The balanced chemical reaction of combustion of pentane is stated below.

${\text{2C}}_5{\text{H}}_{12}+16{\text{O}}_{\text{2}}\to 10{\text{CO}}_{\text{2}}+12{\text{H}}_{\text{2}}\text{O}$

Conclusion

The balanced equation of pentane is stated above.

Interpretation Introduction

(d)

Interpretation:

The balanced equation for the complete combustion of heptane is to be stated.

Concept introduction:

Combustion means the reaction of any substance with atmospheric oxygen. The process of combustion is an exothermic reaction that is energy is transferred to the surroundings. Combustion of alkane forms water and carbon dioxide as a byproduct.

Answer to Problem 20E

The balanced equation for the complete combustion of heptane is stated below.

${\text{2C}}_7{\text{H}}_{16}+22{\text{O}}_{\text{2}}\to 14{\text{CO}}_{\text{2}}+16{\text{H}}_{\text{2}}\text{O}$

Explanation of Solution

The general reaction for the combustion of an alkane is shown below.

${\text{C}}_{\text{n}}{\text{H}}_{\text{2n+2}}+\left(\frac{\text{3n+1}}{\text{2}}\right){\text{O}}_{\text{2}}\to {\text{nCO}}_{\text{2}}+\left(\text{n}+\text{1}\right){\text{H}}_{\text{2}}\text{O}$

Where

• n is the number of carbon atoms.

The number of carbon atom present in heptane is $7$. Therefore, the value of $\text{n}$ is $7$. Substitute $\text{n}=7$ in the above reaction. Multiply the whole reaction by a coefficient $2$ to convert the atoms of ${\text{O}}_{\text{2}}$ into a whole number.

The balanced chemical reaction of combustion of heptane is stated below.

${\text{2C}}_7{\text{H}}_{16}+22{\text{O}}_{\text{2}}\to 14{\text{CO}}_{\text{2}}+16{\text{H}}_{\text{2}}\text{O}$

Conclusion

The balanced equation of heptane is stated above.