Chapter 10, Problem 10.150MP

Interpretation Introduction

(a)

Interpretation:

The empirical formula of methyl-tert-butyl ether is to be determined.

Concept introduction:

The formula to calculate number of moles as per ideal gas equation is as follows:

$n=\frac{PV}{RT}$

Where,

• $R$ is gas constant.
• $V$ denotes the volume.
• $n$ denotes number of moles.
• $T$ denotes temperature.
• $P$ denotes pressure.

Interpretation Introduction

(b)

Interpretation:

The molecular formula and molecular weight of methyl-tert-butyl ether is to be determined.

Concept introduction:

The formula to calculate number of moles as per ideal gas equation is as follows:

$n=\frac{PV}{RT}$

Where,

• $R$ is gas constant.
• $V$ denotes the volume.
• $n$ denotes number of moles.
• $T$ denotes temperature.
• $P$ denotes pressure.

Interpretation Introduction

(c)

Interpretation:

The balanced reaction corresponding to combustion of methyl-tert-butyl ether should be determined.

Concept introduction:

The combustion involves the ignition of hydrocarbon in presence of ${\text{O}}_2$ that generates ${\text{CO}}_2$ and ${\text{H}}_{\text{2}}\text{O}$ as products.As per law of conservation of mass, the total amount of reactants consumed is equal to total amount of products formed in any balanced equation.

Interpretation Introduction

(c)

Interpretation:

The enthalpy of formation of methyl-tert-butyl ether is to be determined.

Concept introduction:

The balanced reaction corresponding to combustion of methyl-tert-butyl ether is as follows:

${\text{C}}_5{\text{H}}_{\text{12}}{\text{O}}_1+\frac{15}{2}{\text{O}}_2\to 5{\text{CO}}_2+6{\text{H}}_{\text{2}}\text{O}$

The enthalpy of formation can be calculated using the following formula:

$\Delta H°=\left[5\Delta H_{\text{f}}°\left({\text{CO}}_2\right)+6\Delta H_{\text{f}}°\left({\text{H}}_{\text{2}}\text{O}\right)\right]-\left[1\Delta H_{\text{f}}°\left({\text{C}}_5{\text{H}}_{\text{12}}{\text{O}}_1\right)+\frac{15}{2}\Delta H_{\text{f}}°\left({\text{O}}_2\right)\right]$