   Chapter 20, Problem 35PS

Chapter
Section
Textbook Problem

Methyl myristate, C13H27CO2CH3(ℓ), can be used as a biofuel. (a) Write a balanced chemical equation for the reaction that occurs when 1 mol of methyl myristate, C13H27CO2CH3(ℓ), is burned, forming CO2(g) and H2O(g). (b) Using enthalpy of formation data, calculate the standard enthalpy change for the oxidation of 1.00 mol of methyl myristate (ΔfH° = −771.0 kJ/mol) to form CO2(g) and H2O(g). (c) Which compound, methyl myristate [C13H27CO2CH3(ℓ)] or hexadecane (C16H34, one of many hydrocarbons in petroleum based diesel fuel), is predicted to provide the greater energy per mole of fuel? Per liter? (ΔfH° for C16H34 = −456.1 kJ/mol) [d(methyl myristate) = 0.86 g/mL, and d(C16H34) = 0.77 g/mL].

(a)

Interpretation Introduction

Interpretation: The balanced equation for the burning of methyl myristate has to be written.

Concept introduction:

• Balanced chemical equation of a reaction is written according to law of conservation of mass.
• Stoichiometry of a chemical reaction is the relation between reactants and products of the reaction and it is represented by the coefficients used for the reactants and products involved in the chemical equation.
Explanation

When methyl myristate is burned the gas CO2 and H2O are produced as the products.

The balanced equation for the combustion of methyl myristate is given as:

C13H27CO2CH3(l)

(b)

Interpretation Introduction

Interpretation: Enthalpy change for the oxidation of methyl myristate should be determined using the given data.

Concept introduction:

Enthalpy of combustion: At standard conditions when one mole of substance is burnt completely in presence of oxygen, the enthalpy change involved is called enthalpy of combustion.

ΔH0comb=nΔH0fproducts-nΔH0freactants

(c)

Interpretation Introduction

Interpretation: The fuel which provides more energy (Hexadecane or methyl myristate) should be determined.

Concept introduction:

Enthalpy of combustion: At standard conditions when one mole of substance is burnt completely in presence of oxygen, the enthalpy change involved is called enthalpy of combustion.

ΔH0comb=nΔH0fproducts-nΔH0freactants

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