   Chapter 3, Problem 114E

Chapter
Section
Textbook Problem

a. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and carbon dioxide gas. b. Assuming gasoline is 100.% isooctane, with a density of 0.692 g/mL, what is the theoretical yield of carbon dioxide produced by the combustion of 1.2 × 1010 gal of gasoline (the approximate annual consumption of gasoline in the United States)?

(a)

Interpretation Introduction

Interpretation:

The balanced equation for combustion of Isooctane should be written.

Concept introduction:

Balanced equation:

• The balanced equation is nothing but the all ionic compounds are represented as neutral compounds using the molecular formula.
• In the balanced equation, the number of atoms for each element and total charge are equal in the reaction for in both reactants and the products sides.

Mole:

The ratio between mass of the sample taken and molar mass of compound to give a mole of the analyte present in taken gram of sample.

Mole=MassMolarmass

Explanation

To write the balanced equation for combustion of isooctane

One mole of isooctane reacts with 12.5 mole of Oxygen to gives 8 mole of Carbon dioxide and 9 mole of water.

Hence the balanced equation for combustion of Isooctane is,

C8H18 + 12

(b)

Interpretation Introduction

Interpretation:

Theoretical yield of carbon dioxide from combustion given gasoline should be calculated.

Concept introduction:

Balanced equation:

• The balanced equation is nothing but the all ionic compounds are represented as neutral compounds using the molecular formula.
• In the balanced equation, the number of atoms for each element and total charge are equal in the reaction for in both reactants and the products sides.

Mole:

The ratio between mass of the sample taken and molar mass of compound to give a mole of the analyte present in taken gram of sample.

Mole=MassMolarmass

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