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Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404

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BuyFindarrow_forward

Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404
Textbook Problem

  1. a. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and carbon dioxide gas.
  2. 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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