Chapter 2, Problem 133GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Empirical and molecular formulas.(a) Fluorocarbonyl hypofluorite is composed of 14.6% C, 30.0% O, and 46.3% F. The molar mass of the compound is 82 g/mol. Determine the empirical and molecular formulas of the compound,(b) Azulene, a beautiful blue hydrocarbon, is 93.71% C and has a molar mass of 128.16 g/mol. What are the empirical and molecular formulas of azulene?

(a)

Interpretation Introduction

Interpretation: The empirical and molecular formulas for the given fluorocarbonyl hypofluorite should be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Equation for finding Molecular formula from the empirical formula,

MolarmassEmpiricalformula mass × Empirical formula

• Equation for number moles from mass and molar mass,

Numberofmoles=MassingramsMolarmass

• Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Given: Mass percent of carbon, oxygen and Florine in the given compound fluorocarbonyl hypofluorite are 14.6â€‰â€‰%â€‰,â€‰39.0â€‰%â€‰â€‰andâ€‰â€‰46.3â€‰% respectively.

Mass percent of an element means, 100g of compound contains that mass percent of an element in grams. Therefore, mass ofÂ  14.6â€‰gâ€‰ carbon â€‰39.0â€‰g of oxygen and 46.3Â g of F are present respectively in 100g of fluorocarbonyl hypofluorite.

Equation for number moles from mass and molar mass is,

â€‚Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰Massâ€‰inâ€‰gramsâ€‰Molarâ€‰mass

Therefore, the number of moles of C is,

Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰14.6â€‰g12.01g/molâ€‰=â€‰1.215â€‰mol

The number of moles of oxygen is,

Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰39â€‰â€‰g16â€‰g/molâ€‰=â€‰2.437â€‰mol

The number of moles of F is,

Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰46.3â€‰â€‰g19â€‰g/molâ€‰=â€‰2.437â€‰mol

So, the mole ratio between elements in fluorocarbonyl hypofluorite is,

Â Â Â Â C:F:Oâ€‰â€‰=â€‰â€‰1

(b)

Interpretation Introduction

Interpretation: The empirical and molecular formulas for the given azulene should be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Equation for finding Molecular formula from the empirical formula,

MolarmassEmpiricalformula mass × Empirical formula

• Equation for number moles from mass and molar mass,

Numberofmoles=MassingramsMolarmass

• Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started