Chapter 10, Problem 100E

### Chemistry

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

Chapter
Section

### Chemistry

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

# The molar heat of fusion of benzene (C6H6) is 9.92 kJ/mol. Its molar heat of vaporization is 30.7 kJ/mol. Calculate the heat required to melt 8.25 g benzene at its normal melting point. Calculate the heat required to vaporize 8.25 g benzene at its normal boiling point. Why is the heat of vaporization more than three times the heat of fusion?

Interpretation Introduction

Interpretation: The heat of vaporization and heat required to melt 8.25 g benzene should be calculated.

Concept Introduction:

Heat of vaporization:

The energy required for a quantity of liquid substance converted in to into a gases substance is called heat of vaporization.

Explanation

Explanation

Record the given data:

Molar heat of fusion of benzene = 9.92 kJ/mol.

Molar heat of vaporization = 30.7 kJ/mol.

The given molar heat of fusion and molar heat of vaporization of benzene are recorded as shown above.

To calculate the heat required to melt 8.25 g benzene at its normal melting point.

Molecular weight of benzene is 78.11g .

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â  =â€‰8.25â€‰gâ€‰benzeneÃ—1molâ€‰benzene78.11â€‰gÃ—9.92â€‰kJ1â€‰moleâ€‰benzene=â€‰1.05â€‰kJ

• The given heat of fusion of benzene and molecular weight of benzene are plugging in the equation to give heat required to melt 8.25 g benzene.
• The required heat for melt 8.25 g benzene is 1.05â€‰kJ

### 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