   Chapter 21, Problem 101GQ

Chapter
Section
Textbook Problem

The standard enthalpy of formation of OF2 gas is + 24.5 kJ/mol. Calculate the average O—F bond enthalpy.

Interpretation Introduction

Interpretation:

To calculate the average OF bond enthalpy in OF2 molecule.

Concept introduction:

The bond dissociation energy is the energy required to break one mole of the gas (in a gaseous state) to give the separate atoms in a gaseous state. The bond dissociation energy is the energy of a single bond while bond energy is the average of the all bond dissociation energies. For the diatomic molecule bond dissociation energy is equal to the bond energy of the molecule.

The change of enthalpy to form one mole of a substance from its constituent elements when all the substances in the standard form is known as standard enthalpy of formation.

The standard enthalpy of formation (ΔfH) in terms of standard bond dissociation enthalpy (B) is written as,

ΔfH=BproductsBreactants (1)

Explanation

The average OF bond enthalpy in OF2 molecule is calculated below.

Given:

Refer to the

The bond dissociation of O2 molecule is written as,

O2(g)2O(g)

The standard bond dissociation enthalpy (BOO) of O2 molecule is 498kJmol1.

The bond dissociation of F2 molecule is written as,

F2(g)2F(g)

The standard bond dissociation enthalpy (BFF) of F2 molecule is 155kJmol1.

The reaction of formation of OF2 molecule from its constituent elements is written as follows,

F2(g)+12O2(g)OF2(g)

The standard enthalpy of formation (ΔfHOF2) of OF2 is 24.5kJmol1

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

Find more solutions based on key concepts 