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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

Oxygen atoms can combine with ozone to form oxygen:

O3(g) + O(g) → 2 O2(g)

Δ r H = −392 kJ/mol-rxn

Using Δ r H and the bond dissociation enthalpy data in Table 8.8, estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, O3. How does your estimate compare with the energies of an O—O single bond and an O=O double bond? Does the oxygen-oxygen bond dissociation enthalpy in ozone correlate with its bond order?

Interpretation Introduction

Interpretation:

The bond dissociation enthalpy for the Oxygen–Oxygen bond in Ozone should be determined and should be compared with the energies of O-O and O=O.  Finally, the bond dissociation enthalpy of ozone should be correlated with the bond order.

Concept Introduction:

Bond dissociation enthalpy: Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

The process of breaking bonds in a molecule is always endothermic, so ΔrH for bond breaking is always positive.

Explanation

O3(g)+O(g)2O2(g)

Given that,ΔrH0 = -392kJ/mol-rxn

  ΔrH0 = ΔH(bonds broken)-ΔH(bonds formed)

Analyzing the given reaction shows that for formation of the molecule (2O=O), the dissociation of one O-O bond happens together with formation of O=O.

The average bond dissociation enthalpy for 1 mol of O=O is 498kJ/mol

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