One reaction involved in the sequence of reactions leading to the destruction of ozone is NO 2 ( g ) +O ( g ) → NO ( g ) +O 2 ( g ) Calculate Δ r H ° for this reaction by using the thermodynamic data in Appendix D. Use your Δ r H ° value, plus data from Table 10.3, to estimate the nitrogen-oxygen bond energy in N O 2 . (Hint: The structure of nitrogen dioxide, N O 2 , is best represented as a resonance hybrid of two equivalent Lewis structures.)
One reaction involved in the sequence of reactions leading to the destruction of ozone is NO 2 ( g ) +O ( g ) → NO ( g ) +O 2 ( g ) Calculate Δ r H ° for this reaction by using the thermodynamic data in Appendix D. Use your Δ r H ° value, plus data from Table 10.3, to estimate the nitrogen-oxygen bond energy in N O 2 . (Hint: The structure of nitrogen dioxide, N O 2 , is best represented as a resonance hybrid of two equivalent Lewis structures.)
Solution Summary: The author explains how the nitrogen-oxygen bond energy should be estimated based on Hess's law.
One reaction involved in the sequence of reactions leading to the destruction of ozone is
NO
2
(
g
)
+O
(
g
)
→
NO
(
g
)
+O
2
(
g
)
Calculate
Δ
r
H
°
for this reaction by using the thermodynamic data in Appendix D. Use your
Δ
r
H
°
value, plus data from Table 10.3, to estimate the nitrogen-oxygen bond energy in
N
O
2
. (Hint: The structure of nitrogen dioxide,
N
O
2
, is best represented as a resonance hybrid of two equivalent Lewis structures.)
Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.
Use average bond energies together with the standard enthalpy of formation of C( g) (718.4 kJ/mol) to estimate the standard enthalpy of formation of gaseous benzene, C6H6( g). (Remember that average bond energies apply to the gas phase only.) Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene,82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?
A scientist studies the bond energies of different compounds containing nitrogen (N). The scientist observes that the N–N bonds in one group of compounds have a bond energy of 209 kJ/mol, while the N–N bonds in another group of compounds have a bond energy of 418 kJ/mol. In one or two sentences, postulate a reason for this difference.
For the O2+ ion predict (a) number of unpaired electrons, (b) bond order, (c) bond enthalpy and bond length.
Chapter 10 Solutions
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
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The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY