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 heat of formation data from Appendix E to calculate ∆H ° for the following reaction:ClO2 (g) + O(g) → ClO(g) + O2(g)
Hydrazine, N2H4, burns in oxygen as follows:
N2H4 + O2 → N2 + 2H2O
[The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496]
Draw the chemical structures of the reactants and products and
give the formula to calculate enthalpy change in a reaction, ΔH.
Based on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)
Chapter 10 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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