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Chapter 10: Problem 99

One reaction involved in the sequence of reactions leading to the destruction of ozone is $$\mathrm{NO}_{2}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$$ Calculate \(\Delta H^{\circ}\) for this reaction by using the thermodynamic data in Appendix D. Use your \(\Delta H^{\circ}\) value, plus data from Table \(10.3,\) to estimate the nitrogenoxygen bond energy in \(\mathrm{NO}_{2}\). [Hint: The structure of nitrogen dioxide, \(\mathrm{NO}_{2}\), is best represented as a resonance hybrid of two equivalent Lewis structures.]

Short Answer

Expert verified
After calculating the enthalpy change (\(\Delta H^{\circ}\)) and estimating the nitrogen-oxygen bond energy, the values to these should be presented here. Remember to include units for full credit.

Step by step solution

01

Calculation of the Enthalpy Change (\(\Delta H^{\circ}\))

Using the thermodynamic data from Appendix D, find the values for the enthalpy of formation for each of the reactants and products. The formula used to calculate \(\Delta H^{\circ}\) is \(\Delta H^{\circ} = \sum H^{\circ}_{\text{products}} - \sum H^{\circ}_{\text{reactants}}\). Substitute the respective values into the equation and solve for \(\Delta H^{\circ}\).
02

Estimation of Nitrogen-Oxygen Bond Energy in \(\mathrm{NO}_{2}\)

The nitrogen-oxygen bond energy in \(\mathrm{NO}_{2}\) can be estimated by first determining the total energy of the bonds in the products and the reactants using data from Table 10.3. Subtract the total bond energy of the reactants from that of the products. This estimated value will be the nitrogen-oxygen bond energy in \(\mathrm{NO}_{2}\). The calculation takes into account that \(\mathrm{NO}_{2}\) is best represented as a resonance hybrid of two equivalent Lewis structures.

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Most popular questions from this chapter

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) \(\mathrm{Al}(\mathrm{OH})_{3}\); (c) \(\mathrm{NH}_{4} \mathrm{F}\); (d) \(\mathrm{KClO}_{3}\); (b) \(\mathrm{Ca}(\mathrm{CN})_{2}\); (e) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\).

The formal charges on the \(\mathrm{O}\) atoms in the ion \([\mathrm{ONO}]^{+}\) is \((\mathrm{a})-2 ;(\mathrm{b})-1 ;(\mathrm{c}) 0 ;(\mathrm{d})+1\).

A compound consists of \(47.5 \%\) S and \(52.5 \%\) Cl, by mass. Write a Lewis structure based on the empirical formula of this compound, and comment on its deficiencies. Write a more plausible structure with the same ratio of \(\mathrm{S}\) to \(\mathrm{Cl}\).

In certain polar solvents, \(\mathrm{PCl}_{5}\) undergoes an ionization reaction in which a \(\mathrm{Cl}^{-}\) ion leaves one \(\mathrm{PCl}_{5}\) molecule and attaches itself to another. The products of the ionization are \(\mathrm{PCl}_{4}^{+}\) and \(\mathrm{PCl}_{6}^{-}\). Draw a sketch showing the changes in geometric shapes that occur in this ionization (that is, give the shapes of \(\mathrm{PCl}_{5}\), \(\mathrm{PCl}_{4}^{+},\) and \(\mathrm{PCl}_{6}^{-}\) ). $$2 \mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{4}^{+}+\mathrm{PCl}_{6}^{-}$$

What is the formal charge of the indicated atom in each of the following structures? (a) the central \(\mathrm{O}\) atom in \(\mathrm{O}_{3}\) (b) \(\mathrm{Al}\) in \(\mathrm{AlH}_{4}^{-}\) (c) \(\mathrm{Cl}\) in \(\mathrm{ClO}_{3}^{-}\) (d) \(\sin \sin ^{2} \theta^{-}\) (e) \(\mathrm{Cl}\) in \(\mathrm{Cl} \mathrm{F}_{3}\)
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