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Chapter 18: Problem 18

Why is the photodissociation of \(\mathrm{N}_{2}\) in the atmosphere relatively unimportant compared with the photodissociation of \(\mathrm{O}_{2} ?\)

Short Answer

Expert verified
The photodissociation of \(\mathrm{N}_{2}\) is relatively unimportant compared to \(\mathrm{O}_{2}\) because \(\mathrm{N}_{2}\) has a stronger bond and weaker absorption spectrum than \(\mathrm{O}_{2}\). Additionally, the photodissociation of \(\mathrm{O}_{2}\) has significant atmospheric implications, such as the formation of the ozone layer, while the photodissociation of \(\mathrm{N}_{2}\) does not have such effects.

Step by step solution

01

Understanding the molecules

\(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) are both diatomic molecules, with nitrogen and oxygen being the two most abundant elements in Earth's atmosphere. Nitrogen makes up about 78% of the atmosphere, while oxygen makes up about 21%.
02

Analyzing Bond Strength

One factor that affects the photodissociation of molecules is their bond strength. \(\mathrm{N}_{2}\) has a triple bond, which is stronger than the double bond found in \(\mathrm{O}_{2}\). The bond dissociation energy of \(\mathrm{N}_{2}\) is about 941 kJ/mol, while that of \(\mathrm{O}_{2}\) is about 498 kJ/mol. This means that it requires more energy to break the bond in \(\mathrm{N}_{2}\) than in \(\mathrm{O}_{2}\).
03

Comparing Absorption Spectra

Both \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) absorb ultraviolet (UV) radiation, causing them to photodissociate. However, their absorption spectra are different. \(\mathrm{O}_{2}\) strongly absorbs wavelengths below 240 nm, while \(\mathrm{N}_{2}\) has a much weaker absorption in this region. This means that \(\mathrm{O}_{2}\) will absorb more UV radiation and undergo photodissociation more readily than \(\mathrm{N}_{2}\).
04

Atmospheric Implications

The photodissociation of \(\mathrm{O}_{2}\) in the atmosphere is important because it leads to the formation of ozone (O3). The ozone layer in Earth's stratosphere protects life on the surface from harmful ultraviolet radiation. In contrast, the photodissociation of \(\mathrm{N}_{2}\) has less significant atmospheric implications, as it does not contribute to the formation of any protective layer or participate in major life-sustaining processes like photosynthesis or respiration.
05

Conclusion

The photodissociation of \(\mathrm{N}_{2}\) is relatively unimportant compared with the photodissociation of \(\mathrm{O}_{2}\) for a few reasons: 1. The bond strength in \(\mathrm{N}_{2}\) is stronger than in \(\mathrm{O}_{2}\), making it more difficult to break apart. 2. The absorption spectrum of \(\mathrm{N}_{2}\) is weaker than that of \(\mathrm{O}_{2}\) in the relevant wavelength region, meaning it absorbs less ultraviolet radiation. 3. The photodissociation of \(\mathrm{O}_{2}\) has significant implications for Earth's atmosphere, such as the formation of the ozone layer, while the photodissociation of \(\mathrm{N}_{2}\) does not have such effects.

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Most popular questions from this chapter

Natural gas consists primarily of methane, \(\mathrm{CH}_{4}(\mathrm{~g})\). (a) Write a balanced chemical equation for the complete combustion of methane to produce \(\mathrm{CO}_{2}(g)\) as the only carbon-containing product. (b) Write a balanced chemical equation for the incomplete combustion of methane to produce \(\mathrm{CO}(g)\) as the only carbon-containing product. (c) At \(25^{\circ} \mathrm{C}\) and \(1.0\) atm pressure, what is the minimum quantity of dry air needed to combust \(1.0 \mathrm{~L}\) of \(\mathrm{CH}_{4}(\mathrm{~g})\) completely to \(\mathrm{CO}_{2}(\mathrm{~g})\) ?

The water supply for a midwestern city contains the following impurities: coarse sand, finely divided particulates, nitrate ion, trihalomethanes, dissolved phosphorus in the form of phosphates, potentially harmful bacterial strains, dissolved organic substances. Which of the following processes or agents, if any, is effective in removing each of these impurities: coarse sand filtration, activated carbon filtration, aeration, ozonization, precipitation with aluminum hydroxide?

The estimated average concentration of \(\mathrm{NO}_{2}\) in air in the United States in 2006 was \(0.016\) ppm. (a) Calculate the partial pressure of the \(\mathrm{NO}_{2}\) in a sample of this air when the atmospheric pressure is 755 torr \((99.1 \mathrm{kPa}) .\) (b) How many molecules of \(\mathrm{NO}_{2}\) are present under these conditions at \(20^{\circ} \mathrm{C}\) in a room that measures \(15 \times 14 \times 8 \mathrm{ft}\) ?

A reaction that contributes to the depletion of ozone in the stratosphere is the direct reaction of oxygen atoms with ozone: $$\mathrm{O}(\mathrm{g})+\mathrm{O}_{3}(g) \longrightarrow 2 \mathrm{O}_{2}(g)$$ At \(298 \mathrm{~K}\) the rate constant for this reaction is \(4.8 \times 10^{5} \mathrm{M}^{-1} \mathrm{~s}^{-1}\). (a) Based on the units of the rate constant, write the likely rate law for this reaction. (b) Would you expect this reaction to occur via a single elementary process? Explain why or why not. (c) From the magnitude of the rate constant, would you expect the activation energy of this reaction to be large or small? Explain. (d) Use \(\Delta H_{f}^{\circ}\) values from Appendix \(C\) to estimate the enthalpy change for this reaction. Would this reaction raise or lower the temperature of the stratosphere?

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