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Chapter 18: Problem 24

Which of the following reactions in the stratosphere cause an increase in temperature there? (a) \(\mathrm{O}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{3}^{*}(g)\) (b) $\mathrm{O}_{3}^{*}(g)+\mathrm{M}(g) \longrightarrow \mathrm{O}_{3}(g)+\mathrm{M}^{*}(g)$ (c) \(\mathrm{O}_{2}(g)+h \nu \longrightarrow 2 \mathrm{O}(g)\) (d) $\mathrm{O}(g)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{N}(g)$ (e) All of the above

Short Answer

Expert verified
The reactions (a) and (d) are exothermic and cause an increase in temperature in the stratosphere.

Step by step solution

01

Analyze Reaction (a)

Analyze the reaction: \(\mathrm{O}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{3}^{*}(g)\). It consists of oxygen atoms combining to form ozone (\(\mathrm{O}_3\)). The ozone is in an excited state denoted by the asterisk. As it is a combination reaction, it is usually exothermic, meaning it releases energy.
02

Analyze Reaction (b)

Analyze the reaction: \(\mathrm{O}_{3}^{*}(g)+\mathrm{M}(g) \longrightarrow \mathrm{O}_{3}(g)+\mathrm{M}^{*}(g)\). In this reaction, the excited ozone transfers its energy to another molecule M (termed the collision partner). The result is the ground state ozone and an excited-state molecule M. This reaction is energy-transfer, and does not affect the overall temperature.
03

Analyze Reaction (c)

Analyze the reaction: \(\mathrm{O}_{2}(g)+h \nu \longrightarrow 2 \mathrm{O}(g)\). In this photodissociation reaction, a photon (hν) supplies the energy required to dissociate diatomic oxygen (\(\mathrm{O}_2\)) into two single oxygen atoms. It is an endothermic reaction as it absorbs energy.
04

Analyze Reaction (d)

Analyze the reaction: \(\mathrm{O}(g)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{N}(g)\). This reaction involves the formation of a nitrogen monoxide molecule from the combination of a single oxygen atom and a nitrogen molecule, followed by a dissociation into nitrogen monoxide and an atomic nitrogen. The change in energy cannot be deduced directly without the help of thermodynamic data, but it is known that it is exothermic reaction.
05

Answer the question

From our analysis, reactions (a) and (d) are exothermic and cause an increase in temperature in the stratosphere. Therefore, the correct answer is (a) and (d).

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Most popular questions from this chapter

Hydrogen phosphate \(\left(\mathrm{HPO}_{4}^{2-}\right)\) can be removed in water treatment by the addition of slaked lime, $\mathrm{Ca}(\mathrm{OH})_{2} .$ Write a balanced chemical equation for the reaction (using ions as reactant), in which \(\mathrm{Ca}_{5}(\mathrm{OH})\left(\mathrm{PO}_{4}\right)_{3}\) forms as a precipitate.

Write balanced chemical equations for each of the following reactions: (a) The carbon dioxide molecule undergoes photodissociation in the upper atmosphere. (b) The carbon dioxide molecule undergoes photoionization in the upper atmosphere. (c) Carbon monoxide undergoes oxidation by ozone in the stratosphere. (d) Carbon dioxide dissolves in water to form hydrogen carbonate.

The estimated average concentration of \(\mathrm{NO}_{2}\) in air in the United States in 2015 was 0.010 ppm. (a) Calculate the partial pressure of the \(\mathrm{NO}_{2}\) in a sample of this air when the atmospheric pressure is \(101 \mathrm{kPa} .(\mathbf{b})\) How many molecules of \(\mathrm{NO}_{2}\) are present under these conditions at \(25^{\circ} \mathrm{C}\) in a room that measures \(10 \mathrm{~m} \times 8 \mathrm{~m} \times 2.50 \mathrm{~m} ?\)

A first-stage recovery of magnesium from seawater is precipitation of \(\mathrm{Mg}(\mathrm{OH})_{2}\) with \(\mathrm{CaO};\) $$ \mathrm{Mg}^{2+}(a q)+\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)+\mathrm{Ca}^{2+}(a q) $$ What mass of \(\mathrm{CaO}\), in grams, is needed to precipitate $1000 \mathrm{~kg}\( of \)\mathrm{Mg}(\mathrm{OH})_{2} ?$

One of the principles of green chemistry is that it is better to use as few steps as possible in making new chemicals. In what ways does following this rule advance the goals of green chemistry? How does this principle relate to energy efficiency?
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