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Chapter 18: Problem 74

Write balanced chemical equations for each of the following reactions: (a) The nitric oxide molecule undergoes photodissociation in the upper atmosphere. (b) The nitric oxide molecule undergoes photoionization in the upper atmosphere. (c) Nitric oxide undergoes oxidation by ozone in the stratosphere. (d) Nitrogen dioxide dissolves in water to form nitric acid and nitric oxide.

Short Answer

Expert verified
(a) \( NO \xrightarrow{h\nu} N + O \) (b) \( NO + h\nu \rightarrow NO^+ + e^- \) (c) \( NO + O_3 \rightarrow NO_2 + O_2 \) (d) \( 3NO_2 + H_2O \rightarrow 2HNO_3 + NO \)

Step by step solution

01

(a) Photodissociation of nitric oxide in the upper atmosphere

In this reaction, nitric oxide (NO) undergoes photodissociation. Photodissociation is the process by which a molecule absorbs a photon of light and breaks apart into smaller fragments. For NO, it will dissociate into nitrogen (N) and oxygen (O) atoms. The balanced chemical equation for this reaction is: \[ NO \xrightarrow{h\nu} N + O \]
02

(b) Photoionization of nitric oxide in the upper atmosphere

In this reaction, nitric oxide (NO) undergoes photoionization. Photoionization is the process by which a molecule absorbs a photon of light and becomes ionized by losing an electron. For NO, it will form a positively charged nitric oxide ion (NO+) and an electron (e-). The balanced chemical equation for this reaction is: \[ NO + h\nu \rightarrow NO^+ + e^- \]
03

(c) Oxidation of nitric oxide by ozone in the stratosphere

In this reaction, nitric oxide (NO) undergoes oxidation by ozone (O3) in the stratosphere. This reaction produces nitrogen dioxide (NO2) and oxygen (O2) molecules as products. The balanced chemical equation for this reaction is: \[ NO + O_3 \rightarrow NO_2 + O_2 \]
04

(d) Dissolving nitrogen dioxide in water to form nitric acid and nitric oxide

In this reaction, nitrogen dioxide (NO2) dissolves in water (H2O) to form nitric acid (HNO3) and nitric oxide (NO). The balanced chemical equation for this reaction is: \[ 3NO_2 + H_2O \rightarrow 2HNO_3 + NO \] These are the balanced chemical equations for the given reactions involving nitric oxide and related molecules.

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Most popular questions from this chapter

The solar power striking Earth every day averages 168 watts per square meter. The highest ever recorded electrical power usage in New York City was \(13,200 \mathrm{MW} .\) A record established in July of \(2013 .\) Considering that present technology for solar energy conversion is about 10\(\%\) efficient, from how many square meters of land must sunlight be collected in order to provide this peak power? (For comparison, the total area of New York City is 830 km.)

An important reaction in the formation of photochemical smog is the photodissociation of \(\mathrm{NO}_{2} :\) $$\mathrm{NO}_{2}+h \nu \longrightarrow \mathrm{NO}(g)+\mathrm{O}(g)$$ The maximum wavelength of light that can cause this reaction is 420 \(\mathrm{nm}\) . (a) In what part of the electromagnetic spectrum is light with this wavelength found? (b) What is the maximum strength of a bond, in kJ/mol, that can be broken by absorption of a photon of \(420-\mathrm{nm}\) light? (c) Write out the photodissociation reaction showing Lewis-dot structures.

The degradation of \(\mathrm{CF}_{3} \mathrm{CH}_{2} \mathrm{F}(\) an \(\mathrm{HFC})\) by \(\mathrm{OH}\) radicals in the troposphere is first order in each reactant and has a rate constant of \(k=1.6 \times 10^{8} M^{-1} \mathrm{s}^{-1}\) at \(4^{\circ} \mathrm{C} .\) If the tropospheric concentrations of \(\mathrm{OH}\) and \(\mathrm{CF}_{3} \mathrm{CH}_{2} \mathrm{F}\) are \(8.1 \times 10^{5}\)and \(6.3 \times 10^{8}\) molecules/cm\(^{3},\) respectively, what is the rate of reaction at this temperature in \(M / \mathrm{s} ?\)

Magnesium ions are removed in water treatment by the addition of slaked lime, \(\mathrm{Ca}(\mathrm{OH})_{2}\). Write a balanced chemical equation to describe what occurs in this process.

The organic anion is found in most detergents. Assume that the anion undergoes aerobic decomposition in the following manner: $$\begin{aligned} 2 \mathrm{C}_{18} \mathrm{H}_{29} \mathrm{SO}_{3}^{-}(a q)+51 \mathrm{O}_{2}(a q) & \longrightarrow \\ & 36 \mathrm{CO}_{2}(a q)+28 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{H}^{+}(a q)+2 \mathrm{SO}_{4}^{2-}(a q) \end{aligned}$$ What is the total mass of \(\mathrm{O}_{2}\) required to biodegrade 10.0 \(\mathrm{g}\) of this substance?
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