/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 53 If an average \(\mathrm{O}_{3}\)... [FREE SOLUTION] | 91影视

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Chapter 18: Problem 53

If an average \(\mathrm{O}_{3}\) molecule "lives" only \(100-200\) seconds in the stratosphere before undergoing dissociation, how can \(\mathrm{O}_{3}\) offer any protection from ultraviolet radiation?

Short Answer

Expert verified
Although individual ozone (O3) molecules have a short lifespan of 100-200 seconds, they continuously form and dissociate in the stratosphere, creating a protective ozone layer. Ozone molecules form when UV radiation breaks apart oxygen molecules (O2) into free oxygen atoms, which then collide with other O2 molecules to form O3. Ozone molecules dissociate when they absorb UV radiation, breaking down into O2 molecules and free oxygen atoms. This ongoing cycle of formation and dissociation maintains the ozone layer, enabling it to absorb harmful ultraviolet radiation and protect life on Earth.

Step by step solution

01

Understanding the ozone molecule#writer_sdk# An ozone molecule, also known as O3, consists of three oxygen atoms bonded together. Ozone molecules exist primarily in the Earth's stratosphere, which is located approximately 10-50 km above the Earth's surface. The ozone layer plays a vital role in protecting the Earth from harmful UV radiation, which can cause skin cancer, cataracts, and damage to the immune system as well as to marine and plant life.

Step 2: Formation of ozone molecules#writer_sdk# Ozone molecules are formed in the stratosphere when ultraviolet (UV) radiation breaks apart regular oxygen molecules (O2) into free oxygen atoms. When UV radiation with a wavelength shorter than 240 nm hits an O2 molecule, the radiation energy is strong enough to break the oxygen bond and produce two free oxygen atoms. These free oxygen atoms can then collide with other O2 molecules to form O3: \[ O_2 + UV_{<240 nm} \to 2O \] \[ O + O_2 \to O_3 \]
02

Dissociation of ozone molecules#writer_sdk# Ozone molecules are not very stable and can quickly dissociate (break apart) when they absorb ultraviolet radiation. When ozone molecules absorb UV radiation with a wavelength between 240 nm and 310 nm, they break apart into O2 molecules and free oxygen atoms. This dissociation process can be represented as follows: \[ O_3 + UV_{240-310 nm} \to O_2 + O \] The free oxygen atoms produced in dissociation can then react with more O2 molecules to form new ozone molecules, as described in Step 2.

Step 4: Explaining the protective role of ozone#writer_sdk# Although individual ozone molecules only "live" for 100-200 seconds before dissociating, the continuous cycle of ozone formation and dissociation helps to maintain an overall ozone presence in the stratosphere. By absorbing ultraviolet radiation (particularly the hazardous UV-C radiation), ozone molecules prevent that energy from reaching Earth's surface, effectively protecting life on Earth. Overall, despite the short lifespan of ozone molecules, the cycling processes of formation and dissociation maintain the ozone layer and enable it to offer continuous protection against harmful ultraviolet radiation.

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Most popular questions from this chapter

The organic anion is found in most detergents. Assume that the anion undergoes aerobic decomposition in the following manner: $$ \begin{array}{r} 2 \mathrm{C}_{18} \mathrm{H}_{29} \mathrm{SO}_{3}^{-}(a q)+51 \mathrm{O}_{2}(a q) \longrightarrow \\ 36 \mathrm{CO}_{2}(a q)+28 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{H}^{+}(a q)+2 \mathrm{SO}_{4}{ }^{2-}(a q) \end{array} $$ What is the total mass of \(\mathrm{O}_{2}\) required to biodegrade \(1.0 \mathrm{~g}\) of this substance?

Explain why increasing concentrations of \(\mathrm{CO}_{2}\) in the atmosphere affect the quantity of energy leaving Earth but do not affect the quantity entering from the Sun.

Air pollution in the Mexico City metropolitan area is among the worst in the world. The concentration of ozone in Mexico City has been measured at 441 ppb (0.441 ppm). Mexico City sits at an altitude of 7400 feet, which means its atmospheric pressure is only \(0.67\) atm. Calculate the partial pressure of ozone at 441 ppb if the atmospheric pressure is \(0.67\) atm.

(a) Why is the fluorine present in chlorofluorocarbons not a major contributor to depletion of the ozone layer? (b) What are the chemical forms in which chlorine exists in the stratosphere following cleavage of the carbonchlorine bond?

Molecules in the upper atmosphere tend to contain double and triple bonds rather than single bonds. Suggest an explanation. [Section 18.2]
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