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Chapter 18: Problem 23

(a) What is the difference between chlorofluorocarbons and hydrofluorocarbons? (b) Why are hydrofluorocarbons potentially less harmful to the ozone layer than CFCs?

Short Answer

Expert verified
The main difference between chlorofluorocarbons (CFCs) and hydrofluorocarbons (HFCs) is the presence of chlorine in CFCs and hydrogen in HFCs. CFCs can break down in the stratosphere, releasing chlorine atoms, which catalyze reactions that deplete the ozone layer. In contrast, HFCs do not contain chlorine and do not contribute to ozone depletion. However, they are potent greenhouse gases and contribute to global warming.

Step by step solution

01

Defining Chlorofluorocarbons (CFCs) and Hydrofluorocarbons (HFCs)

Chlorofluorocarbons (CFCs) are types of compounds that are made up of carbon, chlorine, and fluorine atoms. Hydrofluorocarbons (HFCs), on the other hand, are composed of hydrogen, fluorine, and carbon atoms.
02

Differentiating between Chlorofluorocarbons (CFCs) and Hydrofluorocarbons (HFCs)

The fundamental difference between these two groups of compounds is the presence of chlorine in CFCs and hydrogen in HFCs. This variation in their composition results in different chemical properties and environmental impacts.
03

Understanding the Environmental Impact of Chlorofluorocarbons (CFCs)

CFCs are very stable in the lower atmosphere and thus do not break down easily. However, when they rise to the stratosphere (upper atmosphere), they can be broken down by solar radiation, releasing chlorine atoms. These chlorine atoms are capable of catalyzing reactions that deplete the ozone layer, a region of the atmosphere that blocks the majority of the sun's harmful ultraviolet radiation.
04

Understanding the Environmental Impact of Hydrofluorocarbons (HFCs)

Unlike CFCs, HFCs do not contain chlorine and thus do not contribute to ozone depletion when they break down in the stratosphere. Therefore, they are considered less harmful to the ozone layer. However, it's important to note that despite the fact that HFCs do not harm the ozone layer, they are potent greenhouse gases that can contribute significantly to global warming. As a result, their use is also being phased down internationally.

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Most popular questions from this chapter

A reaction for converting ketones to lactones, called the Baeyer-Villiger reaction, is used in the manufacture of plastics and pharmaceuticals. 3 Chloroperbenzoic acid is shock-sensitive, however, and prone to explode. Also, 3 -chlorobenzoic acid is a waste product. An alternative process being developed uses hydrogen peroxide and a catalyst consisting of tin deposited within a solid support. The catalyst is readily recovered from the reaction mixture. (a) What would you expect to be the other product of oxidation of the ketone to lactone by hydrogen peroxide? (b) What principles of green chemistry are addressed by use of the proposed process?

One mystery in environmental science is the imbalance in the "carbon dioxide budget." Considering only human activities, scientists have estimated that 1.6 billion metric tons of \(\mathrm{CO}_{2}\) is added to the atmosphere every year because of deforestation (plants use \(\mathrm{CO}_{2},\) and fewer plants will leave more \(\mathrm{CO}_{2}\) in the atmosphere). Another 5.5 billion tons per year is put into the atmosphere because of burning fossil fuels. It is further estimated (again, considering only human activities) that the atmosphere actually takes up about 3.3 billion tons of this \(\mathrm{CO}_{2}\) per year, while the oceans take up 2 billion tons per year, leaving about 1.8 billion tons of \(\mathrm{CO}_{2}\) per year unaccounted for. This "missing" \(\mathrm{CO}_{2}\) is assumed to be taken up by the "land." What do you think might be happening? [Sections \(18.1-18.3]\)

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The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. (a) Using the density, specific heat, and heat of vaporization of water from Appendix \(\mathrm{B}\), calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at \(20^{\circ} \mathrm{C}\). (b) If the energy is provided by electricity costing \(\$ 0.085 / \mathrm{kWh},\) calculate its cost. (c) If distilled water sells in a grocery store for \(\$ 1.26\) per gal, what percentage of the sales price is represented by the cost of the energy?

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