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Chapter 1: Problem 37

The EPA characterizes ozone as "good up high, bad nearby." Explain.

Short Answer

Expert verified
Ozone is beneficial in the stratosphere as it protects from UV radiation but harmful at ground level as a pollutant.

Step by step solution

01

Understanding Ozone

Ozone is a molecule composed of three oxygen atoms, denoted as O鈧�. Depending on where ozone is located in the Earth's atmosphere, it can be either beneficial or harmful.
02

The Role of Ozone in the Stratosphere

In the stratosphere, which is a layer of the atmosphere located about 10 to 30 miles above the Earth鈥檚 surface, ozone plays a crucial role in protecting life on Earth. The ozone layer absorbs most of the sun's harmful ultraviolet (UV) radiation, preventing it from reaching the surface, which reduces the risk of skin cancer and other health issues.
03

The Impact of Ozone at Ground Level

At ground level, or in the troposphere, ozone is created by chemical reactions between oxides of nitrogen (NOx) and volatile organic compounds (VOC) in the presence of sunlight. This ground-level ozone is a key component of smog and can be harmful to human health, causing or exacerbating respiratory problems, and it can damage crops and other vegetation.
04

Comparison of High vs. Low Ozone

While high-altitude ozone acts as a protective barrier, low-level ozone is a pollutant. The statement "good up high, bad nearby" encapsulates this duality: ozone is beneficial when it forms a layer in the stratosphere but is dangerous when it accumulates near the Earth's surface.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stratosphere
The stratosphere is a layer of the Earth's atmosphere that stretches from about 10 to 30 miles above the planet's surface.
It is home to the essential ozone layer. This layer serves as a protective shield by absorbing a significant amount of the sun's harmful ultraviolet (UV) radiation.
Without this shield, life on Earth would be exposed to excessive UV radiation, leading to increased rates of skin cancer, cataracts, and other health issues. The stratosphere is crucial for maintaining the balance of life by filtering out these harmful rays from the sun.
Troposphere
The troposphere is the lowest layer of the Earth's atmosphere, extending from the surface up to about 6 to 10 miles. All weather patterns and life activities occur here.
Tropospheric ozone is not emitted directly into the air but is formed by the reaction of sunlight on air containing hydrocarbons and nitrogen oxides emitted by cars, power plants, and other sources.
Unlike the protective ozone in the stratosphere, ozone in the troposphere acts as a pollutant at ground level. It contributes to the formation of smog and poses health risks such as breathing issues, especially for children, the elderly, and those with pre-existing respiratory conditions.
Ultraviolet Radiation
Ultraviolet (UV) radiation is a type of energy produced by the sun and some artificial sources, like tanning beds. UV radiation is categorized into three types based on wavelength: UVA, UVB, and UVC.
The stratospheric ozone primarily absorbs the more harmful UVB and UVC rays. Without this absorption, the Earth's surface would face more intense UV radiation, leading to severe health effects on living organisms, including increased skin cancer rates and biodiversity damage.
Understanding the types of UV radiation helps us appreciate the stratospheric ozone's role in protecting all life forms on Earth.
Smog
Smog is a type of air pollution resulting from a mixture of smoke, chemicals, and fog. It is particularly prominent in urban areas.
One of the major components of smog is ground-level ozone. This ozone is formed when sunlight triggers a chemical reaction between nitrogen oxides and volatile organic compounds in the air.
Smog not only affects air quality but also can severely impact human health, contributing to respiratory problems and heart disease.
  • Smog reduces visibility, causing hazards for drivers and aviation.
  • It also affects plant life by hindering photosynthesis.
  • Efforts to reduce smog involve controlling emissions of nitrogen oxides and volatile organic compounds.
By managing these emissions, we can work towards cleaner air and better overall health outcomes.

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Most popular questions from this chapter

Express each of these numbers in scientific notation. a. \(1500 \mathrm{~m}\), the distance of a foot race b. \(0.0000000000958 \mathrm{~m}\), the distance between \(\mathrm{O}\) and \(\mathrm{H}\) atoms in a water molecule c. \(0.0000075 \mathrm{~m}\), the diameter of a red blood cell d. \(150,000 \mathrm{mg}\) of \(\mathrm{CO}\), the approximate amount breathed daily

Prior to 1990 , diesel fuel could contain as much as \(2 \%\) sulfur. New regulations have changed this, and today most diesel fuel is ultra-low sulfur diesel (ULSD) containing a maximum of \(15 \mathrm{ppm}\) sulfur. ULTRA-LOW SULFUR HIGHWAY DIESEL FUEL (15 ppm Sulfur Maximum) Required for use in all model year 2007 and later highway diesel vehicles and engines. Recommended for use in all diesel vehicles and engines. a. Express 15 ppm as a percent. Likewise, express \(2 \%\) in terms of ppm. How many times lower is the ULSD than the older formulation of diesel fuel? b. Write a chemical equation that shows how burning diesel fuel containing sulfur contributes to air pollution. c. Diesel fuel contains the hydrocarbon \(\mathrm{C}_{12} \mathrm{H}_{26}\). Write a chemical equation that shows how burning diesel adds carbon dioxide to the atmosphere. d. Comment on burning diesel fuel as a sustainable practice, both in terms of how things have improved and in terms of where they still need to go.

Look up the ozone air quality data for two states, one in the Sun Belt and one not. Account for any difference you find.

A headline from the Anchorage Daily News in Alaska (January 17, 2008): "Family in car overcome by carbon monoxide. Fire department saves five after slide into snow bank." a. If your car is in a snow bank and the engine is running, CO may accumulate inside the car. Normally, however, CO does not accumulate in the car. Explain. b. Why didn't the occupants detect the \(\mathrm{CO}\) ?

Nail polish remover containing acetone was spilled in a room \(6 \mathrm{~m} \times 5 \mathrm{~m} \times 3 \mathrm{~m}\). Measurements indicated that \(3600 \mathrm{mg}\) of acetone evaporated. Calculate the acetone concentration in micrograms per cubic meter.
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