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. Describe a mechanism by which \(\mathrm{CO}_{2}\) is removed from the atmosphere and ultimately ends up below the surface (Hint: What is the source of the fossil fuels?) [Sections \(18.1-18.3 ]\)

Short Answer

Expert verified
The unaccounted-for 1.8 billion metric tons of CO₂ per year may be sequestered through a mechanism involving photosynthesis and the carbon cycle. Plants and other photosynthetic organisms remove CO₂ from the atmosphere and convert it into organic compounds. As these plants die and are buried under sediment, they become part of the fossil fuel formation process over millions of years, ultimately ending up below the Earth's surface as coal, oil, or natural gas. This process helps store carbon beneath the Earth's surface; however, burning fossil fuels releases this stored carbon back into the atmosphere, contributing to the global carbon budget imbalance.

Step by step solution

01

Understand the given data

The data provided in the exercise states that human activities add: - 1.6 billion metric tons of CO2 is added to the atmosphere yearly because of deforestation - 5.5 billion metric tons of CO2 due to burning fossil fuels Additionally, the atmosphere takes up 3.3 billion metric tons of CO₂ per year, the ocean takes up about 2 billion metric tons per year, leaving 1.8 billion metric tons of CO₂ per year unaccounted for.
02

Identify the source of fossil fuels

Fossil fuels, such as coal, oil, and natural gas, are formed from the remains of ancient plants and animals that have been subjected to heat and pressure over millions of years. They are primarily composed of carbon and hydrogen, and when burned as a fuel, they release CO2 into the atmosphere.
03

Understand the carbon cycle

The carbon cycle is a natural process through which carbon atoms circulate between the Earth's surface, atmosphere, and oceans. It includes key processes such as photosynthesis, respiration, and decomposition, and plays a significant role in determining the levels of CO2 in the atmosphere.
04

Describe a mechanism by which CO2 is removed from the atmosphere

One mechanism by which CO2 is removed from the atmosphere is through photosynthesis. Plants take in CO₂ from the atmosphere and, using sunlight, convert it into glucose and oxygen. This glucose can then be used by the plants for growth and is transformed into more complex organic molecules, such as cellulose and lignin. As these plants die and are buried under layers of sediment, they can become part of the fossil fuel formation process over millions of years, ultimately ending up below the Earth's surface in the form of coal, oil, or natural gas.
05

Conclusion

The unaccounted-for CO₂ may be getting sequestered in various ways, one of which is being incorporated into the process of fossil fuel formation. Photosynthesis by plants and other photosynthetic organisms removes CO₂ from the atmosphere and converts it into organic compounds. These compounds, through a series of geological processes, can eventually become fossil fuels, storing the carbon beneath the Earth's surface. However, burning fossil fuels releases this stored carbon back into the atmosphere in the form of CO₂, contributing to the global carbon budget imbalance.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

You are working with an artist who has been commissioned to make a sculpture for a big city in the eastern United States. The artist is wondering what material to use to make her sculpture because she has heard that acid rain in the eastern United States might destroy it over time. You take samples of granite, marble, bronze, and other materials, and place them outdoors for a long time in the big city. You periodically examine the appearance and measure the mass of the samples. (a) What observations would lead you to conclude that one or more of the materials are well-suited for the sculpture? (b) What chemical process (or processes) is (are) the most likely responsible for any observed changes in the materials? [Section 18.2]

The average bond enthalpies of the \(\mathrm{C}-\mathrm{F}\) and \(\mathrm{C}-\) Cl bonds are 485 \(\mathrm{kJ} / \mathrm{mol}\) and 328 \(\mathrm{kJ} / \mathrm{mol}\) , respectively. (a) What is the maximum wavelength that a photon can possess and still have sufficient energy to break the \(\mathrm{C}-\mathrm{F}\) and \(\mathrm{C}-\mathrm{Cl}\) bonds, respectively? (b) Given the fact that \(\mathrm{O}_{2}, \mathrm{N}_{2},\) and \(\mathrm{O}\) in the upper atmosphere absorb most of the light with wavelengths shorter than \(240 \mathrm{nm},\) would you expect the photodissociation of \(\mathrm{C}-\mathrm{F}\) bonds to be significant in the lower atmosphere?

Do the reactions involved in ozone depletion involve changes in oxidation state of the O atoms? Explain.

(a) What is the difference between a CFC and an HFC? (b) It is estimated that the lifetime for HFCs in the stratosphere is \(2-7\) years. Why is this number significant? (c) Why have HFCs been used to replace CFCs? (d) What is the major disadvantage of HFCs as replacements for CFCs?

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.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free