Photosynthetic plants use the following reaction to produce glucose, cellulose, and so forth: $$ 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \stackrel{\text { Sunlight }}{\longrightarrow} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) $$ How might extensive destruction of forests exacerbate the greenhouse effect?

Short Answer

Expert verified
Extensive destruction of forests exacerbates the greenhouse effect by reducing the capacity of plants to absorb CO₂ from the atmosphere during photosynthesis and releasing large amounts of stored CO₂ back into the atmosphere through decomposition and combustion. The increased CO₂ levels, along with other greenhouse gases, trap more heat in the Earth's atmosphere, resulting in the warming of the planet and leading to climate change. Thus, protecting and restoring forests is essential for reducing the greenhouse effect and mitigating climate change.

Step by step solution

01

Understand photosynthesis process

Photosynthesis is the process by which plants, algae, and some bacteria convert sunlight into chemical energy, stored in the form of glucose molecules. During this process, the plants absorb carbon dioxide (CO₂) from the atmosphere and water (H₂O) from the soil, and in the presence of sunlight, they produce glucose (C₆H₁₂O₆) and release oxygen (O₂) back into the atmosphere. The general equation for photosynthesis is given by: \(6 CO_2(g) + 6 H_2O(l) \stackrel{\text{Sunlight}}{\longrightarrow} C_6H_{12}O_6(s) + 6 O_2(g)\)
02

Recognize carbon dioxide's role in the greenhouse effect

The greenhouse effect is a natural process that helps to maintain Earth's temperature by trapping heat from the sun within the atmosphere. It occurs because greenhouse gases (GHGs), including carbon dioxide (CO₂), water vapor (H₂O), methane (CH₄), and others, absorb and emit longwave infrared radiation. While the greenhouse effect is crucial for life on Earth, excessive concentrations of GHGs in the atmosphere can cause global temperatures to rise, leading to climate change. Carbon dioxide is one of the primary GHGs responsible for the greenhouse effect, and human activities, such as burning fossil fuels and deforestation, have substantially increased its concentration in the atmosphere.
03

Explain the consequences of deforestation

Forests play a critical role in regulating the global carbon cycle by absorbing and storing significant amounts of CO₂ through photosynthesis. They also release stored carbon as CO₂ when they are burned, decompose, or otherwise destroyed. Extensive deforestation, the large-scale removal of forests, interrupts this balance and can exacerbate the greenhouse effect in several ways: 1. The destruction of forests reduces the total amount of photosynthesis occurring on Earth, which leads to less CO₂ being removed from the atmosphere. 2. Forest fires and the decomposition of organic matter release vast amounts of CO₂ stored in wood and soil back into the atmosphere. 3. The conversion of forests into other land uses, such as agriculture or urban areas, often produces additional GHG emissions by altering the ecosystem's carbon storage capacity and vegetation structure.
04

Conclude the relationships between deforestation and the greenhouse effect

Extensive destruction of forests exacerbates the greenhouse effect by reducing the capacity of plants to absorb CO₂ from the atmosphere during photosynthesis, as well as releasing large amounts of stored CO₂ back into the atmosphere through decomposition and combustion. The increased CO₂ levels, along with other greenhouse gases, trap more heat in the Earth's atmosphere, resulting in the warming of the planet and leading to climate change. Thus, protecting and restoring forests is essential for reducing the greenhouse effect and mitigating climate change.

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Most popular questions from this chapter

A sample of nickel is heated to \(99.8^{\circ} \mathrm{C}\) and placed in a coffeecup calorimeter containing \(150.0 \mathrm{~g}\) water at \(23.5^{\circ} \mathrm{C}\). After the metal cools, the final temperature of metal and water mixture is \(25.0^{\circ} \mathrm{C}\). If the specific heat capacity of nickel is \(0.444 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\), what mass of nickel was originally heated? Assume no heat loss to the surroundings.

A system releases \(125 \mathrm{~kJ}\) of heat while \(104 \mathrm{~kJ}\) of work is done on it. Calculate \(\Delta E\).

Calculate \(\Delta H^{\circ}\) for each of the following reactions using the data in Appendix 4: $$ \begin{array}{c} 4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s) \\ 2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g) \\ 2 \mathrm{Na}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{O}(s)+\mathrm{CO}(\mathrm{g}) \end{array} $$ Explain why a water or carbon dioxide fire extinguisher might not be effective in putting out a sodium fire.

The enthalpy of neutralization for the reaction of a strong acid with a strong base is \(-56 \mathrm{~kJ} / \mathrm{mol}\) water produced. How much energy will be released when \(200.0 \mathrm{~mL}\) of \(0.400 \mathrm{M} \mathrm{HCl}\) is mixed with \(150.0 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{NaOH}\) ?

On Easter Sunday, April 3, 1983 , nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: \(2 \mathrm{HNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(s) \longrightarrow 2 \mathrm{NaNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)\) a. Calculate \(\Delta H^{\circ}\) for this reaction. Approximately \(2.0 \times 10^{4}\) gal nitric acid was spilled. Assume that the acid was an aqueous solution containing \(70.0 \% \mathrm{HNO}_{3}\) by mass with a density of \(1.42 \mathrm{~g} / \mathrm{cm}^{3}\). What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? \(\left(\Delta H_{\mathrm{f}}^{\circ}\right.\) for \(\mathrm{NaNO}_{3}(a q)=-467 \mathrm{~kJ} / \mathrm{mol}\) ) b. According to The Denver Post for April 4, 1983 , authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of \(\Delta H^{\circ}\), what was their major concern?

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