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Chapter 13: Problem 28

What is thermal pollution? Why is it harmful to aquatic life?

Short Answer

Expert verified
Thermal pollution is the rise in temperature in bodies of water due to human activities like industrial output. This rise in temperature can be harmful to aquatic life by reducing oxygen levels in the water, disrupting life cycles, and even causing the death of species that cannot resist the elevated temperatures.

Step by step solution

01

Define Thermal Pollution

Thermal pollution refers to an increase in the normal temperature of natural bodies of water, which may be a result of human activities. Common contributors to thermal pollution are power plants, industrial manufacturers, and residential areas that release hot or warm water into nearby bodies of water such as rivers, seas, or oceans.
02

Explain Effects on Aquatic Life

Increasing the temperature of water bodies can have harmful effects on aquatic life. Warmer waters carry less oxygen, which aquatic creatures need to survive. This reduction in oxygen levels can lead to the death of fish and other aquatic organisms. In addition, warmer temperatures can disrupt the life cycle of many aquatic species, with certain stages requiring specific temperature conditions to occur such as breeding or hatching. Moreover, some species might not be able to resist the heat and die, causing a shift in the local biodiversity.

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Most popular questions from this chapter

Calculate the molality of each of these solutions: (a) \(14.3 \mathrm{~g}\) of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) in \(676 \mathrm{~g}\) of water, (b) 7.20 moles of ethylene \(\operatorname{glycol}\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)\) in \(3546 \mathrm{~g}\) of water.

A mixture of ethanol and 1 -propanol behaves ideally at \(36^{\circ} \mathrm{C}\) and is in equilibrium with its vapor. If the mole fraction of ethanol in the solution is \(0.62,\) calculate its mole fraction in the vapor phase at this temperature. (The vapor pressures of pure ethanol and 1 -propanol at \(36^{\circ} \mathrm{C}\) are \(108 \mathrm{mmHg}\) and 40.0 \(\mathrm{mmHg}\), respectively.)

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The solubility of \(\mathrm{N}_{2}\) in blood at \(37^{\circ} \mathrm{C}\) and at a partial pressure of \(0.80 \mathrm{~atm}\) is \(5.6 \times 10^{-4} \mathrm{~mol} / \mathrm{L}\). A deepsea diver breathes compressed air with the partial pressure of \(\mathrm{N}_{2}\) equal to \(4.0 \mathrm{~atm} .\) Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of \(\mathrm{N}_{2}\) gas released (in liters) when the diver returns to the surface of the water, where the partial pressure of \(\mathrm{N}_{2}\) is \(0.80 \mathrm{~atm}\)

Calculate the molarity and the molality of \(\mathrm{NH}_{3}\) for a solution of \(30.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) in \(70.0 \mathrm{~g}\) of water. The density of the solution is \(0.982 \mathrm{~g} / \mathrm{mL}\).
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