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Chapter 10: Problem 11

Why does water evaporate?

Short Answer

Expert verified
Water evaporates because the kinetic energy of its molecules, influenced by temperature, allows some of them to break the relatively weak intermolecular hydrogen bonds and transform from the liquid phase to the gaseous phase (water vapor). The rate of evaporation depends on factors like temperature, humidity, and surface area.

Step by step solution

01

Understanding Intermolecular Forces

Intermolecular forces are the forces between molecules. In the case of water, there are hydrogen bonds between water molecules. These bonds are relatively weaker compared to covalent bonds. The strength of intermolecular forces affects the rate at which water evaporates.
02

Explaining Kinetic Molecular Theory

The kinetic molecular theory states that all particles (atoms, ions, and molecules) are in constant motion. Due to their motion, they possess kinetic energy. The kinetic energy of particles is directly proportional to the temperature of the substance. Higher temperatures indicate increased kinetic energy, hence, particles move with greater speed.
03

Describing the Effect of Temperature on Evaporation

When the temperature increases, the kinetic energy of the water molecules also increases, causing them to move faster and with more energy. As a result, some water molecules acquire enough energy to break the hydrogen bonds holding them together. These molecules then escape the liquid state and become gaseous, which we recognize as water vapor. This process is called evaporation.
04

Factors Affecting the Rate of Evaporation

The rate at which water evaporates depends on several factors such as temperature, humidity, and surface area. A higher temperature increases the rate of evaporation, while higher humidity decreases it. A larger surface area of water also allows more molecules to evaporate at a faster rate. In conclusion, water evaporates due to the kinetic energy of its molecules, which allows some molecules to break the intermolecular hydrogen bonds and escape the liquid phase. The rate of evaporation depends on factors such as temperature, humidity, and surface area.

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Most popular questions from this chapter

What quantity of energy does it take to convert \(0.500 \mathrm{~kg}\) ice at \(-20 .{ }^{\circ} \mathrm{C}\) to steam at \(250 .{ }^{\circ} \mathrm{C}\) ? Specific heat capacities: ice, \(2.03 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} ;\) liquid, \(4.2 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} ;\) steam, \(2.0 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} ; \Delta H_{\text {vep }}=\) 40.7 \(\mathrm{kJ} / \mathrm{mol} ; \Delta H_{\mathrm{fec}}=6.02 \mathrm{~kJ} / \mathrm{mol}\).

Compare and contrast the structures of the following solids. a. diamond versus graphite b. silica versus silicates versus glass

Consider a sealed container half-filled with water. Which statement best describes what occurs in the container? a. Water evaporates until the air is saturated with water vapor; at this point, no more water evaporates. b. Water evaporates until the air is overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. c. Water does not evaporate because the container is sealed. d. Water evaporates, and then water evaporates and recondenses simultaneously and continuously. e. Water evaporates until it is eventually all in vapor form. Explain each choice. Justify your choice, and for choices you did not pick, explain what is wrong with them.

What type of solid will each of the following substances form? a. \(\mathrm{CO}_{2}\) g. \(\mathrm{KBr}\) b. \(\mathrm{SiO}_{2}\) h. \(\mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{Si}\) i. \(\mathrm{NaOH}\) d. \(\mathrm{CH}_{4}\) j. \(\underline{U}\) e. Ru k. \(\mathrm{CaCO}_{3}\) f. \(\mathrm{I}_{2}\) 1\. \(\mathrm{PH}_{3}\)

Rationalize the difference in boiling points for each of the following pairs of substances: a. \(n\) -pentane \(\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\) \(36.2^{\circ} \mathrm{C}\) neopentane CC(C)(C)C \(9.5^{\circ} \mathrm{C}\) b. HF \(20^{\circ} \mathrm{C}\) \(\mathrm{HCl} \quad-85^{\circ} \mathrm{C}\) c. HCl \(-85^{\circ} \mathrm{C}\) \(\mathrm{LiCl} \quad 1360^{\circ} \mathrm{C}\) d. \(n\) -pentane \(\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\) \(36.2^{\circ} \mathrm{C}\) \(\begin{array}{lll}n \text { -hexane } & \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3} & 69^{\circ} \mathrm{C}\end{array}\)
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