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Chapter 15: Problem 50

(a) What is the difference between evaporation and boiling? (b) Can a solid evaporate?

Short Answer

Expert verified
Evaporation occurs at any temperature from the surface, boiling occurs at a specific boiling point within a liquid. Solids can sublimate, not evaporate.

Step by step solution

01

Understanding Evaporation

Evaporation is a process where molecules at the surface of a liquid gain enough energy to change into a gas. It happens at any temperature below the boiling point and occurs at the surface of the liquid.
02

Understanding Boiling

Boiling is a process where a liquid turns into a gas at a specific temperature known as the boiling point. During boiling, vapor bubbles form within the liquid and rise to the surface.
03

Key Differences

The main difference between evaporation and boiling is that evaporation is a surface phenomenon and occurs at any temperature, while boiling is a bulk phenomenon that occurs at a specific temperature (boiling point).
04

Solid Evaporation

Generally, solids do not evaporate in the way liquids do, because molecules in a solid are not free to move. However, some solids can sublimate, which is a direct transition from solid to gas.

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Key Concepts

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

Evaporation
Evaporation is a natural and essential process, playing a crucial role in the water cycle. It occurs when molecules at the surface of a liquid gain enough kinetic energy to overcome intermolecular forces and transition into the gaseous state. Unlike boiling, evaporation can happen at any temperature, as long as the liquid molecules have sufficient energy. Because it's a surface phenomenon, factors like temperature, surface area, and air movement can affect the rate of evaporation. In warmer conditions, molecules move more energetically, leading to faster evaporation.

Here are some key points about evaporation:
  • Occurs only at the surface of the liquid.
  • Does not require a specific temperature.
  • Rate increases with higher temperatures and larger surface areas.
Boiling
Boiling is a fundamental phase transition where a liquid changes to a gas throughout its entire volume, not just on the surface. This process happens when the liquid reaches its boiling point, a specific temperature where vapor pressure matches atmospheric pressure. At this point, vapor bubbles form inside the liquid and rise to the surface, indicating a rapid state change.

Understanding the conditions of boiling is vital:
  • Occurs at a specific temperature called the boiling point.
  • Involves the entire liquid, not just the surface.
  • Boiling point can vary with changes in atmospheric pressure.
Sublimation
Sublimation is an intriguing phase transition where a solid directly turns into a gas without passing through the liquid state. This process is less common than evaporation or boiling but can be observed in materials such as dry ice (solid carbon dioxide) and iodine. Sublimation occurs under specific conditions, often requiring reduced pressure or temperature increases.

Key takeaways on sublimation include:
  • Direct change from solid to gas.
  • No intermediate liquid phase involved.
  • Observed in certain materials under specific conditions.
States of Matter
Matter can exist in different states, primarily solid, liquid, and gas, with each state having distinct properties. Solids have fixed shapes and volumes because their molecules are tightly packed, only vibrating in place. Liquids have definite volumes but take the shape of their containers, as the molecules can slide past one another. Gases have neither fixed volumes nor shapes, with molecules moving freely and quickly.

The transition between these states is known as a phase change, influenced by temperature and pressure. Understanding these states is essential to grasp how materials behave in various conditions.
  • Solid: fixed shape and volume.
  • Liquid: definite volume, shape of the container.
  • Gas: no fixed shape or volume.

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Most popular questions from this chapter

Ammonia is used as a refrigerant in some industrial refrigeration units. The molar enthalpy of vaporization of liquid ammonia is \(23.33 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}\). Calculate the amount of heat absorbed in the vaporization of \(5.00\) kilograms of \(\mathrm{NH}_{3}(l)\)

Sketch the phase diagram for oxygen using the following data: $$ \begin{array}{lcc} \hline & \text { Triple point } & \text { Critical point } \\ \hline \text { temperature/K } & 54.3 & 154.6 \\ \text { pressure/Torr } & 1.14 & 37826 \\ \hline \end{array} $$ The normal melting point and normal boiling point of oxygen are \(-218.8^{\circ} \mathrm{C}\) and \(-183.0^{\circ} \mathrm{C}\). Does oxygen melt under an applied pressure as water does?

Arrange the following molecules in order of increasing molar enthalpy of vaporization: \(\begin{array}{llll}\mathrm{CH}_{4} & \mathrm{C}_{2} \mathrm{H}_{6} & \mathrm{CH}_{3} \mathrm{OH} & \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\end{array}\)

Given that \(23.6\) kilojoules of heat are required to completely vaporize \(60.0\) grams of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\) at \(80.1^{\circ} \mathrm{C}\), calculate the molar enthalpy of vaporization, \(\Delta H_{\text {vap }}\), of benzene.

(*) Steel can be made by inserting atoms of carbon into the spaces between the atoms in metallic iron. Iron has a body-centered crystal structure with a density of \(7.86 \mathrm{~g} \cdot \mathrm{cm}^{-3}\). Carbon has an atomic radius of \(77 \mathrm{pm}\). Show that there is enough space between the iron atoms to hold a carbon atom.
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