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Chapter 10: Problem 71

Explain the difference between sublimation and evaporation.

Short Answer

Expert verified
Answer: The key differences between sublimation and evaporation include: 1. Phase Transition: Sublimation involves a solid substance changing directly into its gaseous state without passing through the liquid phase, while evaporation involves a liquid substance transforming into its gaseous state. 2. Temperature and Pressure Conditions: Sublimation occurs when the temperature and pressure of the solid are below the triple point, whereas evaporation occurs when the liquid's temperature is increased or the pressure is decreased. 3. Energy: Sublimation usually requires more energy than evaporation, as it involves overcoming both the solid's lattice energy and the liquid's intermolecular forces, whereas evaporation only involves overcoming the intermolecular forces between the liquid molecules.

Step by step solution

01

Definition of Sublimation

Sublimation is the process in which a solid substance transitions directly into its gaseous state without going through the liquid phase. This occurs when the temperature and pressure of the solid are below its triple point, which is the specific combination of temperature and pressure where all three phases (solid, liquid, and gas) of a substance can coexist in equilibrium.
02

Example of Sublimation

A common example of sublimation is the process of dry ice (solid carbon dioxide) turning into carbon dioxide gas. When dry ice is exposed to room temperature, it does not melt into a liquid but instead turns directly into gas, producing a fog-like appearance.
03

Definition of Evaporation

Evaporation is the process in which a liquid substance changes into its gaseous state due to an increase in temperature, pressure or both. In this process, molecules within the liquid gain kinetic energy and escape from the surface of the liquid, turning into gas.
04

Example of Evaporation

A common example of evaporation is the process of water turning into water vapor. When you boil a pot of water, the liquid water molecules gain enough energy to escape from the surface, turning into water vapor. Additionally, evaporation occurs when water puddles or wet clothes dry and turn into water vapor at room temperature, as the molecules in the liquid phase gain energy from the environment and become gaseous.
05

Key Differences between Sublimation and Evaporation

Here are the main differences between sublimation and evaporation: 1. Phase Transition: In sublimation, a solid substance changes directly into its gaseous state without passing through the liquid phase. In evaporation, a liquid substance transforms into its gaseous state. 2. Temperature and Pressure Conditions: Sublimation occurs when the temperature and pressure of the solid are below the triple point, whereas evaporation occurs when the liquid's temperature is increased, or the pressure is decreased. 3. Energy: Sublimation usually requires more energy than evaporation since transitioning from a solid to a gas involves overcoming both the solid's lattice energy and the liquid's intermolecular forces. In evaporation, only the intermolecular forces between the liquid molecules need to be overcome.

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Key Concepts

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

Sublimation
Sublimation is a fascinating phase transition where a solid turns directly into a gas without passing through the liquid state. Imagine you're holding a block of dry ice; instead of melting, it produces a mystifying fog as it becomes carbon dioxide gas. This process can occur because, at certain conditions, the molecules are so energetic that they break free from their solid lattice arrangement straight into the gas phase.

Importance in Nature and Technology

Sublimation isn't just a cool science experiment; it plays a role in the natural water cycle, where snow and ice can vaporize in cold, dry conditions. Additionally, it's an essential concept in freeze-drying, a technique to preserve food and pharmaceuticals by removing ice directly from frozen material, effectively preventing bacteria growth and spoilage.
Evaporation
Now, let's dip our toes into evaporation. This everyday phenomenon involves a liquid transforming into a gas. On a sunny day, you might observe a puddle disappearing, which is the essence of evaporation at work. It's not magic, but the result of individual liquid molecules gaining enough kinetic energy to break away from their peers and soar into the air as gas.

Role in Everyday Life

Evaporation isn't just about drying puddles; it's crucial in cooling technologies like air conditioning and refrigeration. It's also a key player in the water cycle, where it's responsible for turning bodies of water into humidity and clouds in the atmosphere. Plus, it's the reason we feel cooler after sweating 鈥� as sweat evaporates, it takes some heat away from our skin.
Triple Point

The triple point of a substance is where the magic of phase transitions takes on a whole new level. It's the specific set of pressure and temperature conditions where solids, liquids, and gases can all exist together in a delicate balance. To visualize this, picture a world where water can be ice, liquid, and vapor all at the same time.


This unique scenario is vital for calibrating thermometers and clearly shows the distinct properties of substances. Understanding the triple point helps us grasp why substances behave differently under varying atmospheric conditions. It's a cornerstone concept for chemists and physicists alike.

Kinetic Energy

In our exploration of phase transitions, kinetic energy is the invisible hero. Put simply, it's the energy that an object possesses due to its motion. The faster the molecules within a substance move, the higher their kinetic energy.


Crucial to Phase Changes

When molecules in a liquid gain kinetic energy, they can escape into the air as gas - a process you're familiar with as evaporation. Similarly, in sublimation, kinetic energy enables a solid's molecules to leap directly into the gaseous phase. Whether water evaporates or dry ice sublimates, it's kinetic energy behind the scenes, powering these transformations.

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Most popular questions from this chapter

One of the compounds in Figure \(\mathrm{P} 10.16\) is insoluble in water; the other has a water solubility of \(0.87 \mathrm{g} / 100 \mathrm{mL}\) at \(20^{\circ} \mathrm{C} .\) Identify which is which, and explain your reasoning.

Which phase of a substance (gas, liquid, or solid) is most likely to be the stable phase: (a) at low temperatures and high pressures; (b) at high temperatures and low pressures?

Explain why the solubility of the series of alcohols with the formula \(\mathrm{C}_{n} \mathrm{H}_{2 n+2} \mathrm{OH}\) decreases with increasing \(n\).

The boiling point of phosphine, \(\mathrm{PH}_{3}\left(-88^{\circ} \mathrm{C}\right),\) is lower than that of ammonia, \(\mathrm{NH}_{3}\left(-33^{\circ} \mathrm{C}\right)\), even though \(\mathrm{PH}_{3}\) has twice the molar mass of \(\mathrm{NH}_{3} .\) Why?

Explain why the melting point of methyl fluoride, \(\mathrm{CH}_{3} \mathrm{F}\) \(\left(-142^{\circ} \mathrm{C}\right),\) is higher than the melting point of methane, \(\mathrm{CH}_{4}\left(-182^{\circ} \mathrm{C}\right)\).
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