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Chapter 10: Problem 6

Why does a gas fill its container, but a liquid does not?

Short Answer

Expert verified
Gases fill their containers because their particles are in constant motion and exert pressure on the container's walls, having enough energy to occupy the entire volume. Conversely, liquids only assume the shape of their container, not filling it completely, because their particles have less energy, are more attracted to each other, and cannot move as freely as gas particles.

Step by step solution

01

Understand Particle Motion

The first step to understanding why a gas fills its container but a liquid does not, involves understanding how particles in different states of matter behave. Particles in a gas have a lot of kinetic energy and move in random, high-speed directions. This constant motion and lack of attraction between particles allows a gas to expand and fill its container.
02

Compare with Liquid Behavior

Now compare this to a liquid. Liquid particles are closer together and have less kinetic energy than gas particles. This does cause liquid to take the shape of its container, but only to the extent of its volume. This is why a liquid does not expand to fill its container.
03

Explain Gas Behavior

Next, explain this behavior with gas. As gas particles move and collide with their container's walls, they exert pressure. This pressure, along with the high-speed, random motion of the gas particles in all directions, allows the gas to fill the container completeley, regardless of the container's shape or volume.

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Key Concepts

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

Particle Motion in States of Matter
Understanding how particles move in different states of matter is fundamental to grasping why a gas fills its container while a liquid does not. In the gaseous state, particles possess a high degree of freedom and move in random, rapid motions. This is due to the amount of kinetic energy they have; a greater amount means more vigorous movement. In contrast, liquid particles are packed more closely, with attractions between them restricting their motion predominantly to vibrational and some translational movements, rather than the extensive freedom seen in gases. This explains why liquids assume the shape of the bottom of a container rather than expanding throughout.
Gas Expansion
The expansion of gas is a direct consequence of the energetic movement of its particles. The concept of gas expansion can be elucidated by imagining a multitude of tiny particles bouncing off the walls of their container with significant force. Each collision spreads the particles further apart, as they possess sufficient kinetic energy to overcome any attractions between them. This innate tendency of gas particles to expand is what allows them to occupy any volume available to them, completely filling their container.
Kinetic Energy and States of Matter
Kinetic energy, the energy of motion, is pivotal in differentiating between the states of matter. In gases, the high kinetic energy of particles allows for constant, dynamic motion, dictating the ability of these particles to fill a container completely. On the other hand, particles in liquids have less kinetic energy, which confines them to a limited space and prevents expansion to fill a container in the way gases do. This concept illustrates why kinetic energy is such a critical factor in the behavior of matter in different physical states.
Liquid Behavior
Liquid behavior can be characterized by the moderate kinetic energy of its particles, allowing them to slide past one another, conforming to the container's shape. However, it is the balance between this kinetic energy and the intermolecular forces that keeps the liquid from expanding. The inherent surface tension within liquids also contributes to their inability to expand and fill a container like gases; liquids tend to minimizing their surface area due to cohesion among molecules.
Pressure Exerted by Gases
When discussing the pressure exerted by gases, it's essential to capture the continual collisions between gas particles and the container walls. Each collision imparts force onto the container's surfaces, which collectively is recognized as pressure. This activity is relentless due to the gas particles' continuous and random motion, driven by their kinetic energy. A key factor affecting this pressure is the volume of the container; a smaller volume results in more frequent collisions and thus, higher pressure, following the principles described by Boyle's Law in chemistry.

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Most popular questions from this chapter

Explain how an increase in the strength of intermolecular forces affects each of the following properties of a substance. (a) vapor pressure of a solid (b) hardness of a molecular solid (c) boiling point of a liquid (d) viscosity of a liquid (e) melting point of a molecular solid

Arrange the following substances in order of increasing boiling point: \(\mathrm{Br}_{2}, \mathrm{Cl}_{2}\), and \(\mathrm{I}_{2}\).

What is surface tension? Discuss properties of liquids that are controlled by surface tension.

How is the vapor pressure of a liquid related to its boiling point?

Arrange the following substances in order of increasing boiling point: \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{OH}\), and \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\).
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