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Chapter 11: Problem 118

Explain why gases always occupy the entire container they are in, but solids and liquids do not.

Short Answer

Expert verified
Gases occupy the entire container they are in because they have negligible intermolecular forces and high kinetic energy, which causes their particles to move freely and independently, constantly spreading out and filling the available space. In contrast, solids and liquids do not occupy the entire container due to stronger intermolecular forces that hold their particles closer together, with solids having a fixed arrangement and liquids having a fixed volume but taking the shape of the container.

Step by step solution

01

Understanding the states of matter

Gases, liquids, and solids are the three basic states of matter. The main differences between these states lie in the arrangement and movement of their particles. In solids, the particles are held together by strong intermolecular forces and have a fixed shape and volume. In liquids, the particles are still close, but they are free to slide past each other, allowing the liquid to flow and take the shape of its container while maintaining a fixed volume. In gases, the particles are much farther apart and move more rapidly, which allows gases to take the shape and volume of their container.
02

Intermolecular forces

Intermolecular forces are the forces that hold the particles of a substance together. In solids, these forces are strong, and the particles are packed close together in a fixed arrangement. In liquids, the intermolecular forces are weaker, allowing the particles to flow and move past each other without breakingaway from each other completely. In gases, the intermolecular forces are negligible, so the gas particles move freely and independently from each other.
03

Kinetic energy of particles

The kinetic energy of particles (the energy they possess due to their motion) also plays a crucial role in determining the state of a substance. In solids, the particles have lower kinetic energy, as they are held together by stronger forces and their movements are restricted to vibrating around their fixed positions. In liquids, the particles have higher kinetic energy than in solids, and they move more freely, allowing them to slide past each other. In gases, the particles have the highest kinetic energy, moving rapidly in all directions, bouncing off each other and the container walls.
04

Gases occupying the entire container

Now that we understand the differences between the states of matter, it becomes easier to explain why gases always occupy the entire container they are in. Since the intermolecular forces are negligible in gases, there is nothing holding the particles close together. Furthermore, the high kinetic energy of the gas particles means that they are constantly in motion, bouncing off each other and the container walls. As a result, gas particles will continue to spread out and fill the space available to them, eventually occupying the entire container.
05

Solids and liquids not occupying the entire container

In contrast, solids and liquids do not occupy the entire container because of the stronger intermolecular forces present. In solids, the particles are held together in a fixed arrangement, and the shape is unaffected by the container. The shape of a liquid is determined by the container, but the volume does not change because the particles are still close together, held in place by the intermolecular forces. Therefore, solids and liquids do not occupy the entire container like gases do.

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Most popular questions from this chapter

What happens to the volume of a gas in a cylinder with a movable piston if: (a) The pressure is doubled while the temperature is held constant? (b) The temperature is doubled while the pressure is held constant? (c) The pressure and the temperature are both doubled? (The movable piston means the volume of the cylinder, and therefore of the gas, can change.)

True or false? \(1 \mathrm{~atm}=76 \mathrm{~mm} \mathrm{Hg}=760 \mathrm{~cm} \mathrm{Hg}\). If false, fix it.

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In an ideal gas, the molecules are considered to have no forces.

A 7.24-g sample of gas is contained in a 4.00-L flask. Its pressure is \(765.0 \mathrm{~mm} \mathrm{Hg}\), and its temperature is \(25.0^{\circ} \mathrm{C}\). What is the molar mass of this gas?
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