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Chapter 8: Problem 2

List the three common phases in the order they exist from lowest energy to highest energy.

Short Answer

Expert verified
Solid, liquid, gas (from lowest to highest energy).

Step by step solution

01

Identify the Phases

The three common phases of matter are solid, liquid, and gas. Each phase has a different energy level due to the arrangement and movement of its particles.
02

Determine Energy Levels

In the solid phase, particles are closely packed and vibrate in place, resulting in the lowest energy state. In the liquid phase, particles have more energy, allowing them to move past each other while remaining in contact. In the gas phase, particles have the highest energy, moving freely and far apart from each other.
03

Order the Phases by Energy

Based on the energy levels determined in the previous step, arrange the phases from lowest to highest energy. Solid has the lowest energy, followed by liquid, and gas has the highest energy.

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Key Concepts

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

Solid Phase
The solid phase is characterized by particles that are tightly packed together. This arrangement allows for minimal movement.
These particles only vibrate slightly in their fixed positions, which means they have relatively low kinetic energy.
  • Solids have a definite shape and volume. This is because the particles are arranged in a closely knit structure, often in a specific, regular pattern known as a crystal lattice.
  • Due to the strong intermolecular forces holding the particles in place, solids are incompressible and have high density compared to liquids and gases.
Solids can change to liquids through a process called melting, requiring energy input to overcome the intermolecular forces.
Liquid Phase
The liquid phase is a fascinating state of matter where particles have more energy compared to solids. In this phase, particles are not as tightly held together.
They can move around more freely while still maintaining contact with each other.
  • Liquids have a definite volume like solids but lack a fixed shape. They take the shape of their container, demonstrating fluidity.
  • The particles in a liquid are more spread out than in a solid but less than in a gas, meaning liquids are less dense than solids and more than gases.
Throughout the liquid phase, substances can easily flow and mix, making it possible for them to be poured or stirred. When heated, liquids can transition to gases, in a transformation known as vaporization.
Gas Phase
The gas phase is where particles have the highest energy and display some unique characteristics. In this phase, particles are far apart and move independently of each other.
This independent movement results in gases spreading out to fill the spaces available, irrespective of the size or shape of the container.
  • Gases have neither a defined shape nor a definite volume. They expand and contract significantly, depending on the external conditions like temperature and pressure.
  • The low density of gases compared to solids or liquids is due to the large spaces between its particles.
In the gas phase, particles move at high speeds, constantly colliding with each other and the walls of their container. This property leads to diffusion and effusion, allowing gases to mix easily and exert pressure on surfaces.

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Most popular questions from this chapter

An air/gas vapor mix in an automobile cylinder has an initial temperature of \(450 \mathrm{~K}\) and a volume of \(12.7 \mathrm{~cm}^{3}\). The gas mix is heated to \(565^{\circ} \mathrm{C}\). If pressure and amount are held constant, what is the final volume of the gas in cubic centimeters?

Does the identity of a gas matter when using Charles's law? Why or why not?

According to the kinetic theory of gases, the individual gas particles are (always, frequently, never) moving.

Arrange the following pressure quantities in order from smallest to largest: \(1 \mathrm{mmHg}\), \(1 \mathrm{~Pa}\), and 1 atm.

The equation for the formation of ammonia gas \(\left(\mathrm{NH}_{3}\right)\) is as follows: $$ N_{2(g)}+3 H_{2(g)} \rightarrow 2 N H_{3(g)} $$ At \(500^{\circ} \mathrm{C}\) and \(1.00 \mathrm{~atm}, 10.0 \mathrm{~L}\) of \(\mathrm{N}_{2}\) gas are reacted to make ammonia. a. If the pressures and temperatures of \(\mathrm{H}_{2}\) and \(\mathrm{NH}_{3}\) were the same as those of \(\mathrm{N}_{2}\), what volume of \(\mathrm{H}_{2}\) would be needed to react with \(\mathrm{N}_{2}\), and what volume of \(\mathrm{NH}_{3}\) gas would be produced? b. Compare your answers to the balanced chemical equation. Can you devise a "shortcut" method to answer Exercise \(4 \mathrm{a}\) ?
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