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SCI10 Q4 MOD1.3

Kinetic Molecular Theory of Gases

Properties of Matter

  • Definition: Matter has mass and volume.

  • Observable Properties: Hardness, texture, color, flexibility, malleability, electrical conductivity:

    • Solids & Liquids: These properties are easily studied.

    • Gases: Properties are not directly measurable; behavior is explained through Kinetic Molecular Theory (KMT).

States of Matter


    • Solid: Particles are very close and move in fixed positions (strong attractions).

    • Liquid: Particles are far apart and can slide against each other (weaker attractions).

    • Gas: Particles are far apart with very weak forces of attraction and have no definite shape or volume (freely moving).

Key Differences in Properties of States

Property

Solid

Liquid

Gas

Shape

Fixed shape

Takes shape of the container

Takes shape of the container

Volume

Fixed volume

Fixed volume

No definite volume

Density

Quite high density

High density

Very low density

Diffusion

No diffusion

Slow diffusion

Rapid diffusion

Ease of Compression

Difficult to compress

Slightly compressible

Easily compressed

Kinetic Molecular Theory (KMT) Overview

  • Explains properties and behavior of gases:

    • Expresses relationships among pressure, volume, and temperature at a molecular level.

    • Discusses behavior of atoms and molecules making up gases.

General Observations About Gases

  • Gases: occupy a small space, can spread, are composed of tiny particles in constant motion.

  • Increase in temperature causes gas particles to move and spread faster.

The KMT Postulates

  1. Large Number of Particles: Gases consist of a vast number of particles that are very small compared to the distance between them.

  2. Random Motion and Collision: Gas particles move randomly and collide with each other and their container, creating pressure.

  3. Elastic Collisions: Collisions between gas molecules are perfectly elastic, meaning no energy is lost.

  4. Negligible Interactions: Gas particles experience negligible attractions and repulsions.

  5. Kinetic Energy and Temperature: Average kinetic energy of gas particles is directly proportional to their temperature (Kelvin).


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SCI10 Q4 MOD1.3

Kinetic Molecular Theory of Gases

Properties of Matter

  • Definition: Matter has mass and volume.

  • Observable Properties: Hardness, texture, color, flexibility, malleability, electrical conductivity:

    • Solids & Liquids: These properties are easily studied.

    • Gases: Properties are not directly measurable; behavior is explained through Kinetic Molecular Theory (KMT).

States of Matter

    • Solid: Particles are very close and move in fixed positions (strong attractions).

    • Liquid: Particles are far apart and can slide against each other (weaker attractions).

    • Gas: Particles are far apart with very weak forces of attraction and have no definite shape or volume (freely moving).

Key Differences in Properties of States

Property

Solid

Liquid

Gas

Shape

Fixed shape

Takes shape of the container

Takes shape of the container

Volume

Fixed volume

Fixed volume

No definite volume

Density

Quite high density

High density

Very low density

Diffusion

No diffusion

Slow diffusion

Rapid diffusion

Ease of Compression

Difficult to compress

Slightly compressible

Easily compressed

Kinetic Molecular Theory (KMT) Overview

  • Explains properties and behavior of gases:

    • Expresses relationships among pressure, volume, and temperature at a molecular level.

    • Discusses behavior of atoms and molecules making up gases.

General Observations About Gases

  • Gases: occupy a small space, can spread, are composed of tiny particles in constant motion.

  • Increase in temperature causes gas particles to move and spread faster.

The KMT Postulates

  1. Large Number of Particles: Gases consist of a vast number of particles that are very small compared to the distance between them.

  2. Random Motion and Collision: Gas particles move randomly and collide with each other and their container, creating pressure.

  3. Elastic Collisions: Collisions between gas molecules are perfectly elastic, meaning no energy is lost.

  4. Negligible Interactions: Gas particles experience negligible attractions and repulsions.

  5. Kinetic Energy and Temperature: Average kinetic energy of gas particles is directly proportional to their temperature (Kelvin).