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States of Matter
4 students

States of Matter

Properties and applications of Solids, Liquids and gases
Created byVinay Arya
Last updated 1/2020
English

What you'll learn

  • Properties of Solid, liquid and gases

Course content

2 sections • 10 lectures • 2h 22m total length

  • Introduction: 5.1. Contents of States11:59

    Explore the three states of matter—solids, liquids, and gases—and outline the course contents, including properties, gas laws, kinetic theory, and liquefaction concepts.

  • 5.2. Properties of Matter13:09

    Explore the states of matter—solids, liquids, and gases—and how particle attraction and thermal energy govern shape, volume, and phase changes. Heat and cool drive transitions between these states.

  • 5.3. Measurable properties of Gases20:11

    Explore the measurable properties of gases, including volume and pressure, and how barometers and manometers measure atmospheric and gas pressures.

  • 5.4. Gas Laws18:55

    Explore the gas laws—Boyle's, Charles', and the related ideal gas equation—through demonstrations of pressure, volume, and temperature using balloons, vacuum, dry ice, and liquid nitrogen.

  • 5.5. Ideal Gases and Dalton's law of Partial pressure11:09

    The lecture explains the ideal gas equation and the related gas laws, including Boyle's law and Dalton's law of partial pressures, and explores applications, diffusion, and effusion.

  • 5.6. Kinetic Molecular Theory of Gases20:30

    Explore the kinetic molecular theory of gases through a microscopic model of particles, elastic collisions, large empty space, Brownian motion, and temperature-driven changes in average kinetic energy and pressure.

  • 5.7. Maxwell's Boltzmann law and vander Waals Equation16:49

    Delve into the Maxwell–Boltzmann distribution and the ideal gas law, then present van der Waals corrections for volume and pressure, yielding the van der Waals equation.

  • 5.8. Liquification of Gases10:23

    Explore how gases liquefy by cooling, applying pressure, or expanding compressed gas, and how critical temperature limits liquefaction, with examples like liquid nitrogen, ammonia, and Freon.

  • 5.9. Liquid state and its properties10:17

    Explore the liquid state and its properties, including volume, shape, compression, density, and viscosity, and understand how intermolecular forces keep liquids cohesive while they take the container's shape.

  • 5.10. Properties of Liquids9:00

    Explore the properties of liquids, including fluidity, surface tension and the formation of a meniscus, diffusion differences from gases, and vapor pressure driving evaporation.

Requirements

  • Basics of Surroundings

Description

Matter exists in solid, liquid and gaseous states. Solids have fixed shape and volume, liquids have fixed volume but no fixed shape, gases have neither fixed shape nor fixed volume. We will interact about the arrangement of constituting particles of different states of matter, their characteristic properties and discuss the laws governing their behavior.

Intermolecular Forces. The force of attraction between molecules which keep molecules together are called intermolecular forces.

Molecular Interactional Energy. The energy due to force of attraction between molecules is called molecular interactional energy. Molecular interactions lead to intermolecular attractive and repulsive forces.

Thermal Energy. The energy which moves the molecules apart is called thermal energy. It is defined as energy possessed by matter by virtue of its temperature and is also measure of thermal motion or movement of molecules.

Change in State. It involves competition between ordering molecular interaction energy and disor­dering thermal energy.

Gaseous State. In gases, molecules have almost no molecular interactions and thermal motion is random translatory movement of molecules that is why they do not have fixed shape and volume because they have large intermolecular space, therefore weak force of attraction. For gases like hydrogen, helium intermolecular forces can be neglected at high temperature and low pressure.

Who this course is for:

  • Beginners, 11 grade students and research Scholars

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