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(LEC-01) Kinetic Theory of gases | Assumption of Kinetic theory of gases | IITJAM || B.Sc. | M.Sc. |

Physics Darshan・33 minutes read

The lecture series covers the Kinetic Theory of Gases from basic to advanced levels, emphasizing practical application through numerical problem-solving and introducing the study of gas molecules' motion and energy. The importance of understanding the three states of matter, the evolution of Kinetic Theory of Gases, and the characteristics of ideal gases, including Avogadro's number and the ideal gas law equations, are also highlighted.

Insights

  • Kinetic Theory of Gases delves into the motion and energy of gas molecules, emphasizing the study of their behavior through mathematical formulations and practical applications.
  • The evolution of Kinetic Theory of Gases, driven by scientists like Bernoulli and Maxwell, revolutionized the understanding of matter, revealing the nature of gas molecules, the concept of ideal gases, and the significance of Avogadro's number in defining the properties of gases.

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Recent questions

  • What is the Kinetic Theory of Gases?

    The Kinetic Theory of Gases is a study of gas molecules' motion and energy, emphasizing the random movement of gas particles and their interactions.

  • How are gas molecules different from solids and liquids?

    Gas molecules are farthest apart compared to solids and liquids, with weaker intermolecular forces and more freedom of movement.

  • Who discovered that atoms were not the smallest particles?

    The discovery that atoms were not the smallest particles was made in 1879 with the revelation of the electron, leading to the understanding that molecules were combinations of atoms.

  • What is Avogadro's number?

    Avogadro's number is approximately 6.02 x 10^23, representing the number of molecules in one mole of gas and playing a crucial role in gas calculations.

  • What are the characteristics of an ideal gas?

    An ideal gas is characterized by point mass molecules with zero dimensions, moving randomly with equal probability and uniform distribution, exhibiting perfectly elastic collisions and possessing only kinetic energy.

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Summary

00:00

Kinetic Theory of Gases Lecture Series

  • Lecture series on Kinetic Theory of Gases starting from basic level to advanced level
  • Suitable for students from fresher B.Sc. level to those preparing for competitive exams like GATE or JAM
  • Topics covered include Maxwell Distribution of Molecular Velocity, Equator No Energy, and Degree of Freedom
  • Emphasis on concrete theory presentation and solving numerical problems
  • Importance of practical application through solving numericals for effective learning
  • Introduction to Kinetic Theory of Gases as a study of gas molecules' motion and energy
  • Three states of matter: solid, liquid, and gas, with varying intermolecular forces
  • All gas molecules are identical in size and appearance
  • Strongest intermolecular forces in solids, followed by liquids, and least in gases
  • Evolution of Kinetic Theory of Gases through mathematical formulations by scientists like Bernoulli and Maxwell

16:37

"Discovery of Electron and Kinetic Theory"

  • The discovery of the electron in 1879 revealed that atoms were not the smallest particles.
  • At that time, atoms were considered the smallest, with molecules being combinations of atoms.
  • Molecules in solids are closest, in liquids they are slightly farther, and in gases they are farthest apart.
  • Forces between molecules can be negligible, making them easy to study.
  • Scientists conducted experiments, formulated mathematical theories, and developed the Kinetic Theory of Gases.
  • The theory aimed to simplify calculations and mathematical formulations for gases.
  • One mole of gas contains approximately 6.02 x 10^23 molecules, known as Avogadro's number.
  • The ideal gas law equations PV = nRT and PV = NT are followed by gases under specific conditions.
  • The number of molecules in gases can be calculated based on pressure, volume, and temperature.
  • Gas molecules are assumed to be point masses with zero dimensions, moving randomly in all directions with equal probability and uniform distribution in the absence of external fields.

35:39

Uniformity and Individuality in Gas Molecules

  • In the case of uniform distribution, all molecules in a gas have identical surroundings, with no change as one moves from one molecule to another.
  • Ideal gas is characterized by isotropic surroundings, meaning that every molecule's surroundings are identical, allowing movement to any position within the gas.
  • Real gas molecules maintain their individuality, while ideal gas molecules exhibit uniformity in their surroundings.
  • Intermolecular forces in gases are negligible, with only a significant respect force present between gas molecules.
  • Ideal gas possesses only kinetic energy, with collisions between molecules being perfectly elastic, resulting in no energy loss.
  • Molecules in gases move with varying velocities, ranging from zero to infinity, with the speed of light being the maximum possible velocity and absolute zero velocity being unattainable.
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