Kinetic Molecular Theory of Gases

This flashcard set covers the historical contributions of chemists, the fundamental postulates of Kinetic Molecular Theory, and the mathematical derivations of gas laws and velocities.

Daniel Bernoulli (1738)

The scientist who put forward the kinetic molecular theory of gases.

R.J. Clausius (1857)

The scientist who derived the kinetic equation $PV = \frac{1}{3} mNc^2$ and deduced all the gas laws from it.

James Maxwell (1859)

The scientist who gave the law of distribution of velocities.

Boltzmann (1870)

The scientist who contributed to and studied the distribution of energies among the gas molecules.

van der Waals

The scientist who modified the general gas equation for real gases as $(P + \frac{an^2}{V^2})(V - nb) = nRT$.

Kinetic Molecular Theory of Gases (KMT)

A set of postulates that describes the nature and behaviour of an ideal gas.

Mono-atomic molecules

Gases consisting of single atoms, such as $He$, $Ne$, and $Ar$.

Elastic Collisions

A postulate of KMT stating that collisions among gas molecules are perfectly elastic, meaning no energy is lost.

Pressure

The force per unit area exerted by gas molecules due to their collisions with the walls of a container.

Average Kinetic Energy Postulate

The postulate stating that the average kinetic energy of gas molecules varies directly as the absolute temperature of the gas.

Clausius' Kinetic Equation

$PV = \frac{1}{3} mNc^2$, where $m$ is the mass of one molecule, $N$ is the number of molecules, and $\bar{c^2}$ is the mean square velocity.

Mean square velocity ($\bar{c^2}$)

The average of the squares of all possible velocities, defined as $\frac{n_1c_1^2 + n_2c_2^2 + n_3c_3^2 + \text{...}}{N}$.

Root mean square velocity ($C_{rms}$)

The square root of the mean square velocity, expressed as C_{rms} = \frac{\frac{3RT}{M}}.

Boyle's Law (from KMT)

At a constant temperature and number of moles, the product $PV$ is a constant quantity ($PV = k'$).

Most probable velocity

The velocity possessed by the maximum number of molecules, related to the quantitative relationship where higher temperature leads to greater velocities.