A gas is a fundamental state of matter that is a collection of molecules with significant distance between them. Gases are highly compressible and are the least dense state of matter.
Pressure and volume are inversely proportional to each other, volume and temperature are proportional to each other, pressure and temperature are proportional to each other, and the number of moles and volume are proportional to each other.
The ideal gas law relates pressure, volume, number of moles, and temperature using the ideal gas constant.
The van der Waals modified gas law takes into account molecular size, intermolecular forces, and volume to define real gases that deviate from ideal behavior.
The ideal gas law assumes the following: (1) the collisions between molecules are elastic and their motion is frictionless, (2) the total volume of the gas molecules is orders of magnitudes smaller than the volume occupied by the gas, (3) there are no intermolecular forces acting between the molecules or their surroundings, and (4) the molecules are constantly in motion, and the distance between two molecules is significantly larger than the size of individual molecules.
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