Ideal Gas Law

Ideal Gas law

Some Flerfs understand there is a relation between pressure and temperature. But they never quantify what that would mean in reality.

TODO:

1. insert images/tables of measured pressure and temperature over altitude vs the predicted pressure by the Ideal Gas Law.
2. temperature/pressure insert measurements inside and outside

Formula

The most frequently introduced forms are:$$pV=nRT=n{k}_{\text{B}}{N}_{\text{A}}T=N{k}_{\text{B}}T$$where:

• $p$ is the absolute pressure of the gas,
• $V$ is the volume of the gas,
• $n$ is the amount of substance of gas (also known as number of moles),
• $R$ is the ideal, or universal, gas constant, equal to the product of the Wikipedia:Boltzmann constant and the Wikipedia:Avogadro constant,
• $k_{\text{B}}$ is the Wikipedia:Boltzmann constant,
• $N_A$ is the Wikipedia:Avogadro constant,
• $T$ is the absolute temperature of the gas,
• $N$ is the number of particles (usually atoms or molecules) of the gas.

In SI units, p is measured in pascals, V is measured in cubic metres, n is measured in moles, and T in kelvins scale is a shifted Celsius scale, where 0 K = −273.15 °C, the lowest possible temperature). R has for value 8.314 J/(mol·K) = 1.989 ≈ 2 cal/(mol·K), or 0.0821 L⋅atm/(mol⋅K).