From 973a4404185b3c12e579a630c134224ccea69df0 Mon Sep 17 00:00:00 2001 From: eggy Date: Tue, 12 Jan 2021 15:54:15 -0500 Subject: [PATCH] phys: gas laws 1 --- docs/sph3u7.md | 15 +++++++++++++++ 1 file changed, 15 insertions(+) diff --git a/docs/sph3u7.md b/docs/sph3u7.md index e93d017..ac1889f 100644 --- a/docs/sph3u7.md +++ b/docs/sph3u7.md @@ -587,6 +587,21 @@ $$Q=mL$$ ## 3.2 - Modelling a gas +### Ideal gases + +An ideal gas is an imaginary gas used to model real gases. The following assumptions are made: + + - Gas particles are all identical and perfectly spherical + - Gas particles do not exert any intermolecular forces — as such, their potential energy does not change + - Gas particles collide perfectly elastically + - Gas particles are so small that their volume is significantly smaller than that of the container + +The average kinetic energy of the gas particles is proportional to the temperature of a gas. A greater speed of gas particles also increases the **collisions** between gas particles and the walls of the box, therefore increasing **pressure**, therefore increasing **temperature**. The pressure of a gas on a surface can be expressed by the force $F$ over its area $A$. +$$p=\frac{F}{A}$$ + +The state of an ideal gas in a container can be modelled by the following equation, where $p$ is the pressure of the pressure in pascals or newtons per square metre ($\text{Pa}$ or $\text{Nm}^{-2}$), $V$ is the volume in cubic metres, $n$ is the number of moles of gas particles, $R$ is the universal gas constant ($R=8.31\text{J}\cdot\text{mol}^{-1}\cdot\text{K}^{-1}$), and $T$ is the temperature of the gas in Kelvin: +$$pV=nRT$$ + ## 4.1 - Oscillations !!! definition