diff --git a/docs/sch3uz.md b/docs/sch3uz.md
index c158b2a..6e3786f 100644
--- a/docs/sch3uz.md
+++ b/docs/sch3uz.md
@@ -393,7 +393,7 @@ Although the solution may be kept in the flask briefly, if it is not used soon i
 
 ### Gas laws
 
-According to the **kinetic molecular theory**, gases are largely empty empty space with partiles moving randomly in straight lines due to weak or no intermolecular forces acting on them. Gas particles:
+According to the **kinetic molecular theory**, gases are largely empty empty space with particles moving randomly in straight lines due to weak or no intermolecular forces acting on them. Gas particles:
 
  - move in all directions,
  - are much smaller than the spaces between them,
@@ -403,6 +403,17 @@ According to the **kinetic molecular theory**, gases are largely empty empty spa
 
 Because gases are the only state of matter that have negligible intermolecular forces within the substance and so move independently of one another, they are the only **compressible** state of matter.
 
+**Boyle's law** states that the pressure and volume of a fixed amount of an ideal gas are inversely proportional to each other at a **constant temperature**.
+$$P\propto\frac{1}{V}$$
+
+<img src="/resources/images/pv-graph.png" width=700>(Source: Kognity)</img>
+
+**Charles' law** states that the **absolute** temperature and volume of a fixed amount of an ideal gas are directly proportional to each other at a **constant pressure**.
+$$V\propto T$$
+
+**Gay-Lussac's law** states that the **absolute** temperature and pressure of a fixed amount of an ideal gas are directly proportional to each other at **constant volume**.
+$$P\propto T$$
+
 ## 2.1 - Atoms
 
 !!! definition
diff --git a/docs/sph3u7.md b/docs/sph3u7.md
index ac1889f..c710e4a 100644
--- a/docs/sph3u7.md
+++ b/docs/sph3u7.md
@@ -602,6 +602,8 @@ $$p=\frac{F}{A}$$
 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:
 $$pV=nRT$$
 
+Please see [HL Chemistry#Gas laws](/sch3uz/#gas-laws) for more information.
+
 ## 4.1 - Oscillations
 
 !!! definition