diff --git a/content/physics/thermodynamics.md b/content/physics/thermodynamics.md
index b97e523..3a87ffd 100644
--- a/content/physics/thermodynamics.md
+++ b/content/physics/thermodynamics.md
@@ -114,3 +114,88 @@ b=\frac{L}{4\pi r^2}
 $$
 
 The above is true when $L$ is procured from the source, most likely using the Boltzmann's law.
+# Gas Laws and the Ideal Gas Law
+
+## Ideal Gas Law
+The **Ideal Gas Law** is a fundamental equation describing the behavior of ideal gases:
+
+$$
+PV = nRT
+$$
+
+Where:
+- $P$ = Pressure (in atm, Pa, or another unit)
+- $V$ = Volume (in liters or cubic meters)
+- $n$ = Number of moles of gas
+- $R$ = Ideal gas constant ($0.0821 \, \mathrm{L \cdot atm \cdot mol^{-1} \cdot K^{-1}}$)
+- $T$ = Temperature (in Kelvin)
+
+This equation relates the pressure, volume, temperature, and quantity of an ideal gas.
+
+---
+
+## Boyle's Law
+**Boyle's Law** states that the pressure of a gas is inversely proportional to its volume when temperature and the number of moles are constant:
+
+$$
+P \propto \frac{1}{V} \quad \text{or} \quad P_1V_1 = P_2V_2
+$$
+
+### Key Points:
+- As volume decreases, pressure increases.
+- The relationship is hyperbolic.
+
+---
+
+## Charles's Law
+**Charles's Law** states that the volume of a gas is directly proportional to its absolute temperature when pressure and the number of moles are constant:
+
+$$
+V \propto T \quad \text{or} \quad \frac{V_1}{T_1} = \frac{V_2}{T_2}
+$$
+
+### Key Points:
+- As temperature increases, volume increases.
+- Temperature must be in Kelvin.
+
+---
+
+## Gay-Lussac's Law
+**Gay-Lussac's Law** states that the pressure of a gas is directly proportional to its absolute temperature when volume and the number of moles are constant:
+
+$$
+P \propto T \quad \text{or} \quad \frac{P_1}{T_1} = \frac{P_2}{T_2}
+$$
+
+### Key Points:
+- As temperature increases, pressure increases.
+- Temperature must be in Kelvin.
+
+---
+
+## Avogadro's Law
+**Avogadro's Law** states that the volume of a gas is directly proportional to the number of moles when pressure and temperature are constant:
+
+$$
+V \propto n \quad \text{or} \quad \frac{V_1}{n_1} = \frac{V_2}{n_2}
+$$
+
+### Key Points:
+- Adding more gas increases volume proportionally.
+- This law explains why equal volumes of gases contain equal numbers of molecules at the same temperature and pressure.
+
+---
+
+## Combined Gas Law
+The **Combined Gas Law** combines Boyle's, Charles's, and Gay-Lussac's Laws into one equation when the number of moles is constant:
+
+$$
+\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}
+$$
+
+This equation can be used to calculate changes in pressure, volume, or temperature of a gas sample.
+
+---
+
+Use these laws to analyze relationships between variables and predict gas behavior under different conditions!
+