Let's get this chemistry party started 🎉! First, we need to understand the combined gas law. This law tells us that the pressure (p), volume (V), and temperature (T) of a gas are interconnected - a change in one results in changes in the others. It's like a complex game of seesaw on a molecular scale!

Mathematically speaking, this relationship is expressed as \(\frac{pV}{T}\) = constant.

Alright, but there's a catch! The constant from our combined gas law is not just a random number, but is proportional to the amount of the gas (n). This gives us a new and spiced-up equation:

\(\frac{pV}{T}\) = nR, where R is the superstar known as the Universal Gas Constant. Rewriting this, we get:

💡Ideal Gas Equation: pV = nRT

Here, R is the 'Universal Gas Constant'. Its value and units change depending on the units used for p, V, T, and n.

If we decide to go full geek mode 🤓 and use standard SI units (p in Pascal [Pa], V in cubic meters [m³], T in Kelvin [K], and n in moles [mol]), R would be approximately 8.31 Joules per Kelvin per mole (J K⁻¹ mol⁻¹).