State and explain ideal gas law?

Part: 1: Ideal Gas Law:

• The relationship between the pressure $\mathrm{P}$, volume $\mathrm{V}$, and temperature $\mathrm{T}$ of gas in the limit of low pressures and high temperatures, such that the molecules of the gas move practically independently of one other, is known as the ideal gas law.
• In this situation, all gases satisfy a state equation known as the ideal gas law:
• $\mathrm{PV}=\mathrm{nRT}$
• Where $\mathrm{n}$ represents the number of moles of gas and $\mathrm{R}$ represents the universal (or perfect) gas constant, $8.31446261815324\mathrm{J}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$.
• The universal gas constant is defined as ${\mathrm{N}}_{\mathrm{A}}$ i.e., Avogadro's number multiplied by the Boltzmann constant$\mathrm{k}$.

Part: 2: Ideal gases are hypothetical gases made up of molecules that adhere to a few rules:

• The ideal gases do neither attract nor repel one another.
• Ideal gas themselves take up no volume.