We will use the Ideal Gas Law:
[tex]\begin{gathered} PV=nRT \\ P:pressure\text{ }measured\text{ }in\text{ }atm \\ V:volume\text{ }in\text{ }L \\ n:moles\text{ }of\text{ }gas\text{ }present \\ R:gas\text{ }contant\text{ }that\text{ }converts\text{ }to\text{ }0.082Latmmol^{-1}K^{-1} \\ T:temperature\text{ }in\text{ }K \end{gathered}[/tex]
We will substitute the given values into the formula to determine the unknown:
[tex]\begin{gathered} n=\frac{PV}{RT} \\ n=\frac{4.88\text{ }atm\times166\text{ }L}{0.082Latmmol^{-1}K^{-1}\times220.8K} \\ n=44.74\text{ }moles \end{gathered}[/tex]
Moles of the ideal gas is 44.74.
