For this problem we will use the ideal gas law:
[tex]\begin{gathered} PV=nRT \\ P:pressure(atm) \\ V:volume(L) \\ n:number\text{ }of\text{ }moles\text{ }of\text{ }gas \\ R:ideal\text{ }gas\text{ }constant(0.082Latmmol^{-1}K^{-1}) \\ T:absolute\text{ }temperarture(K)=273.15K+80.4\degree C=353.55K \end{gathered}[/tex]We will substitute the known values into this equation to determine the number of moles:
[tex]\begin{gathered} n=\frac{PV}{RT} \\ \\ n=\frac{3.85atm\times32.4L}{0.082Latmmol^{-1}K^{-1}\times353.55K} \\ \\ n=4.30mol \end{gathered}[/tex]Answer: 4.3 mol of gas.
