Answer:
The molar mass of the gas is 44.19 g/mol
Explanation:
Amount of sample of gas = m = 13.5 g
Volume occupied by the gas = V = 5.10 L
Pressure of the gas = P = 149.83 KPa
1 KPa = 0.00986 atm
P = [tex]149.83 \textrm{ KPa} \times 0.00986 \textrm{ atm/KPa} = 1.48 \textrm{ atm}[/tex]
Assuming M g/mol to be the molar mass of the gas
Assuming the gas is behaving as an ideal gas
[tex]\textrm{PV} =\textrm{nRT} \\\textrm{PV} = \displaystyle \frac{m}{M}\textrm{ RT } \\1.48 \textrm{ atm}\times 5.10 \textrm{ L} = \displaystyle \frac{13.5 \textrm{ g}}{M}\times 0.0821 \textrm{ L.atm.mol}^{-1}.K^{-1}\times 301\textrm{K} \\M = 44.19 \textrm{ g/mol}[/tex]
The molar mass of gas is 44.19 g/mol
