# Question 931a5

Nov 9, 2016

The density of the gas at given temperature and pressure

$= \text{mass of gas"/"volume of the gas"=3.45/1.85" g/L"=1.865" g/L}$

By equation of state for ideal gas we know

$P V = \frac{w}{M} R T$

Where

$P \to \text{pressure} = 1.05 a t m$

$V \to \text{volume} = 1.85 L$

$T \to \text{temperature} = 49 + 273 = 322 K$

$R \to \text{ideal gas constant} = 0.082 L a t m {K}^{-} 1 m o {l}^{-} 1$

M->"molar mass of the gas"=?#

$M = \frac{w R T}{P V} = \frac{3.45 \times 0.082 \times 322}{1.05 \times 1.85} = 46.9 g m o {l}^{-} 1$