# A 0.5090*g mass of gas exerts a pressure of 746*mm*Hg, and occupies a volume of 0.1294*L at a temperature of 364*K? What is its molecular mass?

Apr 17, 2017

$\text{Molecular mass} \le 120 \cdot g \cdot m o {l}^{-} 1$

#### Explanation:

From the Ideal Gas Equation:

$n = \frac{P V}{R T}$

i.e. $\text{mass"/"molar mass} = \frac{P V}{R T}$

i.e. "molar mass"=("mass"xxRT)/(PV)

$= \frac{0.5090 \cdot g \times 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1 \times 364 \cdot K}{\frac{746 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t {m}^{-} 1} \times 0.1294 \cdot L}$

??*g*mol^-1