# An 0.846*g mass of gas exerts a pressure of 752*"Torr", and expresses a volume of 354*mL, at a temperature of 100 ""^@C. What is the molar mass of the gas?

$\text{Mass"/"Molar mass} = \frac{P \times V}{R \times T}$; from where did I get this relationship?
And thus "Molar mass"=(RxxTxx"mass")/(PxxV)
$= \frac{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 373 \cdot K \times 0.846 \cdot g}{\left(752 \cdot \text{Torr")/(760*"Torr} \cdot a t {m}^{-} 1\right) \times 0.354 \cdot L}$
$\cong 74 \cdot g \cdot m o {l}^{-} 1$