A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 degrees C and a pressure of 753 mmHg. What is the molar mass of the gas?

Nov 18, 2017

We solve the Ideal Gas equation......and we know that $1 \cdot a t m$ will support a column of mercury that is $760 \cdot m m$ high.....

i.e. $1 \cdot a t m \equiv 760 \cdot m m \cdot H g$

Explanation:

$n = \frac{P V}{R T} = \text{Mass"/"Molar mass}$

And thus $\text{Molar mass"=(RT)/(PV)xx"mass}$

(0.0821*(L*atm)/(K*mol)xx358.1*Kxx0.555*g)/((753*mm*Hg)/(760*mm*Hg*atm^-1)xx0.117*L)=??*g*mol^-1....