A $0.20 \cdot g$ $0.20g$ mass of gas occupies a $0.200 \cdot L$ $0.200L$ volume at one atmosphere, and $300 \cdot K$ $300*K$ . What is the molar mass of the gas?

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Answer 1 · 2017-03-26T18:49:19

$Molar mass$ $"Molar mass"$ $=$ $=$ $24.6 \cdot g \cdot m o l^{- 1}$ $24.6*g*mol^-1$

We use the Ideal Gas Equation.......

$P V = n R T$ $PV=nRT$

And thus $n = \frac{Mass}{Molar Mass} = \frac{P V}{R T}$ $n="Mass"/"Molar Mass"=(PV)/(RT)$

And so, $Molar Mass = \frac{Mass \times R T}{P V}$ $"Molar Mass"=("Mass"xxRT)/(PV)$

$=(0.20*gxx0.0821*cancelL*cancel(atm)*cancel(K^-1)*mol^-1xx300*cancelK)/(1*cancel(atm)xx0.200*cancelL)$

$=24.6*g*mol^-1$ . I think this is dimensionally correct, however, it does not correspond to a gas I can think of right now.........

A 0.20*g0.20⋅g0.20*g mass of gas occupies a 0.200*L0.200⋅L0.200*L volume at one atmosphere, and 300*K300⋅K300*K. What is the molar mass of the gas?