An experiment shows that a 248-mL gas sample has a mass of 0.433 g at a pressure of 745 mm Hg and a temperature of 28°C. What is the molar mass of the gas?

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Answer 1 · 2018-05-31T07:04:31

$"Molar mass"~=100*g*mol^-1$

$PV=nRT="mass"/"molar mass"RT$

And thus $"molar mass"=(RT)/(PV)$

And so here.... $"molar mass"=(0.0821*(L*atm)/(K*mol)xx301.1*K)/((745*mm*Hg)/(760*mm*Hg*atm^-1)xx0.248*L)$

$=??*g*mol^-1$

The key idea of this problem was the recognition that $760*mm*Hg-=1*atm$ ...and thus a unit of length was proportional to a unit of pressure....