Question #261173

The rate of effusion of a particular gas was measured to be 24.0 mL /min. Under the same conditions the rate of effusion of pure methane gas, CH4 is 47.8 mL/min. What is the molar mass of the unknown gas?



1
Expert's answer
2021-11-05T00:57:52-0400

The rate of effusion of two gases is inversely proportional to the square root of their masses:


Rate1Rate2=M2M1\frac{Rate1}{Rate2}=\frac{\sqrt {M2}}{\sqrt {M1}}

The molecular weight of M1,CH4, is 16.04g/mol

Squaring both sides, you get:


M2M1=[Rate1Rate2]2\frac{M2}{M1}=[\frac{Rate 1}{Rate2}]^2


M2=M1×[Rate1Rate2]2=16.04×[47.824.0]2=63.63g/molM2=M1×[\frac{Rate1}{Rate2}]^2=16.04×[\frac{47.8}{24.0}]^2 = 63.63g/mol


Molecular weight of unknown gas =63.63g/mol


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