Question

A gaseous mixture is composed of equal number of moles of CH4, C2H6 and C2H2. Determine the
average molecular mass of mixture (in amu).
​

Answer 1

Answer:

effective weight = sum of weigths in equimolar ratio / 2

= 23.

therefore weigth of 2.27 litres = (23*2.27)/22.4

Explanation:

Answer 2

We know that,

The average molecular mass $=\frac{Total \ mass }{Total\ moles}$

Let the total number of moles be x.

Hence, the weight of $CH_4$ =$x\times \ molar\ mass= x\times 16= 16x$

Hence, the weight of $C_2H_6$ =$x\times \ molar\ mass= x\times 30= 30x$

Hence, the weight of $C_2H_2$ =$x\times \ molar\ mass= x\times 26= 26x$

Total mass=$16x+30x+26x=72x$

Therefore average mass =$\frac{72x}{x+x+x}=\frac{72x}{3x}=24$

So, average molecular mass of the mixture is 24 amu.

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