34.05 mL of phosphorus vapour weighs 0.0625 g at 546 ∘ C and 0.1 bar pressure. What is the molar mass of phosphorus?

Explanation

We are given that
`V = 34.05 mL = 34.05 xx 10^(-3)L`
m=0.0625g
`T= 546^(@)C = 546^(@)C = 546 +273=819K`
p=0.1 bar
We are to calculate the molar mass of phosphorus.
We know that
pV=nRT
`0.1 xx 34.05 xx 10^(-3) = (0.0625)/(M) xx 0.0821 xx 819`
`M=(0.0625 xx 0.0821 xx 819)/(0.1 xx 34.05 xx 10^(-3)) = 1247.7g`