34.05 mL of phosphorus vapour weighs 0.0625g at 546^(@)C` and 0.1 bar pressure. What is the molar mass of phosphorus?

Explanation

Suppose, the molar mass of phosphorus`=Mg*mol^(-1)`
So, 0.0625g of phosphorus`=(0.0625)/(M)mol` of phosphorus
As given, P=0.1 bar, T=(273+546)K=819K,
V=34.05mL=`34.05xx10^(-3)L`
therefore, 0.1 bar`xx34.05xx10^(-3)L`
`=(0.0625)/(M)mol xx0.082L*bar*mol^(-1)*K^(-1)xx819K`
or, `M=1232.71`, hence molar mass`=1232.71g*mol^(-1)`