Question

A metal m forms a volatile chloride containing 65.5% chlorine. if the density of the chloride relative to hydrogen is 162.5, find the molecular formula of the chloride.

Answer 1

$M_2Cl_6$ is the desired formula of Chloride

Step-by-step explanation:

Percentage of Cl = 65.5%

Percentage of metal = 100- 65.5 = 34.5 %

So the empirical formula of chloride= $MCl_3$

Empirical Formula mass = 162.5 gm

Vapour density = 162.5  

molecular mass = 2(VD)= 325

n = empirical mass molecular mass = 2

n = $\frac {empirical\ mass}{molecular\ mass} = 2$

So. the Molecular formula = $(MCl_3)_2= M_2Cl_6$

Answer 2

As we know,

Molar mass = 2 x vapour density

2×162.5=325g

Mass of Cl in compound =0.655×325=213g

Mass of metal =325−213=112g

So, compound is

M2 Cl6