Question

A solid element burns completely in oxygen to give gaseous oxide without any change in volume. if the vapour density of oxide is 32, the equivalent weight would be?

Answer 1

Molecular mass = 2 x vapour density.

So we get molecular mass is = 64.

$M\left(s\right)+O_2\left(g\right)⟶M{O}_2\left(g\right)$
1 mol 1 mol 1 mol

The molecular weight of gaseous oxide =2× vapour density

=2×32=64

∴ So the molar mass of M=64−2×16=32

So M should be Sulphur (S)

∴ The equivalent weight of S =$\frac{Molecularweight}{valency}$= $\frac{32}{4}=8$