Question

Equivalent weights of two oxides $A$ and $B$ of sulphur are $16$ and $13.33g$ $equivalen{t}^{-1}$ respectively. What are these oxides?

• A. $A$ is $S{O}_2$
• B. $B$ is $S{O}_3$
• C. Both A and B
• D. None of them

Answer 1

The correct option is C Both A and B

As we know, Equivalent mass is the mass of element which reacts with 8 g of oxygen.
Here,
16 g sulphur reacts with 8 g oxygen
Let $A$ be$S_x{O}_y$
$B$ be $S_p{O}_q$
In $A$, $16yg$ oxygen$\equiv (32x+16y)g$ $S_x{O}_y$
hence, $8g$ oxygen $\equiv \frac{32x+16y}{2y}=16$(given)
$\frac{32x}{y}+8=16$
$\frac{x}{y}=\frac{1}{2}=\frac{numberofSatom}{numberofOatom}$
Thus, $A$ is $S{O}_2$
In $B$, $16qg$ oxygen$\equiv (32p+16q)g$ $S_p{O}_q$
$8g$ oxygen$\equiv \frac{32p+16q}{2q}=13.33$ (given)
$\frac{16p}{q}=5.33$
$\frac{p}{q}=\frac{5.33}{16}=\frac{1}{6}=\frac{numberofSatom}{numberofOatom}$
Thus, $B$ is $S{O}_3$