Question

The oxide of an element contains $67.67$% oxygen and the vapour density of its volatile chloride is $79$. Equivalent weight of the element is :

• A. $2.46$
• B. $3.82$
• C. $4.36$
• D. $4.96$

Answer 1

Answer: (B)

$3.82$

100 g of the oxide will contain 67.67 g of oxygen and 32.33 g of the element.

Equivalent weight of an element is its weight which reacts with 8 gm of oxygen to form oxide.

67.67 g of oxygen combines with 32.33 g of the element to form oxide.

1 g of oxygen will combine with $\frac{32.33}{67.67}$ g of element to form oxide.

8 g of oxygen will combine with $8\times \frac{32.33}{67.67}=3.82$ g of element to form oxide.

Hence, the equivalent weight of the element is 3.82.