0.32 gm of a metal on treatment with an acid gave 112mL of hydrogen at STP. Calculate the equivalent weight of the metal.

The correct option is 32.

Concept:
The equivalent weight of a metal is defined as the mass of the metal that displaces or reacts with 1 equivalent of another element. For hydrogen, 1 equivalent of hydrogen gas (_H2) has a mass of 1.008 g, which occupies a volume of 11200 mL (or 11.2 L) at Standard Temperature and Pressure (STP).

Therefore, we can calculate the equivalent weight of the metal using the relation:

$$\text{Equivalent weight of metal}=\frac{\text{Mass of metal (g)}}{\text{Volume of hydrogen at STP (mL)}}\times 11200$$

Given Data:
Mass of metal = 0.32 g
Volume of hydrogen gas displaced = 112 mL at STP

Step-by-Step Calculation:
Substitute the given values into the formula:

$$\text{Equivalent weight}=\frac{0.32}{112}\times 11200$$

Simplifying the expression:

$$\text{Equivalent weight}=0.32\times 100$$

$$\text{Equivalent weight}=32$$

Thus, the equivalent weight of the metal is 32.