Question

0.32 g of metal gave on treatment with an acid 112 mL of hydrogen at NTP. Calculate the equivalent weight of the metal:

• A. 58
• B. 32
• C. 11.2
• D. 24

Answer 1

The correct option is B 32

Given,

Mass of metal=$0.32g$

Volume of hydrogen=$112ml$

$=112\times {10}^{-3}L$

Now we know,

Equivalent Weight of metal is the mass of metal required to produce $1gm$ of Hydrogen $⟶\left(1\right)$

Now, We know $1$ mole of hydrogen= $22.4L$ of $H_2$

$\Rightarrow$ If $0.32g$ Metal produces $112\times {10}^{-3}L$ of $H_2$

$\therefore$ Mass of mass metal required to produce $11.2L$ of $H_2$

$[\because 1gm{H}_2=11.2L$ of $H_2]=\frac{0.32\times 11.2}{112\times {10}^{-3}}=32gm$

$\therefore$ From (1) Equivalent weight of metal= $32gm$