Question

$1\text{g}$ of a metal on treatment with a dilute mineral acid gave $896\text{mL}$ of hydrogen at STP. Calculate the equivalent weight of the metal.

• A. 12.5 g
• B. 8.9 g
• C. 10.2 g
• D. 14.23 g

Answer 1

The correct option is A 12.5 g

$22400\text{mL}$ of hydrogen gas at STP weighs $2\text{g}$ at STP.
$896\text{mL}$ of the gas at STP will weigh = $=\frac{2}{22400}\times 896=0.08\text{g}$

$\frac{\text{weight of the metal}}{\text{weight of hydrogen}}=\frac{\text{equivalent weight of the metal}}{\text{equivalent weight of hydrogen}}$

$\Rightarrow \frac{1}{0.08}=\frac{M}{1}$

On solving, $M=12.5\text{g}$