The volume of hydrogen liberated at STP by treating 2.4 g of magnesium with excess of hydrochloric acid is _______ $$\times 10^{-2}$$ L. Given Molar volume of gas is 22.4 L at STP. Molar mass of magnesium is 24 g mol$$^{-1}$$

Correct Answer: 224

The reaction: $$\text{Mg} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2$$

Moles of Mg = $$\frac{2.4}{24} = 0.1$$ mol

Moles of H$$_2$$ = 0.1 mol (1:1 ratio)

Volume at STP = $$0.1 \times 22.4 = 2.24$$ L = $$224 \times 10^{-2}$$ L

Create a FREE account and get:

Predict your JEE Main percentile, rank & performance in seconds

Check Your Score Now

Ask our AI anything

AI can make mistakes. Please verify important information.

Download resources