Which of the following gases get released when dilute sulphuric acid (H SO ) reacts with magnesium (Mg)?

Question

Accepted Answer

Step-by-step explanation:

1. Write the reaction: magnesium reacts with dilute sulfuric acid to give a salt and hydrogen gas:

$\mathrm{Mg + H_2SO_4 \rightarrow MgSO_4 + H_2 \uparrow}$

2. Oxidation–reduction view: magnesium is oxidized to $\mathrm{Mg^{2+}}$ and $\mathrm{H^+}$ ions from the acid are reduced to hydrogen gas:

$\mathrm{Mg \rightarrow Mg^{2+} + 2e^-}$

$\mathrm{2H^+ + 2e^- \rightarrow H_2}$

Hence $\mathrm{H_2}$ is evolved.

3. Why the others are not formed:
- $\mathrm{SO_2}$ or $\mathrm{SO_3}$ would arise only if sulfuric acid itself were reduced/oxidized under special (usually hot or concentrated) conditions or with strong reducing agents — not in the normal reaction of a metal with dilute acid.
- $\mathrm{O_2}$ is not produced in this simple displacement reaction.

Therefore only gas (4) $\mathrm{H_2}$ is evolved, which corresponds to option d.

FINAL_ANSWER: d

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