Question

In the reaction,
$2H_{2}S+S{O}_2\to 2H_{2}O+3S$
1 mol each of $S{O}_2$ and $H_{2}S$ will give how much sulphur?

• A. 1 mol
• B. 3 mol
• C. 1.5 mol
• D. 2 mol

Answer 1

The correct option is A 1 mol

$2H_{2}S+S{O}_2⟶2H_{2}O+3S$

$1$ $1$ $0$ $0$

Here, $H_{2}S$ is limiting reagent, because it will be exhausted completely in the reaction.

As, $2$ $moles$ of $H_{2}S$ produce $3$ $mole$ of sulphur. $1$ $mole$ of $H_{2}S$ produce $1.5$ $mole$ of sulphur.