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Preparation of Hydrogen from Cold Water and Metals

In the follow...

Question

In the following reaction, at $S T P$ , how many liters of $S O_{2}$ will require to burn completely a pure sulfur in $8$ litres of oxygen?
$S (s) + O_{2} (g) \to S O_{2} (g)$

1

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4

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8

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16

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32

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Solution

The correct option is C $8$
The balanced chemical reaction is $S (s) + O_{2} (g) \to S O_{2} (g)$
1 mole of $S$ reacts with 1 mole of $O_{2}$ to form 1 mole of $S O_{2}$ .
Volume at $S T P$ is directly proportional to the number of moles.
Hence, 8 mole of $S$ reacts with 8 mole of $O_{2}$ to form 8 mole of $S O_{2}$ .

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. . . S O_{2} (g) + . . . . O_{2} (g) \to . . . S O_{3} (g)

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