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Ideal Gas Equation

The molecular...

Question

The molecular weights of oxygen and sulphur dioxide are $32$ and $64$ respectively. If $1$ litre of oxygen at $15^{o}$ C and $740$ mm pressure contains $N$ molecules, the number of molecules in $2$ litre of sulphur dioxide under the same conditions of temperature and pressure will be:

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Solution

By using Avogadro Law,
$V \propto n$ at constant pressure & temperature
Thus, $\frac{V_{O_{2}}}{V_{S O_{2}}} = \frac{n_{O_{2}}}{n_{S O_{2}}}$
$\Rightarrow \frac{1 L}{2 L} = \frac{N / N_{A}}{n_{S O_{2}}}$
$\Rightarrow n_{S O_{2}} = \frac{2 N}{N_{A}}$
Thus, molecules of $S O_{2}$ is $2 N$ .

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