Hydrogen, obtained by the electrical decomposition of water was combined with chlorine to produce $62.5$ g of hydrogen chloride. Calculate the mass (in g) of water decomposed ( rounded to the nearest integer).
$2 H_{2} O ⟶ 2 H_{2} + O_{2}$
$H_{2} + C l_{2} ⟶ 2 H C l$

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Solution

The reactions are as follows:
$2 H_{2} O ⟶ 2 H_{2} + O_{2}$
$H_{2} + C l_{2} ⟶ 2 H C l$
One mole of water produces $2$ moles of $H C l$ .
Hence, the mass of water decomposed to obtain $62.5$ g of $H C l$ is $\frac{18}{2 \times 36.5} \times 62.5 = 15$ g.

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