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(B) The electrolysis of water is represented by the balanced chemical equation:$2 H_2 O (l) \rightarrow 2 H_2 (g) + O_2 (g)$From the stoichiometry of

Vedclass · Accepted Answer

$5.0$

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(B) The electrolysis of water is represented by the balanced chemical equation:$2 H_2 O (l) \rightarrow 2 H_2 (g) + O_2 (g)$From the stoichiometry of the reaction,$2 \ mol$ of water produces $1 \ mol$ of oxygen gas.The molar mass of water $(H_2 O)$ is $18 \ g/mol$.Number of moles of water in $180 \ g$ is:$n(H_2 O) = \frac{180 \ g}{18 \ g/mol} = 10 \ mol$According to the stoichiometry,$2 \ mol$ of $H_2 O$ produces $1 \ mol$ of $O_2$.Therefore,$10 \ mol$ of $H_2 O$ will produce:$n(O_2) = \frac{10 \ mol}{2} = 5 \ mol$Hence,the correct option is $B$.

Number of moles of oxygen gas evolved by electrolysis of $180 \ g$ of water?

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