In the reaction, 2Al_{(s)} + 6HCl_{(aq)} righ | vedclass

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(B) The balanced chemical equation is: $2Al_{(s)} + 6HCl_{(aq)} \rightarrow 2Al^{3+}_{(aq)} + 6Cl^{-}_{(aq)} + 3H_{2(g)}$.From the stoichiometry, $2 \

Vedclass · Accepted Answer

$33.6 \ L \ H_{2(g)}$ at $STP$ is produced for every mole of $Al$ that reacts.

Vedclass · Answer

(B) The balanced chemical equation is: $2Al_{(s)} + 6HCl_{(aq)} ightarrow 2Al^{3+}_{(aq)} + 6Cl^{-}_{(aq)} + 3H_{2(g)}$.From the stoichiometry, $2 \ 	ext{moles of } Al$ produce $3 \ 	ext{moles of } H_{2(g)}$.Therefore, $1 \ 	ext{mole of } Al$ produces $\frac{3}{2} = 1.5 \ 	ext{moles of } H_{2(g)}$.At $STP$, $1 \ 	ext{mole of any gas occupies } 22.4 \ L$.So, $1.5 \ 	ext{moles of } H_{2(g)} = 1.5 	imes 22.4 \ L = 33.6 \ L \ H_{2(g)}$.Thus, $33.6 \ L \ H_{2(g)}$ at $STP$ is produced for every mole of $Al$ that reacts.

In the reaction, $2Al_{(s)} + 6HCl_{(aq)} \rightarrow 2Al^{3+}_{(aq)} + 6Cl^{-}_{(aq)} + 3H_{2(g)}$, which of the following statements is correct?

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