One and a half mole of oxygen combine with al | vedclass

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Question

(D) The balanced chemical equation is: $4Al + 3O_2 \rightarrow 2Al_2O_3$From the stoichiometry of the reaction,$3$ moles of $O_2$ react with $4$ moles

Vedclass · Accepted Answer

$54$

Vedclass · Answer

(D) The balanced chemical equation is: $4Al + 3O_2 ightarrow 2Al_2O_3$From the stoichiometry of the reaction,$3$ moles of $O_2$ react with $4$ moles of $Al$.The molar mass of $Al$ is $27 \ g/mol$,so $4$ moles of $Al$ weigh $4 	imes 27 = 108 \ g$.Since $3$ moles of $O_2$ react with $108 \ g$ of $Al$,then $1.5$ moles of $O_2$ will react with:$\frac{108 \ g}{3 \ mol} 	imes 1.5 \ mol = 36 	imes 1.5 = 54 \ g$ of $Al$.

One and a half mole of oxygen combine with aluminium to form $Al_2O_3$,then the weight of aluminium metal used in this reaction is ............. $g$ (Atomic weight of $Al = 27$)

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