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Stoichiometric Calculations

Al and KClO...

Question

$A l$ and $K C l O_{3}$ react together to form $A l_{2} O_{3}$ as follows:
$2 K C l O_{3} ⟶ 2 K C l + 3 O_{2}$
$4 A l + 3 O_{2} ⟶ 2 A l_{2} O_{3}$
$4$ moles of $K C l O_{3}$ ( $50 %$ pure) on reaction with excess of $A l$ forms x moles of $A l_{2} O_{3}$ . The value of x (as nearest integer) is:

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Solution

The reactions are as follows:
$2 K C l O_{3} ⟶ 2 K C l + 3 O_{2}$
$4 A l + 3 O_{2} ⟶ 2 A l_{2} O_{3}$
$4$ moles of $50 %$ pure $K C l O_{3}$ is provided which means actually $2$ moles are present.
According to the balanced reaction, $2$ moles of $K C l O_{3}$ forms $2$ moles of $A l_{2} O_{3}$ .

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