How many moles of potassium chlorate (KClO_3) | vedclass

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Question

(D) The balanced chemical equation for the thermal decomposition of potassium chlorate is:$2KClO_3(s) \rightarrow 2KCl(s) + 3O_2(g)$From the stoichiom

Vedclass · Accepted Answer

$2/3 	ext{ mole}$

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(D) The balanced chemical equation for the thermal decomposition of potassium chlorate is:$2KClO_3(s) ightarrow 2KCl(s) + 3O_2(g)$From the stoichiometry of the reaction, $2 	ext{ moles}$ of $KClO_3$ produce $3 	ext{ moles}$ of $O_2$.At $STP$, $1 	ext{ mole}$ of any ideal gas occupies $22.4 	ext{ L}$.Therefore, $22.4 	ext{ L}$ of $O_2$ corresponds to $1 	ext{ mole}$ of $O_2$.Using the mole ratio: $\frac{2 	ext{ moles } KClO_3}{3 	ext{ moles } O_2} = \frac{x 	ext{ moles } KClO_3}{1 	ext{ mole } O_2}$.Solving for $x$: $x = \frac{2}{3} 	ext{ moles}$ of $KClO_3$.

How many moles of potassium chlorate $(KClO_3)$ must be heated to produce $22.4 \text{ L}$ of oxygen gas at $STP$?

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