What is the mass of KClO_{3(s)} required to l | vedclass

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(B) The balanced chemical equation for the thermal decomposition of potassium chlorate is: $2 KClO_{3(s)} \longrightarrow 2 KCl_{(s)} + 3 O_{2(g)}$Fro

Vedclass · Accepted Answer

$81.67$

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(B) The balanced chemical equation for the thermal decomposition of potassium chlorate is: $2 KClO_{3(s)} \longrightarrow 2 KCl_{(s)} + 3 O_{2(g)}$From the stoichiometry,$2 	ext{ moles}$ of $KClO_3$ produce $3 	ext{ moles}$ of $O_2$.$2 	ext{ moles}$ of $KClO_3 = 2 	imes 122.5 \ g = 245 \ g$.$3 	ext{ moles}$ of $O_2$ at $STP$ occupy $3 	imes 22.4 \ dm^3 = 67.2 \ dm^3$.Thus,$245 \ g$ of $KClO_3$ produces $67.2 \ dm^3$ of $O_2$.To find the mass $(x)$ required to produce $22.4 \ dm^3$ of $O_2$:$x = \frac{245 \ g 	imes 22.4 \ dm^3}{67.2 \ dm^3} = 81.67 \ g$.

What is the mass of $KClO_{3(s)}$ required to liberate $22.4 \ dm^3$ of oxygen at $STP$ during thermal decomposition (in $g$)? (Molar Mass of $KClO_{3(s)} = 122.5 \ g/mol$)

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