Chemistry, asked by BrainlyMonarch777, 3 months ago

$\large\sf1. \: O_{2} \: is \: evolved \: by \: heating \: KClO_{3} \\ \large\sf using \: MnO_{2} \: as \: a \: catalyst : \: \: \: \:$

$\bf 2KClO_{3} \: \xrightarrow{MnO_{2}} \: 2KCl + 3O_{2}$
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$\sf \small (i) \: \: Calculate \: the \: mass \: of \: KClO_{3} \: required \: to \\ \small \sf produce \: \: \: 6.72 \: \: litres \: of \: \: O_{2} \: at \: \: STP. \\ \\ \small \sf[atomic \: masses \: of \: K = 39, Cl = 35.5, \\ \small \sf O = 16]$
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$\small \sf(ii) \: Calculate \: the \: number \: of \: moles \: of \: oxygen \\ \small \sf present \: in \: the \: above \: volume \: and \: also \\ \small \sf the \: number \: of \: molecules.$

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Answered by Sisters5678

$\large\sf1. \: O_{2} \: is \: evolved \: by \: heating \: KClO_{3} \\ \large\sf using \: MnO_{2} \: as \: a \: catalyst : \: \: \: \:$

$\bf 2KClO_{3} \: \xrightarrow{MnO_{2}} \: 2KCl + 3O_{2}$

$\\$

$\sf \small (i) \: \: Calculate \: the \: mass \: of \: KClO_{3} \: required \: to \\ \small \sf produce \: \: \: 6.72 \: \: litres \: of \: \: O_{2} \: at \: \: STP. \\ \\ \small \sf[atomic \: masses \: of \: K = 39, Cl = 35.5, \\ \small \sf O = 16]$

$\\$

$\small \sf(ii) \: Calculate \: the \: number \: of \: moles \: of \: oxygen \\ \small \sf present \: in \: the \: above \: volume \: and \: also \\ \small \sf the \: number \: of \: molecules.$

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