# An impure sample of sugar is burnt and it gives 134.4 L of carbon dioxide at STP. If the sample weighs 513 g, what is the % purity of the sample?

$C_{12}H_{22}O_{11} + 12O_{2} \rightarrow 12CO_{2} +11H_{2}O$

By Dalton's Atomic Theory, the atoms are neither created nor destroyed

$\therefore$ moles of  $C_{12}H_{22}O_{11}$

$\\*= \frac{1}{12}\times (moles\;of\;CO_{2}) \\*= \frac{1}{12}\times \frac{134.4}{22.4} \\*= \frac{1}{12}\times 6 = 0.5$

molar mass of  $C_{12}H_{22}O_{11}$ = 513g

% purity = $\frac{0.5\times513}{mass\;of\;sample} = \frac{0.5\times513}{513}\times 100 = 50\%$

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