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The masses of carbondioxide and water (in g) respectively formed during complete combustion of $10 \mathrm{~g}$ of glucose at STP are
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$14.66,6.0$
$\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6+6 \mathrm{O}_2, \stackrel{\mathrm{STP}}{\longrightarrow} 6 \mathrm{CO}_2+6 \mathrm{H}_2 \mathrm{O}$
Thus, 1 mole of glucose gives 6 moles of $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$. $\Rightarrow 180 \mathrm{~g}$ of glucose gives $6 \times 44=264 \mathrm{~g}$ of $\mathrm{CO}_2$ and $6 \times$ $18=108 \mathrm{~g}$ of $\mathrm{H}_2 \mathrm{O}$.
$\Rightarrow 10 \mathrm{~g}$ of glucose will give $\frac{264}{18}=14.66 \mathrm{~g}$ and $\frac{108}{18}$ $=6 \mathrm{~g}$ of $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ respectively.
Thus, 1 mole of glucose gives 6 moles of $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$. $\Rightarrow 180 \mathrm{~g}$ of glucose gives $6 \times 44=264 \mathrm{~g}$ of $\mathrm{CO}_2$ and $6 \times$ $18=108 \mathrm{~g}$ of $\mathrm{H}_2 \mathrm{O}$.
$\Rightarrow 10 \mathrm{~g}$ of glucose will give $\frac{264}{18}=14.66 \mathrm{~g}$ and $\frac{108}{18}$ $=6 \mathrm{~g}$ of $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ respectively.
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