The masses of carbon dioxide and water (in g) respectively formed during complete combustion of 10 g of glucose at STP are.

We know,
$C_6{H}_{12}{O}_6+6O_2\to 6C{O}_2+6H2O$          
Moles of 10g of glucose
$=\frac{Weightofglu\cos e}{Molecularmassofglu\cos e}$
$=\frac{10}{(12\times 6+12+16\times 6)}=\frac{10}{180}=\frac{1}{18}moles$
From above reaction 1 mole of glucose produces 6 moles of CO₂.
$\therefore$ 1/18 moles of glu cos e produce
$\begin{array}{l}=\frac{1}{18}\times 6\text{ moles of }{\mathrm{CO}}_2\\ =\frac{1}{3}\text{ moles of }{\mathrm{CO}}_2\end{array}$
$\begin{array}{r}\therefore \text{ Weight of }{\mathrm{CO}}_2=\text{ NO of moles of }{\mathrm{CO}}_2\\ \times \text{ Molecular mass of }{\mathrm{CO}}_2\end{array}$
$\begin{array}{r}=\frac{1}{3}\times (12+16\times 2)\\ =\frac{1}{3}\times 44=14.66g\end{array}$
Similarly, 1 mole of glucose produces 6 moles of H₂O
So, 1/18 moles of glu cose produce of H₂O × Molecular mass of H₂O
$=\frac{1}{3}\times 18=6g$
Thus, the masses of CO₂ and H₂ respectively are 14.66 g and 6 g.