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

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14.66, 6.0

24.0, 12.0

12.0, 6.0

14.66 , 18.0

answer is B.

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Detailed Solution

We know,
$C_{6} H_{12} O_{6} + 6 O_{2} \to 6 C O_{2} + 6 H 2 O$
Moles of 10g of glucose
$= \frac{W e i g h t o f g l u \cos e}{M o l e c u l a r m a s s o f g l u \cos e}$
$= \frac{10}{(12 \times 6 + 12 + 16 \times 6)} = \frac{10}{180} = \frac{1}{18} m o l e s$
From above reaction 1 mole of glucose produces 6 moles of CO₂.
$∴$ 1/18 moles of glu cos e produce
$\begin{array}{l} = \frac{1}{18} \times 6 moles of {CO}_{2} \\ = \frac{1}{3} moles of {CO}_{2} \end{array}$
$\begin{aligned} ∴ Weight of {CO}_{2} = NO of moles of {CO}_{2} \\ \times Molecular mass of {CO}_{2} \end{aligned}$
$\begin{aligned} = \frac{1}{3} \times (12 + 16 \times 2) \\ = \frac{1}{3} \times 44 = 14.66 g \end{aligned}$
Similarly, 1 mole of glucose produces 6 moles of H₂O
So, 1/18 moles of glu cose produce of H₂O × Molecular mass of H₂O
$= \frac{1}{3} \times 18 = 6 g$
Thus, the masses of CO₂ and H₂respectively are 14.66 g and 6 g.