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An organic compound contains $69 %$ carbon and $4.8 %$ hydrogen, the remainder being oxygen. What will be the masses of carbondioxide and water produced when 0.2 g of this substance is subjected to complete combustion?

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0.345 g and 0.024 g

0.91 g and 0.72 g

0.69 g and 0.048 g

0.506 g and 0.086 g

answer is B.

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Detailed Solution

$% C = \frac{12}{44} \times \frac{mass of {CO}_{2}}{mass of substance} \times 100$

$69 = \frac{12}{44} \times \frac{mass of {CO}_{2}}{0 .2} \times 100$

$Mass of {CO}_{2} = \frac{69 \times 44 \times 0 .2}{12 \times 100} = 0 .506 g$

$% H = \frac{2}{18} \times \frac{mass of H_{2} O}{mass of substance} \times 100$

$4 .8 = \frac{2}{18} \times \frac{mass of H_{2} O}{0 .2} \times 100$

$mass of H_{2} O = \frac{4 .8 \times 18 \times 0 .1}{100} = 0 .086 g$

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