An organic compound contains 40% carbon and 6.66% hydrogen. $11.2 l$ of the vapors of that substance weigh 30 g. What is the molecular formula of the compound?

C_{2} H_{4} O_{2}

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C_{3} H_{4} O_{2}

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C_{4} H_{8} O_{2}

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C_{2} H_{4} O

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Solution

The correct option is A $C_{2} H_{4} O_{2}$
According to given data,
Element %

Atomic ratio
Simple ratio
Carbon 40

$\frac{40}{12} = 3.33$
$\frac{3.33}{3.33} = 1$
Hydrogen 6.66

$\frac{6.66}{1} = 6.66$
$\frac{6.66}{3.33} = 2$
Oxygen 53.34

$\frac{53.34}{16} = 3.33$
$\frac{3.33}{3.33} = 1$
$E m p . f o r m u l a = C H_{2} O$
$V . D o f c o m p o u n d = 30, M . W t = 60$
$M o l . f o r m u l a = E m p . f o r m u l a \times \frac{60}{30}$
$= C H_{2} O \times 2$
$= C_{2} H_{4} O_{2}$

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Similar questions

11.2 l

40

C

6.66

H

53.34

O

C H_{2} O

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