A gaseous hydrocarbon gives upon combustion, $0.72 g$ water and $3.08 g$ of $C O_{2}$ . The empirical formula of the hydrocarbon is:

C_{6} H_{5}

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C_{7} H_{8}

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C_{2} H_{4}

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C_{3} H_{4}

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Solution

The correct option is B $C_{7} H_{8}$
C $_{x} H_{y}$ +( $x + \frac{y}{4}) O_{2}$ $\to$ $x C O_{2}$ + $\frac{y}{2} H_{2}$ O

Moles of $H_{2} O = \frac{0.72}{18} = 0.04$

Moles of CO $_{2} = \frac{3.08}{44} = 0.07$

$\frac{y}{2} = 0.04 \times 100$ or $y = 8$ , $x = 0.07$ $\times 100 = 7$

Empirical formula is $C_{7} H_{8}$

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Similar questions

A gaseous hydrocarbon gives upon combustion 0.72 g. of water and 3.08 g. of CO₂. The empirical formula of the hydrocarbon is:

0.72

3.08

C O_{2}

A gaseous hydrocarbon gives upon combustion 0.72 g. of water and 3.08 g. of CO₂. The empirical formula of the hydrocarbon is:

{C O}_{2}

H_{2} O

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