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$5.6 g of an organic compound on burning with excess of oxygen gave 17.6 g of {CO}_{2} and 7.2 {gH}_{2} O . The$ organic compound is

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$C_{6} H_{6}$

$C_{4} H_{8}$

$C_{3} H_{8}$

${CH}_{3} COOH$

answer is B.

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Detailed Solution

$\begin{array}{l} % of carbon = \frac{12 \times wt {of CO}_{2}}{44} \times \frac{100}{W} \\ % H= \frac{2 \times Wt {of H}_{2} O}{18} \times \frac{100}{W} \end{array}$ then find empirical formula

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