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At $300 k$ and 1 atmospheric pressure $10 m l$ of a hydrocarbon required $55 m L$ of $O_{2}$ for complete combustion and $40 m L$ of ${C O}_{2}$ is formed. The formula of the hydrocarbon is

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$C_{4} H_{8}$

$C_{4} H_{7} C l$

$C_{4} H_{6}$

$C_{4} H_{10}$

answer is A.

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Detailed Solution

balanced chemical reaction

$C_{x} H_{y} + (x + \frac{y}{4}) O_{2} \to {x C O}_{2} + \frac{y}{2} H_{2} O$

$10 10 (x + \frac{y}{4}) 10 x$

According to the given data = $10 (x + \frac{y}{4}) = 55$ ---------------------(I)

10 x=40 ---------------(II)

After solving these two equations we get the value of x =4 and y = 6.

So, the formula of compound $C_{4} H_{6}$ .

Therefore, option A is correct.

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