At 300 K and 1 atmsopheric pressure, 10 mL of a hydrocarbon required 55 mL of O_{2}

for complete combustion, and 40 mL of CO_{2}  is formed. The formula of the hydrocarbon is:

Answers (1)

C_{x} H_{y}+\left(x+\frac{y}{4}\right) O_{2} \rightarrow x C O_{2}+\frac{y}{2} H_{2} O$ \\ \\ $\begin{array}{ll}\text { 10 } & \text { 10 }\left(x+\frac{y}{4}\right)\end{array} \quad 10 x$


By given data, 10\left(x+\frac{y}{4}\right)=55 \quad$..(1) 
10 x=40$\\ $\therefore x=4, y=6 \Rightarrow C_{4} H_{6}$

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