10 mL of a gaseous hydrocarbon requires 25 mL of O2 for complete combustion and produces 20 mL of CO2 (all volumes at the same temperature and pressure, water as liquid). The hydrocarbon is

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$10 mL$ of a gaseous hydrocarbon requires $25 mL$ of $O X_{2}$ for complete combustion and produces $20 mL$ of $CO X_{2}$ (all volumes at the same temperature and pressure, water as liquid). The hydrocarbon is

C X_{x} H X_{y} + (x + \frac{y}{4}) O X_{2} x CO X_{2} + (\frac{y}{2}) H X_{2} O (l)

. By Avogadro's law volume ratios equal mole ratios.

x = 20/10 = 2

x + y /4 = 25/10 = 2.5

, so

y /4 = 0.5

and

y = 2

. The hydrocarbon is

C X_{2} H X_{2}