When a hydrocarbon A undergoes complete combustion it requires 11 equivalents of oxygen and produces 4 equivalents of water. What is the molecular formula of A?

Let the hydrocarbon be $$C_xH_y$$. The balanced combustion reaction is:

$$ C_xH_y + \left(x + \frac{y}{4}\right)O_2 \rightarrow xCO_2 + \frac{y}{2}H_2O $$

Given: 11 equivalents of oxygen and 4 equivalents of water.

From water: $$\frac{y}{2} = 4 \implies y = 8$$

From oxygen: $$x + \frac{y}{4} = x + \frac{8}{4} = x + 2 = 11 \implies x = 9$$

The molecular formula is $$C_9H_8$$.

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