When a $0.216\,\text{g}$ sample of an aluminium compound $X$ is reacted with water present in excess, one hydrocarbon gas is produced. That gas undergoes complete combustion in $\text{O}_2$, giving only $\text{H}_2\text{O}$ and $\text{CO}_2$. The volume of $\text{CO}_2$ measured at room temperature and pressure is $108\,\text{cm}^3$. What formula does $X$ have?
- A$\text{Al}_2\text{C}_3$
- B$\text{Al}_3\text{C}_2$
- C$\text{Al}_3\text{C}_4$
- D$\text{Al}_4\text{C}_3$