A flask holds a mixture of 6.41 g of calcium carbide (64.10 g/mol) and 2.88 g of aluminium carbide…

A flask holds a mixture of $6.41\ \text{g}$ of calcium carbide ($64.10\ \text{g/mol}$) and $2.88\ \text{g}$ of aluminium carbide ($143.96\ \text{g/mol}$). Excess water is added: $\text{CaC}_{2} + 2\text{H}_{2}\text{O} \to \text{Ca}(\text{OH})_{2} + \text{C}_{2}\text{H}_{2}$ and $\text{Al}_{4}\text{C}_{3} + 12\text{H}_{2}\text{O} \to 4\text{Al}(\text{OH})_{3} + 3\text{CH}_{4}$. Take $22.4\ \text{L/mol}$ at $273\ \text{K}$ and $1\ \text{atm}$, and $78.00\ \text{g/mol}$ for aluminium hydroxide. Find the volumes of acetylene and of methane, and the mass of aluminium hydroxide that forms.