Given the reaction 2Al + 3CuCl2 → 2AlCl3 + 3Cu, if 10.5 g of CuCl2 react with 12.4 g of Al, what is the limiting reactant?

• A. CuCl2
• B. Neither reactant is limiting
• C. Al
• D. Both reactants are limiting

Answer: (A)

Verified step by step guidance

1. Write down the balanced chemical equation: \$2Al + 3CuCl_2 \rightarrow 2AlCl_3 + 3Cu$.
2. Calculate the molar masses of the reactants: Molar mass of \(CuCl_2\) and molar mass of \(Al\).
3. Convert the given masses of each reactant to moles using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
4. Use the mole ratio from the balanced equation to determine the amount of product each reactant can produce or how much of the other reactant is needed.
5. Compare the mole ratios to identify which reactant is completely consumed first; this reactant is the limiting reactant.