Multiple Choice
What is the number of moles of oxygen atoms in 4.96 mol of H2O2?
3. Chemical Reactions
Stoichiometry
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When 2.50 mol of Al and 3.00 mol of Cl2 combine in the reaction 2Al(s) + 3Cl2(g) ⇌ 2AlCl3(s), how many moles of AlCl3 are formed?
A
1.50 mol
B
3.00 mol
C
2.00 mol
D
2.50 mol
Verified step by step guidance1
Identify the balanced chemical equation: 2Al(s) + 3Cl2(g) ⇌ 2AlCl3(s). This equation tells us that 2 moles of Al react with 3 moles of Cl2 to produce 2 moles of AlCl3.
Determine the limiting reactant by comparing the mole ratio of the reactants to the coefficients in the balanced equation. We have 2.50 mol of Al and 3.00 mol of Cl2.
Calculate the mole ratio for Al: (2.50 mol Al) / (2 mol Al) = 1.25. Calculate the mole ratio for Cl2: (3.00 mol Cl2) / (3 mol Cl2) = 1.00.
Identify the limiting reactant as the one with the smaller mole ratio. In this case, Cl2 is the limiting reactant because 1.00 < 1.25.
Use the limiting reactant to determine the amount of AlCl3 formed. Since 3 moles of Cl2 produce 2 moles of AlCl3, 3.00 mol of Cl2 will produce (3.00 mol Cl2) * (2 mol AlCl3 / 3 mol Cl2) = 2.00 mol of AlCl3.
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