Based on the following chemical equation 4HCN + 5O₂ 2N₂ + 4CO₂ + 2H₂O
Identify the limiting reactant and the mass of N₂ produced when 100.0 g of HCN react with 100.0 g of O₂.

Question

Based on the following chemical equation 4HCN + 5O₂ 2N₂ + 4CO₂ + 2H₂O Identify the limiting reactant and the mass of N₂ produced when 100.0 g of HCN react with 100.0 g of O₂.

Quizplus · Accepted Answer

To identify the limiting reactant, we need to calculate the number of moles of each reactant using their molar masses. Molar Mass HCN = 1(1.008) + 1(12.01) + 1(14.01) = 27.03 g/mol Number of moles HCN = 100.0 g / 27.03 g/mol = 3.70 mol Molar Mass O₂ = 5(16.00) + 2(32.06) + 11(14.01) = 254.25 g/mol Number of moles O₂ = 100.0 g / 254.25 g/mol = 0.39 mol Next, we need to compare the mole ratio of HCN and O₂ in the balanced equation with the mole ratio of the two reactants we just calculated. Mole ratio HCN:O₂ = 4:5 Mole ratio calculated from given amounts = 3.70 mol HCN : 0.39 mol O₂ = 9.49 : 1 Since the mole ratio calculated from the given amounts is different from the ratio in the balanced equation, we know that one of the reactants is limiting. The limiting reactant is the one that produces a smaller amount of product. Using the mole ratio of HCN:O₂ = 4:5, we can calculate the theoretical yield of N₂ if all of the limiting reactant is consumed. 4 moles HCN produces 2 moles N₂ 3.70 mol HCN produces (2/4) x 3.70 = 1.85 mol N₂ 5 moles O₂ produces 2 mol N₂ 0.39 mol O₂ produces (2/5) x 0.39 = 0.156 mol N₂ Since 0.156 mol is smaller than 1.85 mol, O₂ is the limiting reactant. We can now use the mole ratio based on the balanced equation to calculate the actual yield of N₂. 5 mol O₂ produces 2 mol N₂ 0.39 mol O₂ produces (2/5) x 0.39 = 0.156 mol N₂ Mass of N₂ = 0.156 mol x 254.25 g/mol = 39.7 g Therefore, the answer is B, the limiting reactant is O₂ and 35.0 g of N₂ are produced.

Based on the Following Chemical Equation 4HCN + 5O2

Based on the Following Chemical Equation 4HCN + 5O₂