This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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To solve this problem, we first need to determine the molar masses of the reactants and products, then calculate the moles of each reactant to find the limiting reactant, and finally use the limiting reactant to calculate the theoretical yield and percent yield. The balanced chemical equation is: C_7H_6O_3 + (CH_3CO)_2O → C_9H_8O_4 + CH_3COOH (Salicylic acid) + (Acetic anhydride) → (Aspirin) + (Acetic acid) Molar masses: • Salicylic acid (C_7H_6O_3): (7 × 12.01) + (6 × 1.008) + (3 × 16.00) = 84.07 + 6.048 + 48.00 = 138.118 g/mol • Acetic anhydride ((CH_3CO)_2O or C_4H_6O_3): (4 × 12.01) + (6 × 1.008) + (3 × 16.00) = 48.04 + 6.048 + 48.00 = 102.088 g/mol • Aspirin (C_9H_8O_4): (9 × 12.01) + (8 × 1.008) + (4 × 16.00) = 108.09 + 8.064 + 64.00 = 180.154 g/mol a) Which is the limiting reactant? Step 1: Calculate the moles of salicylic acid. Moles of salicylic acid = massmolar mass = 3.0779 g138.118 g/mol = 0.022284 mol Step 2: Calculate the mass of acetic anhydride using its density and volume. Mass of acetic anhydride = density × volume = 1.080 g/mL × 5.050 mL = 5.454 g Step 3: Calculate the moles of acetic anhydride. Moles of acetic anhydride = massmolar mass = 5.454 g102.088 g/mol = 0.053426 mol Step 4: Determine the limiting reactant. From the balanced equation, the stoichiometric ratio between salicylic acid and acetic anhydride is 1:1. Since 0.022284 mol (salicylic acid) is less than 0.053426 mol (acetic anhydride), salicylic acid is the limiting reactant. The limiting reactant is salicylic acid. Salicylic acid b) What is the percent yield of this reaction? Step 5: Calculate the theoretical yield of aspirin. Based on the balanced equation, 1 mole of salicylic acid produces 1 mole of aspirin. Moles of aspirin (theoretical) = moles of limiting reactant = 0.022284 mol Theoretical yield of aspirin = moles × molar mass = 0.022284 mol × 180.154 g/mol = 4.0148 g Step 6: Calculate the percent yield. Percent yield = actual yieldtheoretical yield × 100\% Percent yield = 3.281 g4.0148 g × 100\% = 81.72\% The percent yield of this reaction is 81.72%. 81.72\% Send me the next one 📸