1. Calculate the number of moles in: a. 1.00 g of salicylic acid 1.00g x 1mol / 138.13g = 0.0072 moles C7H6O3: 84.07 + 6.06 + 48.00 = 138.13 g per mol salicylic acid b. 3.0 mL of acetic acid anhydride 3.0mL = 3 g 3 g x 1 mole / 102.1 g = 0.029 mol C4H6O3: 48.04 + 6.06 + 48.00 = 102.1 g/mol 2. Using Equation 8.1 and the following tables, determine the number of moles of aspirin produced from: a. Salicylic acid Moles of Salicylic Acid Mass of Acetylsalicylic Acid b. Acetic anhydride Moles of Acetic Anhydride Mass of Acetylsalicylic Acid 3. The limiting reagent is the reactant that produces the smallest amount of aspirin. The smallest amount of product that can be produced from the available reactants is called the theoretical yield. What is the theoretical yield of this reaction? Limiting Reagent Theoretical Yield of Acetylsalicylic Acid
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Calculate the number of moles of salicylic acid in 1.00 g. The molar mass of salicylic acid (C7H6O3) is 138 g/mol. Number of moles = mass / molar mass Number of moles of salicylic acid = 1.00 g / 138 g/mol = 0.007246 mol Show more…
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Madhur L.
Salicylic Acid + Acetic Anhydride ---> Acetylsalicylic Acid + Acetic Acid C7H6O3 + C4H6O3 -----> C9H8O4 + C2H4O2 1. What is the limiting reagent and the theoretical yield of the above reaction if 1.00 g of salicylic acid is reacted with 1.00 mL of acetic anhydride? 2. If 0.82 g of aspirin were obtained in the reaction, what is the percent yield? 3. If the percent yield of the reaction is reported as 76.8%, how much salicylic acid is required to isolate 1.00 g of aspirin? 4. If 0.100 mol of salicylic acid is reacted with 2.2 molar equivalents of acetic anhydride, how much acetic anhydride, in mL, should be added to the reaction vessel?
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