0.219 g of salicylic acid and 0.676 mL of acetic anhydride (d = 1.082 g/mL) react in the presence of an acid catalyst to produce acetylsalicylic acid. Determine the limiting reagent and then calculate the theoretical yield of the product in grams. Report the theoretical yield to three decimal places.

If you were to use 6.00 g salicylic acid and an excess of acetic anhydride in the synthesis of aspirin, what would be the theoretical yield of acetylsalicylic acid in moles? In grams? Show your solution.

Given the balanced reaction between salicylic acid (C7H603) and acetic anhydride (C4H603) to produce ASA or acetylsalicylic acid (C9H804) and acetic acid (C2H4O2), the following experimental materials are provided: 5.00 g of pure salicylic acid, 7.14 g of acetic anhydride and 8 drops concentrated sulfuric acid as catalyst. After successful synthesis, the group was able to collect 5.25 grams of acetylsalicylic acid. (Atomic weights: C= 12 amu; H = 1 amu; O= 16 amu; density acetic anhydride = 1.08 g/mL). How much of the EXCESS reagent is left unused after the reaction? O 0.37 g O 1.31 g O 3.45 g O 3.69 g O None of the above %3D

What is the theoretical oxygen demand in liters of air for a 50 mg/L solution of acetone, C3H6O to decompose completely? Show the solution. Balanced chemical equation: C3H6O + 4O2→3CO2 + 3H2O Molecular Mass, g/mol: C3H6O = 58.08 O2 = 32 Assume that 1 L of air contains 0.21 L of O2 gas