Chemistry

posted by .

Calculate the theoretical yield of aspirin to be obtained in this experiment, starting with 2.0 g of salicylic acid and 5.0 ml of acetic acid anhydride (density = 1.08 g/ml).

  • Chemistry -

    Writ the equation for salicylic acid + acetic anhydride to produce ASA.

    This is a limiting reagent problem.
    2a. Convert 2.0 g salicylic acid to mols.
    2b. convert 5.0 mL to grams by density, then to mols.

    3. Convert to mols ASA (aspirin)
    a. Convert mols salicylic acid to mols ASA (1:1 ratio).
    b. Convert mols acetic anhydride to mols ASA (1:1 ratio).
    c. Choose the smaller number of mols ASA produced. The reagent producing this result is the limiting reagent.

    4. Convert mols ASA in 2c to grams. That is the theoretical yield.

    Post your work if you get stuck BUT tell me what you don't understand about the next step.

  • chem- please check my answer -

    (5.0ml)x(2.0g/1.08g/ml)x(1 mole S/138g S) x (1 mole Aspirin/1 mole S)x (180g Aspirin/ 1 mole Aspirin) = 12.077 g Aspirin

  • Chemistry -

    I don't get those numbers. Apparently you are using acetic anhydride as the limiting reagent. Unless I made a goof in my calculations, and I may have done that, salicylic acid is the limiting reagent. If you will show your calculations I can check it better.

  • Chemistry -

    3.42g

  • Chemistry -

    how did you get 3.42g?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemisty

    How to calculate the theoretical yield of aspirin to be obtained when 2.0 g of salicylic acid and 5.0 mL of acetic anhydride (density = 1.08 g/mL) are mixed together?
  2. AP Chemistry

    Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation is given below. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 (a) What mass of acetic anhydride is needed to completely consume …
  3. chemistry

    For the theoretical yield, I used the mass of acetic anhydride. Was I supposed to use the mass of salicylic acid (which was 2.00 g) instead?
  4. chemistry - synthesis of aspirin

    I wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid?
  5. chemistry - synthesis of aspirin

    wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid?
  6. chemistry - synthesis of aspirin

    This is an experiment for a synthesis of aspirin lab mass of salicylic acid = 2.005 g mass of acetic acid = ?
  7. chem

    Aspirin, C9H8O4, is produced from salicylic acid, C7H6O3, and acetic anhydride, C4H6O3: C7H6O3 + C4H6O3 --> C9H8O4 + HC2H3O2 a. How much salicylic acid is required to produce 1.5 x 10^2 kg of aspirin, assuming that all of the salicylic …
  8. chem

    Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3), and acetic anhydride (C4H6O3): C7H6O3 + C4H6O3 ¨ C9H8O4 + HC2H3O2 . (c) What is the theoretical yield of aspirin if 189 kg of salicylic acid is allowed to react with 128 …
  9. Chemistry

    Aspirin is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H603. The other product produced is acetic acid, C2H402. C7H6O3+C4H6)3->C9H8O4+C2H4O2 What is the theoretical yield in grams of aspirin, C9H8O4, when …
  10. chem

    A chemist is commissioned to produce twenty pallets of aspirin: C7H6O3 (salicylic acid) + C4H6O3 (acetic anhydride) → C9H8O4 (aspirin) +C2H4O2 (acetic acid) Given a bottle contains 500 tablets (each containing 325 mg of aspirin). …

More Similar Questions