Aspirin can be prepared from salicylic acid (C7H6O3 ), which has a molar mass of 138.12g/mol, and acetic anhydride (C4H,O3 ), whichhas a molar mass of 102.04 g/mol. The densityof acetic anhydride is 1.082 g/mL.C7H6O3 + C4H, O3→ C9H3 O4 + C2H4O2What is the theoretical yield, in grams, of aspirin (C9H3O4), which has a molar mass of 180.15g/mol, possible when reacting 3.25 g of salicylicacid with 3.56 mL of acetic anhydride?

Answered: Image /qna-images/answer/8a30f32f-c78d-461e-b0a3-4cd616a6036a.jpg

Aspirin can be prepared from salicylic acid ( C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride ( C4H6O3 ), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C7H6O3 + C4H;O3 → C9H8O4 + C2H4O2 What is the theoretical yield, in grams, of aspirin ( C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.25 g of salicylic acid with 3.56 mL of acetic anhydride?

Aspirin can be prepared from salicylic acid ( C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride ( C4H6O3 ), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C7H6O3 + C4H;O3 → C9H8O4 + C2H4O2 What is the theoretical yield, in grams, of aspirin ( C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.25 g of salicylic acid with 3.56 mL of acetic anhydride?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter1: The Nature Of Chemistry

Section: Chapter Questions

Problem 127QRT

See similar textbooks

Similar questions

Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
When corn is allowed to ferment, the fructose in the corn is converted to ethyl alcohol according to the following reaction C6H12O6(aq)2C2H5OH(l)+2CO2(g)(a) What volume of ethyl alcohol (d=0.789g/mL) is produced from one pound of fructose? (b) Gasohol can be a mixture of 10 mL ethyl alcohol and 90 mL of gasoline. How many grams of fructose are required to produce the ethyl alcohol in one gallon of gasohol?
Swimming pool water is often made safe for swimming by treating with chlorine in the form of sodium hypocholrite (NaOCI) solution. If a swimming pool contains 5.62×10^5L of water, what volume of 5.00% NaOCI (by mass) solution is required to produce a sodium hypoclorite concentrarion of 3.00×10^-7 mol /L? (assuume the density of water and the NaOCI solution is 1.00g/ml). Do not give handwriting solution.
A certain solution is 4.40% by mass in calcium carbonate (CaCO3) if the density of the solution is 1.02 g/mL, what mass (in grams) of calcium carbonate is contained in 53.3mL of solution?
Fingernail–polish remover is primarily acetone (C3H6O).How many acetone molecules are in a bottle of acetone witha volume of 325 mL? (density of acetone = 0.788 g/cm3)
DNA crystals are 0.144nm^3. What is the volume in milliliters?
Qs/ A 0.2121-g sample of pure Na,C,0, (134.00 g/mol) was t ed with 43.31 mL of KMnO;. What is the normality of the KMnO, solution? The chemical reac- tion is 2MnOj; + 5C,0i + 16H* — 2Mn?* + 10CO, + 8H,O
You wish to prepare 213 grams of 17.4% (w/w) NaI. Assume that the density of water is 1.00 g/mL. You will need grams of sodium iodide and mL of water.
As part of the aspirin synthesis lab the orgo students also had to perform the following calculation to demonstrate their knowledge. Are you able to help them work this out? Saponification is a process in which soap is produced from the chemical reaction between animal fat (triglycerides) and a strong base such as KOH. An example of such balanced chemical reaction is shown here: C51H98O6 + 3KOH → C3H5(OH)3 + 3C16H31O2K (Triglyceride) (Soap) if during the saponification reaction 231.5 g of C51H98O6 is mixed with 231.5 g of KOH and 160 g of soap is produced. Calculate the theoretical yield of soap C16H31O2K and indicate who is the limiting reactant. (Provide your answer to 2 decimal places) Calculate the percent yield for this reaction (Provide your answer to 1 decimal place) *Show ALL steps and mathematical equations involved in your calculations to help the orgo students. Remember to label all…
A solution of sodium hydroxide has a density of 1.14 g/mL and contains 32.8% sodiumhydroxide by mass. If 40.0 mL of this solution is diluted with 30.0 mL of water, what is theconcentration of the dilute sodium hydroxide?
A certain solution is 5.84 % by mass in calcium carbonate (CaCO3). If the density of the solution is 1.02 g/mL, what mass (in grams) of calcium carbonate is contained in 46.4 mL of solution? (3 sf)