A student is recrystallizing 2.034 g of acetylsalicylic acid (aspirin) that was isolated from 8.00 grams of Excedrin. The recrystallization requires a seed crystal to begin. The seed crystal weighs 0.389 g. The student's actual yield after recrystallization is 1.663 g. What is the percent recovery?

A student is recrystallizing 2.034 g of acetylsalicylic acid (aspirin) that was isolated from 8.00 grams of Excedrin. The recrystallization requires a seed crystal to begin. The seed crystal weighs 0.389 g. The student's actual yield after recrystallization is 1.663 g. What is the percent recovery?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 120IL

See similar textbooks

Similar questions

A student crystallizes 1.8 g of benzoic acid and isolate 0.5 g as the first crop. What is the percent recovery in this first crop?
2. Mass of dibenzalacetone= 2.698g Mass of Benzaldehyde = 2.98g moles of dibenzalacetone 2.698g/(234.29g/mol)=0.01152 mol moles of benzaldehyde 2.98g/(106.13g/mol)=0.02808 mol What is the theoretical yield? What is the yield percentage?
The combustlon of propane (C,H,) In the presence of excess oxygen ylelds CO, and H,0 as shown below. C,H, (g) + 50, (95→ 3Co, (g) + 4H,0 (g) When 2.5 mol of O, are consumed in this reaction, mol of CO, are produced. O 2.5 1.5 O 5.0 O3.0
Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9 H8O4) and acetic acid (C₂H4O₂). The balanced equation is C4H6O3 + C7H6O3 → C9H8O4 + C₂H4O2 In a laboratory synthesis, a student begins with 5.96 mL of acetic anhydride (density = 1.08 g/ml) and 2.23 g of salicylic acid. Once the reaction is complete, the student collects 1.76 g of aspirin. Determine the limiting reactant for the reaction. O acetic anhydride Osalicylic acid Submit Part B Correct m = Determine the theoretical yield of aspirin for the reaction. Express your answer in grams to three significant figures. VE ΑΣΦΑ Submit Previous Answers Part C Submit Request Answer Determine the percent yield of aspirin for the reaction. Express the percentage to three significant figures. 15. ΑΣΦ Request Answer ? ? % g
Na2CO3 (aq) + CaCl2 (aq) —> CaCO3 (s) +2NaCl (aq) Mass of Na2CO3 =1.118g Mass of CaCl2= 1.381g Mass of precipitate obtained from the experiment =0.9591g 1) what is the mass of excess reagent left unreacted 2) calculate the theoretical yield(in grams) and the percent yield of the experiment.
The hydrated salt, MY3·xH2O, was heated strongly in a crucible to remove all the water molecules of crystallization. The data for this experiment are given in the table below.Mass of empty crucible and cover 28.86 gMass of crucible, cover, and hydrated salt 32.86 gMass of crucible, cover, and anhydrous salt 31.24 gMolar mass of anhydrous salt 238.03 g/mol (i) Calculate the % composition by mass of water in the hydrated salt. (ii) Determine the value of x. (iii) M is in Period 4 of the Periodic Table of the Elements.If Y = NO3– , identify the element M.
I would need help answering this question with the steps please
Balance the following chemical equation (ifnecessary):C6H6O(I) + O2(g) -> H20 (g) + CO2 (g)
An organic compound found in many kinds of fruit (apples, bananas, melons, cherries, and strawberries). It is added as an artificial flavoring to some foods and drinks to create sweet, fruity flavors. When combustion analysis was carried out on a 2.50g sample of this ester produces 6.10g of CO2 and 2.50g of H2O. If the molar mass of this compound is 144.21g, what is the molecular formula of this compound?
A local water retention pond was found to have elevated levels of mercury concentrated as 14 ng per liter. You would like to collect some mercury for your homemade perpetuum mobile machine. How many moles of mercury can you get you collect and process the entire volume of 1250 m3 of the water in the pond?
Acetyl Salicylic acid is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H6O3 based on the following equation: C7H6O3 + C4H6O3 → C9H8O4 + C2H4O2 SA AA ASA The theoretical yield of ASA was determined to be 1.95 g. The actual yield of acetyl salicylic acid, C9H8O4, is 1.54 g. What is the percent yield? A. 83.6 % B. 78.8 % C. 69.2 % D. 52.3 %
3 - Sulfur – yellow powder with a strong and somewhat unpleasant odor has anti-inflammatory, astringent, detoxifying and disinfectant properties. In addition to these benefits, sulfur has been used to treat skin problems for a long time and remains a valuable ingredient in skin care products, especially soaps. The determination of the sulfur concentration in a soap sample was performed by burning 3.130 mg of crushed sample producing an amount of SO3. The SO3 produced was collected in water and completely converted to H2SO4. The acid formed was titrated with a 0.01530 mol L^-1 NaOH solution using 2.15 mL. Calculate the % (w/w) of S in the soap sample. Data: O = 16.00 S= 32.07 H = 1.008 %3D