Mass of pure aspirin expected: Mass of crude aspirin obtained: Percent yield in crude product = 2.72 = g Mass of crude product obtained Mass of pure product expected x 100 2.72 2.61 2.61 g = 104.2 % x 100 = Give an alternative method of synthesis of aspirin, using salicylic acid as a stating material. Give the mechanism.

Mass of pure aspirin expected: Mass of crude aspirin obtained: Percent yield in crude product = 2.72 = g Mass of crude product obtained Mass of pure product expected x 100 2.72 2.61 2.61 g = 104.2 % x 100 = Give an alternative method of synthesis of aspirin, using salicylic acid as a stating material. Give the mechanism.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 32QAP: When yeast is added to a solution of glucose or fructose, the sugars are said to undergo...

See similar textbooks

Similar questions

On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation, and ethyl alcohol is produced. :math>C6H12O6(aq)2C2H5OH(aq)+2CO2(g) is is the reaction by which wines arc produced from grape juice. Calculate the mass of ethyl alcohol, C2H5OH. Produced when 5.25 g of glucose, C6H12O6, undergoes this reaction.
ce Carrington -STOICHIOMET X wer.html?state=%7B"ids"%3A%5B"1J1faQoGnmRQnPpCs1180ZWUfe Z8de9E"%5D%2C'action"%3A'open"%2 Carrington - STOICHIOMETRY WORKSHEET#1.doc 3. How many formula units of CuCI can be produced by 75.0 g of Cu O? Cu20 + HCI → CuCl + H2O 4. If 35.0 g of oxygen gas is produced by the following reaction, how many liters of hydrogen gas are produced? H2O → H2 + O2
Mass of Na2CO3=5g Mass of CaCl2=4.98g Mass of filter paper=1.11g Na2CO3 and CaCl2 combined, filtered, and dried overnight. The mass of the solid produced = 2.86g Calculate the theoretical yield of solid expected and the percent yield obtained.
Data and Calculations Don't forget units when recording your values! 33.00g Mass of baking soda (NaHCO:) Mass of the dry NaC;H:O: 3H:0 crystals 13.92g Description of the appearance of the NaCHO 3H:O crystals theoretical yield, in Use the mass of NaHCO, (from the data and calculations section) to calculate moles, of NaCH,Oz 3H;0. The theoretical yield of NaC:H;Oz in moles, using the stoichiometry of Reaction 1, is equal to the theoretical yield of the hydrate. moles Theoretical yield of NaC;H;O: 3H:0 136.0779 g/mol What is the molar mass of NaC2HOz 3H20? What is theoretical yield of NaC H:O; 3H;0 in grams? Calculate the percent yield using the following formula: (Mass of dry NaC,H,02 3H20 crystalsy 100% Theoretical yield of NaC,H302 3H,0 8.
Calculation of AH; of Magnesium Oxide Mg + 2 HCI MgCl2 * Hz2 AH, = kJ/mole MgCl2 +H2O > Mgo + 2 HCI -AH2 = kJ/mole He + 를 O2 + H2O AH3 = - 286 kJ/mole net: Mg + 을 O2- MgO 사Hnet = kJ/mole The literature value for the AHf of magnesium oxide is -602 kJ/mole.
An essentially 100% yield is necessary for a chemicalreaction used to analyze a compound, but it is almostnever expected for a reaction that is used to synthesizea compound. Explain this difference
Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: SCa + V;0; - 5Cao - 2V In one process, 1.540 x 10g of V;Og react with 1.970 x 10'g Ca. (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if S07.0 g of V are obtained. Report your answers to the correct number of significant figures.