Question 27 of 29>Aspirin can be sunthesized in the lab by combining salicylic acid (C,H0) and acetic anhydride (C,H O3) to form aspirin(C,H O4) and acetic acid (C, H2O2). The balanced equation for this reaction isC,HO3 +CHO3CHO4+CH,026A student started with 4.48 mL acetic anhydride (density= 1.08 g/mL) and 1.59 g salicylic acid. The student synthesized1.62 g of aspirin.Select the limiting reactant.acetic acid (C2H402)aspirin (C,HgO)O salicylic acid (C,H03)acetic anhydride (C4H03)Calculate the the oretical yield of aspirin (C,HO4)theoretical yield:helpcontact usterms of useprivacy policyabout uscareers A student started with 4.48 mL acetic anhydride (density1.08 g/mL) and 1.59 g salicylic acid. The student synthesized1.62 g of aspirin.Select the limiting reactant.acetic acid (C2H02)Oaspirin (C,H,O4)Osalicylic acid (C,HO3)O acetic anhydride (C4H O3)Calculate the theoretical yield of aspirin (C,H O4)theoretical yield:Calculate the percent yield for aspirin (C,H,O4)%percent yield:helpcontact usterms of useprivacy policyabout uscareers1:232

The reactant that limits the amount of product that is being completely used in the reaction is…

Answered: Question 27 of 29> Aspirin can be…

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem 12RE

See similar textbooks

Similar questions

C9H8O4 is synthesized by reacting stoichiometric amounts of C7H6O3 and (CH3CO)2O, as shown by the balanced chemical equation in the picture: During the synthesis, 500 grams of salicylic acid was available for use in the experiment. Other Details: MW of Salicylic Acid: 138.121 g/mol MW of Acetic Anhydride: 102.09 g/mol Density of Acetic Anhydride: 1/08 g/ml Question: (1) Calculate how many moles of Salicylic acid are available for use in the reaction and (2) assuming that there will be a 75% yield in the experiment, how many grams of Aspirin will be produced?
The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 5 mol NaHCO3 and 8 mol HCl.
1. Oxygen bleach acts in the release of oxygen which best works in hot water mixture. Which of the following bleach or its derivative could be a potential for oxygen bleaching? -OCl- NaOH NaOCl -O²- H2O2 2. In the production of ceramic, silicon carbide and silicon dioxide are being reacted at high temperature. In the process, carbon monoxide is also produced. After the reaction of 100.0 kg of silicon dioxide, 51.4 kg of SiC is obtained. Determine the percent yield of silicon carbide.
The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 33 mol NaHCO3 and 77 mol HCl.HCl. moles of carbonic acid : ____________________mol Which of the two reactants limits the number of moles of H2 CO3 that can be made? 1. HCl 2. NaHCO3 How much excess reactant remains after the reaction? excess reactant : ___________________mol
The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3)(NaHCO3) reacting with one mole of hydrochloric acid (HCl)(HCl) to produce one mole of carbonic acid (H2CO3),(H2CO3), and one mole of sodium chloride (NaCl).(NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 22 mol NaHCO3NaHCO3 and 88 mol HCl.HCl. moles of carbonic acid : mol Which of the two reactants limits the number of moles of H2CO3H2CO3 that can be made? HClHCl NaHCO3NaHCO3 How much excess reactant remains after the reaction? excess reactant : mol
Alkenes react with hydrogen - produce the corresponding alkane hydrogenation - produce margarine Decene Decane C10H20(liquid) +H2(g) ---- C10H22(s) What is the % yield od decane if the actual yield of the product produced was 34.0g? a decene is in excess and there is 2.00g of hydrogen in the reaction. _______-- %
Lysine is an amino acid which has the following elemental composition: C, H, O, N. In one experiment, 2.175g of lysine was combusted to produce 3.94g CO2 and 1.89 H2O . In a seperate experiment, 1.873g of lysine was burned to produce 0.463g NH3. The molar mass of lysine is approximately 150g/mol. Determine the empirical and molecular formula of lysine.
Dinitrogen tetroxide, N2O4 is an important component of rocket fuels. At 25 ℃, N2O4(92.01 g/mol) partially dissociates into NO2 (46.01 g/mol). In an experiment, 7.64 g N2O4and 1.56 g NO2 were placed in a 3-L reaction vessel. Construct a balanced equation anddeduce the value of Kc for this chemical reaction
How many moles of C4H8O2are in 6.00 g of butyric acid?
Determine the limiting and excess reactants in the following problems. Show complete soultions. 1. Given 25 g of hydrochloric acid and 5o grams of Na2SO4 2HCL + Na2SO4 --- 10CO2 + 12H2O
In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their re-search efforts to develop renewable sources of carbon-basedfuels. For more than a decade, Brazil has been engaged in aprogram to replace gasoline with ethanol derived from the rootcrop manioc (cassava).(a) Write separate balanced equations for the complete combus-tion of ethanol (C₂H₅OH) and of gasoline (represented by theformula C₈H₁₈).(b) What mass of oxygen is required to burn completely 1.00 Lof a mixture that is 90.0% gasoline (d=0.742 g/mL) and 10.0%ethanol (d=0.789 g/mL) by volume?(c) If 1.00 mol of O₂ occupies 22.4 L, what volume of O₂ isneeded to burn 1.00 L of the mixture?(d) Air is 20.9% O₂ by volume. What volume of air is needed toburn 1.00 L of the mixture?
plant photosynthesis sugars and oxygen from carbon dioxide and water are shown 6co2+6h2o=c6h12o6+o6 calculate %yield of 1.24g of c6h12o6 are produced by reaction of 1.24of cp2. the molar mass is 44.01g and the molar mass of c6h12o6 is 180.2g

SEE MORE QUESTIONS

Recommended textbooks for you

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781285199030

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS