Concept explainers
(a)
Interpretation: for the given reaction, the mass of salicylic acid required to produce 0.400g of aspirin, the mass of salicylic acid required to produce 0.400g of aspirin if the 74.9% salicylic acid is converted to aspirin and the percent yield of 10.9g of aspirin if 9.26g of salicylic acid reacts with 8.54g of acetic anhydride are needed to be determined.
Concept introduction:
- Balanced chemical equation of a reaction is written according to law of conservation of mass.
- Equation for Number of moles of a substance, from its given mass is,
- Percent yield of reaction is the ratio of mass of actual yield to the mass of theoretical yield and multiplied with hundred.
(b)
Interpretation: for the given reaction, the mass of salicylic acid required to produce 0.400g of aspirin, the mass of salicylic acid required to produce 0.400g of aspirin if the 74.9% salicylic acid is converted to aspirin and the percent yield of 10.9g of aspirin if 9.26g of salicylic acid reacts with 8.54g of acetic anhydride are needed to be determined.
Concept introduction:
- Balanced chemical equation of a reaction is written according to law of conservation of mass.
- Equation for Number of moles of a substance, from its given mass is,
- Percent yield of reaction is the ratio of mass of actual yield to the mass of theoretical yield and multiplied with hundred.
(c)
Interpretation: for the given reaction, the mass of salicylic acid required to produce 0.400g of aspirin, the mass of salicylic acid required to produce 0.400g of aspirin if the 74.9% salicylic acid is converted to aspirin and the percent yield of 10.9g of aspirin if 9.26g of salicylic acid reacts with 8.54g of acetic anhydride are needed to be determined.
Concept introduction:
- Balanced chemical equation of a reaction is written according to law of conservation of mass.
- Equation for Number of moles of a substance, from its given mass is,
- Percent yield of reaction is the ratio of mass of actual yield to the mass of theoretical yield and multiplied with hundred.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Chemistry: Atoms First
- Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.arrow_forwardMany over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.arrow_forwardBillions of pounds of urea, CO(NH2)2, are produced annually for use as a fertilizer. The principal reaction employed is: 2NH3+CO2CO(NH2)2+H2O By assuming unlimited amounts of CO2, how many moles of urea can be produced from each of the following amounts of NH3? a.2molNH3b.0.45molNH3c.10gNH3d.2.0kgNH3arrow_forward
- Barium chloride solutions are used in chemical analysis for the quantitative precipitation of sulfate ion from solution. :math>Ba2+(aq)+SO42(aq)BaSO4(s) ppose a solution is known to contain on the order of 1 50 mg of sulfate ion. What mass of barium chloride should be added to guarantee precipitation of all the sulfate ion?arrow_forwardBacterial digestion is an economical method of sewage treatment. The reaction is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate ions. What mass of bacterial tissue is produced in a treatment plant for every 1.0 104 kg of wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium ions are consumed by the bacteria.arrow_forwardThe pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.arrow_forward
- Calculate the molarity of solutions prepared by dilution or calculate the quantities needed to carry out a dilution to prepare a solution of a specified concentration.arrow_forward3.122 What type of reasoning were we using when we developed the equation for dilution, MiVi=MfVf ?arrow_forwardFig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.arrow_forward
- Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.arrow_forwardMethanol, CH3OH, is used in racing cars because it is a clean-burning fuel. It can be made by this reaction: CO(g)+2H2(g)CH3OH(l) What is the percentage yield if 5.0103gH2 reacts with excess CO to form 3.5104gCH3OH ?arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning