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
- A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?arrow_forwardMany 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_forwardOn 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?arrow_forward
- ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.arrow_forwardWhat is the difference between a solute and a solvent?arrow_forwardYou want to prepare a 1.0 mol/kg solution of ethyleneglycol, C2H4(OH)2, in water. Calculate the mass of ethylene glycol you would need to mix with 950. g water.arrow_forward
- 39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.arrow_forwardThe 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.arrow_forwardWhen 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.arrow_forward
- Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.arrow_forward4-89 If 7.0 kg of is added to 11.0 kg of to form which reactant is in excess?arrow_forwardAqueous solutions of ammonium sulfide and mercury(II) nitrate react and a precipitate forms. (a) Write the overall balanced chemical equation and indicate the state (aq) or (s) for each compound. (b) Name each product. (c) Write the complete ionic equation. (d) Write the net ionic equation.arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning