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ENGLISH 207
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Chemistry
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Dec 18, 2024
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5
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Graded AssignmentSCI303A/304A: Chemistry | Unit 6 | Lesson 13: Unit TestGraded AssignmentUnit Test, Part 2Answer the following questions. You may use the periodic table in the Chemistry: Problems and Solutions book for this test. When you have finished, submit this assignment to your teacher by the due date for full credit.(5 points)ScoreClick or tap here to enter text.Ibuprofen (C13H18O2) is the active ingredient in many nonprescription pain relievers. Each tablet contains 200 mg of ibuprofen, and a typical adult dose is two tablets every six hours.Determine the molar mass of ibuprofen (show your work).Calculate the number of moles of ibuprofen in a single tablet (show your work).Calculate the number of moles of ibuprofen that an adult would have taken if she took four doses of ibuprofen in one day (show your work).Answer:the molar mass of ibuprofen c13H18o^2 is 206g/molmolar mass of c13H18o2=(12x13)+(18x 1)+ (16x2)= 156+18+32=206g/mol© 2008 K12 Inc. All rights reserved.Page 1 of 5Copying or distributing without K12’s written consent is prohibited.
Graded AssignmentSCI303A/304A: Chemistry | Unit 6 | Lesson 13: Unit Testmolar mass of c13H18o2=206g/molmass of one tablet=200mg=200 X 10-3=0.2gmole= mass/molar massmole of one tablet =0.2/206one tablet = 200mga dose of ibuprofen=2 tablets=2 x 200=400mgfour dose=4 x 400=1600mg=1600x10^-2=1.6g© 2008 K12 Inc. All rights reserved.Page 2 of 5Copying or distributing without K12’s written consent is prohibited.
Graded AssignmentSCI303A/304A: Chemistry | Unit 6 | Lesson 13: Unit Testmolar mass of ibuprofen = 206g/molmolar=mass/molar massmole for one day= 1.6/206mole for one day=7.77x10^-3 mole(5 points)ScoreClick or tap here to enter text.Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid.Write a balanced equation for the reaction.Calculate the theoretical yield of sulfuric acid.Calculate the percent yield of the reaction.(One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)Answer:the balanced equation for the formation 2so2+o2+2H20 arrow 2H2s04© 2008 K12 Inc. All rights reserved.Page 3 of 5Copying or distributing without K12’s written consent is prohibited.
Graded AssignmentSCI303A/304A: Chemistry | Unit 6 | Lesson 13: Unit Testif 1 mole of s02 occupies 224 x mole occupy 67.2=x=1 X 67.2/22.2x= 3 moles2 moles of s02 yield 2 mole of 2s04Hence 3 moles of S02 also yields 3 moles h 2s04theoretical yield of H 2s04 = 3moles x 98g/mol=294gpercent yield= actual/theoretical yield x 100percent yield = 250g/294g x 100percent yield = 84%© 2008 K12 Inc. All rights reserved.Page 4 of 5Copying or distributing without K12’s written consent is prohibited.
Graded AssignmentSCI303A/304A: Chemistry | Unit 6 | Lesson 13: Unit TestYour ScoreClick or tap here to enter text.of 10© 2008 K12 Inc. All rights reserved.Page 5 of 5Copying or distributing without K12’s written consent is prohibited.