化学英文化学报告Word格式文档下载.docx

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CalculatethePercentYieldofFerrate

TheSpectraVisspectrometerwascalibratedusingDIwaterinfullspectrummode.TheDIwaterwasremovedthoroughlyusingaplasticpipetteandthesodiumferratewasputinitsplace.Theabsorbanceofthesodiumferrateat510nmwasrecorded;

however,sincethevaluerecordeddidnotmeettherequirements,thesolutionwasdiluteduntilthevalueoftheabsorbancerecordedat510nmwasbeneath1.5.Whenthatlevelwasreached,anothersampleofthesolutionwastestedat510nmandanothervaluefortheabsorbancewasrecorded.

Theremainderofthesolutionwasplacedinanotherbeakerinpreparationforthenextphaseoftheexperiment.

TheconcentrationofferrateintheoriginalsolutionwascalculatedusingBeer’sLaw.

Thetwovaluesforconcentrationwereusedbytakingtheaverageofthetwotogettheexperimentalyieldoftheferrate.

Thisvalueoftheexperimentalyieldwascomparedtothetheoreticalyieldthatwascalculatedatthebeginningoftheexperiment.

Part3:

PerformingtheReactionbetweenFerrateandDIatrizoic

Inthispartoftheexperiment,thegoalwastoperformthereactionofferrateandDTZAtoseehowfastthereactiontakes.Thereactionwastobedonetwoseparatetimesandexpectedtobesimilaronetotheother.

Inafirsttime,theSpectraVisspectrometerwascalibratedusingDIwater.AfterthecalibrationtheDIwaterwasdiscardedinawastebeaker.

Then3mLofthesodiumferratesolutionwaspouredintoacuvetteandameasureoftheabsorbanceat510nmwasdone.Similarlytothesecondpart,iftheabsorbancevaluewasabove1.5,thesolutionwasdilutedtogetanappropriateabsorbancevalue.

Thecuvettewasthoroughlycleaned.Afterwards,2.0mLofDTZAat0.040Mwasacquiredand1.5mLofthatsamesolutionwasdrawnwithapipetteandpouredintothecuvette.

Thenextstepshadtobedonequicklyinordertoassureaccurateresults.

1.5mLoftheFeO42-wasaddedtothecuvetteandatthattimeastopwatchwasstarted.Theabsorbancewasmeasuredassoonasbothsolutionsmixedinthecuvette.Thecuvettewasshakedfor5secondsandplacedinthespectrometertomeasureabsorbance.Everyonceinawhileduring5minutesworthofrecordingoftheabsorbancethecuvettewastakenoutandshaken.Themeasurementsweredoneevery30secondsduringthe5minutetimeframe.

Afterthe5minuteswereup,theferrate-DTZAsolutionwasdiscardedinthewastebeakerandthecuvetterinsedout.TheabovewasrepeatedforanothertrialwithanothercombinationofferrateandDTZAidenticaltothepreviousone.

Theworkareawasthencleanedandahypothesisformulatedfortheresearchpartoftheexperiment.

Materials:

·

20mLofCommercialBleach

StirringBar

StirPlate

10gofNaOHpellets

0.50mLof0.30FeCl3solution

SuctionFiltrationapparatus

Graduatedcylinder

GlassVial

SpectraVisspectrometer

Pipettes

Cuvette

Wastebeaker

Testtube

0.040MDTZA

Plasticbucket

Ice

Thermometer

Results（SaraFurgeson）

Thetheoreticalyieldofthereactiontocreatesodiumferrateusingbleach,NaOH,andFeCl3wascalculatedusingtheFeCl3asthelimitingreagent.Asshownintheequationforthereaction,foreverymoleofFeCl3used,onemoleofsodiumferrate（Na2FeO4）wouldbeproduced.

2FeCl3+3NaClO+10NaOH→2Na2FeO4+9NaCl+5H2O

Thereactionused0.50mLof0.30MFeCl3,andthefinalamountofferratesolutionwas19mL.Thetheroreticalyieldwascalculatedtobe0.00769M.

0.50mL*0.30mol/LFeCl3*1L/1000mL=0.00015mol

0.00015mol/19mL*1000mL/L=0.00789mol/L=0.00789M

Staringwith2.6mLofsolution,10mLofwaterwasaddedtodiluteit.It’sabsorbanceat510nmwas1.455,givingitaconcentrationof0.001265M.Anothersamplehadanabsorbanceof1.192at510nmandaconcentrationof0.001037M.UsingtheformulaV1C1=V2C2theoriginalconcentrationsofthesolutionswerecalculatedtobe0.00613Mand0.00502M.Theaveragebetweenthemwas0.00558M.Thiswasdividedbythetheoreticalyieldof0.00789Mgivinga70.7percentyield.

Calculatingconcentrationsofsamples

V1C1=V2C2

2.6mL*C1=12.6mL*0.001265M

C1=0.00613M

2.6mL*C1=12.6mL*0.001037M

C1=0.00502M

Averageoftwoconcentrations

（0.00613M+0.00502M）/2=0.00558M

Calculatingthepercentyield

（0.00558M/0.00789M）*100%=70.7%

Thereactionbetweenthosesolutionsof00558MferratewastimedasitreactedwithDTZA.Theabsorbancewasmeasuredasthetimedpassedtocalculatehowfastthereactionwastakingplaceandhowfasttheconcentrationwaschanging.Thenthisexperimentwasrepeatedatdifferenttemperaturestoseeifloweringthetemperaturewouldslowdownthereaction.Thetemperaturestestedwere1,4.8,12,and16degreesCelsius.AlltheratesofreactionweretakenfromFigures3through7andcompiledintoTable8andFigure8forcomparison.

Trial1:

Time（s）

ABS@510nm

FerrateConc.（M）

0.631

0.000548696

30

0.656

0.000570435

60

0.674

0.000586087

90

0.622

0.000540870

120

0.605

0.000526087

150

0.583

0.000506957

180

0.560

0.000486957

210

0.552

0.000480000

240

0.542

0.000471304

270

300

Table1:

Thistableshowsthedifferencesinabsorbanceat510nmandconcentrationasthetimechangesforthefirsttrialofthereactionbetweenferrateandDTZA.

Figure1:

ThisshowsthefirsttrialoftimedreactionbetweenferrateandDTZAandtherelatedequation.

Trial2:

0.589

0.000512174

0.578

0.000502609

0.579

0.000503478

0.582

0.000506087

0.569

0.000494783

0.562

0.000488696

0.558

0.000485217

0.556

0.000483478

Table2:

Thistableshowsthedifferencesinabsorbanceat510nmandconcentrationasthetimechangesforthesecondtrialofthereactionbetweenferrateandDTZA.

Figure2:

ThisshowsthesecondtrialoftimedreactionbetweenferrateandDTZAandtherelatedequation.

Reactionsat1DegreeCelsius

0.828

0.000720000

0.830

0.000721739

0.837

0.000727826

0.729

0.000633913

0.719

0.000625217

0.655

0.000569565

0.633

0.000550435

0.658

0.000572174

0.667

0.000580000

0.630

0.000547826

0.643

0.000559130

Table3:

ThisshowsthesamereactionwhentheferrateandDZTAstartedat1degreeCelsius.Asthereactiontakesplace,absorbanceandconcentrationchangewithtime.

Figure3:

Thisshowstherelationshipbetweenthetimeandtheconcentrationwhenthereactionstartedat1degreeCelsius.

Reactionsat4DegreesCelsius

0.867

0.000753913

0.868

0.000754783

0.861

0.000748696

0.845

0.000734783

0.835

0.000726087

0.834

0.000725217

0.844

0.000733913

0.832

0.000723478

0.827

0.00071913

Table4:

ThisshowsthesamereactionwhentheferrateandDZTAstartedat4degreesCelsius.Asthereactiontakesplace,absorbanceandconcentrationchangewithtime.

Figure4:

Thisshowstherelationshipbetweenthetimeandtheconcentrationwhenthereactionstartedat4degreesCelsius.

Reactionsat8DegreesCelsius

0.939

0.000816522

0.81

0.000704348

0.805

0.0007

0.809

0.000703478

0.816

0.000709565

0.793

0.000689565

0.822

0.000714783

0.812

0.000706087

0.806

0.00070087

Table5:

ThisshowsthesamereactionwhentheferrateandDZTAstartedat8degreesCelsius.Asthereactiontakesplace,absorbanceandconcentrationchangewithtime.

Figure5:

Thisshowstherelationshipbetweenthetimeandtheconcentrationwhenthereactionstartedat8degreesCelsius.

Reactionsat12DegreesCelsius

0.647

0.000562609

0.635

0.000552174

0.91

0.000791304

0.847

0.000736522

0.817

0.000710435

0.839

0.000729565

0.802

0.000697391

0.807

0.000701739

0.776

0.000674783

0.78

0.000678261

0.803

0.000698261

Table6:

ThisshowsthesamereactionwhentheferrateandDZTAstartedat12degreesCelsius.Asthereactiontakesplace,absorbanceandconcentrationchangewithtime.

Figure6:

Thisshowstherelationshipbetweenthetimeandtheconcentrationwhenthereactionstartedat12degreesCelsius.Theconcentrationat0and30secondswaslowerthanallofthefollowingreadings.Therewasprobablysomeerror,sothesetwotimeswereignored.

Reactionsat16DegreesCelsius

0.745

0.000647826

0.725

0.000630435