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Chemistry Laboratory II Completed PDFs (11)

by: William Decker

Chemistry Laboratory II Completed PDFs (11) CEM 162

Marketplace > Michigan State University > Chemistry > CEM 162 > Chemistry Laboratory II Completed PDFs 11
William Decker
GPA 3.71
Chemistry Laboratory II (2)
Amy Pollock

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About this Document

Complete Set of 11 Chemistry Laboratory II PDFs.
Chemistry Laboratory II (2)
Amy Pollock
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This 32 page Bundle was uploaded by William Decker on Sunday October 11, 2015. The Bundle belongs to CEM 162 at Michigan State University taught by Amy Pollock in Fall2013. Since its upload, it has received 56 views. For similar materials see Chemistry Laboratory II (2) in Chemistry at Michigan State University.


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Date Created: 10/11/15
Abbutq Anwosaaso 0 9 is a ohm Dug J D D G G G G Completionlperformance Zrz 3 393 m Handling ofchemicalsispills 012 G G D Q Product yield and appearance 23 2 g g g g g Observations and explanations Table 2 3 3 g igTotaI no 9 Table 1 Weighing data Mass of CuCl2392H20 used 7 ORCE g Moles ofCuCl22H20 used lot 3140 mol Mass of CuCl produced g 3 Moles of CuCl produced mol l CPm QOV 1Tb g Percent yield of product q 0 Wt thgce39 1 M a 100 b quot d m with 1 Table 2 Observations and explanations Wm 0W 9 3 Mkam 1 What happens when potassium iodide reacts with copperll sulfate solution 5 TR gamm 06 tom 5C6 miss so wa l3 1 2 What happens when aqueous ammonia reacts with copperl chloride in the absence of air Tue assume Kw as M at his is was kw mm WC in as it tomb Q UzA 3 What happens when air is admitted to the copperl chloride ammonia solution so ems mass law as drug 5 w maigite ff aaIaO39IHo nae 13 A Lg 9 Q g U 0 S O H 6 0 lt9 D 6 lt0 lt0 D 2 0 lt23 0 39 Q T AMbmjer 0 GD GB GD quot GD GD C2 6 ilCcmpleticn performance 12 6 Precision of data in Table4 2 35 u j39HGraphs neatness straight best t 0213 C5 3 1 34 Accuracy ofreacticn orders I 2 2 g Tot339 5 K X10 m Table 2 Weighings I quot Mass Ofsodium sul te 9 Table 3 Estimated reaction orders Mass of sodium bisulfite I g Eistimated order with respect to A 1 Estimated order with respect to B Table 4 Reaction Data w at 3032 32 a 50 5039 30337 18152quot I b 3950 50 I 11quot a 2 a 50 J 100 me 97 W b 50 100 39I M91 357 3a 50 150 a bl ax l C s g b 50 150 quot391 41a I 50 I 2amp0 HO r l e O b 50 200 5at 25 P 100 J I 1 7 013 b 35 100 33 100 I 100 Lib 5 Oe q b 100 100 7 150 100 2351565 1365b e lt3 5 b 150 100 v I u Ba 200 I 100 I a I i 1 b a g 390 3 21 Chemical Kinetics The Formaldehyde CIOCK ReaCtion 2 I e F Table 5 Data for thereaction at lower temperature Reaction Reaction Average Rate Tna39 A B Temp C Time sec Tlme 1 Isec 39 f quot 39 9a n 50 a 50 t 0 t A 39 397 ifquot quot v I b H 50 50 g 3 quotV k Rate relative to Trial 1 m 21 3932 H Table 6 05m fer the reaction at higher temperature 4 39 I Reaction Reaction Average Rate Tmquot A B Temp 13 Time see Time 1Isec 10a 50 50 L 39 39 b 50 39 50 I Rate relatlve to Trlal1 m pm A DJ q Table 7 Summary Data Trial mL of A log mL or A mL of 339 logmL or B quoteggquot lograte 1 so 75 39 ot l 410 2 635 rte 557 furs 393 S Q 10 e0 1118 i03l au 4 go No reg 395 25 040 39 l 0 b t I t 01 quot L M 6 100 100 at l u 3 L Lab 7 150 113 orb I tbs quot i Q a 200 mo no I I n m 73 l at Table 8 Line slope data liable 9 Reaction orders from measured line slopes Slope of line through points 1 4 I Order with respect to B 39Slope of line through points 5 8 1 ea 9 Order with respect to A quotquot j J Angle between lines q 0 0 Overall order of reaction 0 39 39 39 J 22 i 1 3 7 Chemical Kinetics J39he Formaldehyde Clock Reaction M W m Graph of Iograte vs Jog mL of A and log mL of B u r 0 2 39 Us b5 awwvau 23 DMmmTkgmrf g anvu 03gt 0 0 F I 3 Abram 9109 M A woven 91me J oh q l I Ex um Graphs neatness straight best fit in oo e oeoo o sa o o v 99 9 9 oe ltn o ev We Precision of data in Table 2 2L Accuracy of mole fraction Table 3 912 Equilibrium constant expression Table 3 I I1 attormwretcyr of values for K Tables 5 and 6 1 2 5 Total Q 110 Table 2 Data fot the method23f continuous variation Test Tube KSCN mL 39 FeNt 133 83Fth 1 Frac ngem Absorbance 1 9 1 f 9 e r 9 t 3910 2 i 1 a 9 999 0 5 3 2 739 9 9 979 I Z f a om 4 3 6 9 067 We 5 4 5 9 056 Db Lo r 5 e 39 9919 39 7 5 3 9 033 a 39 1099 I 8 7 2 9 022 1 9 r a 1 9 911 h f a L 1 1 9 0 9 00 39 O Standard 2 Excess 39 31 I ChemiCal Equilibria The Formation offan lronThiocyahate Complex A 5 Haas cJ FA TacahWoQaifg Table 3 Reaction between Fe and SON Mole fraction of xFe at intercept v S l O v if Value of n in FeSGNn Equilibrium equation R e tat jaw J Equilibrium constant expression LEEGQQDIL E l li blcni s lL Ea Table 4 Calculation of the concentration of the complex TestTube KSCN mL lnltlallltscn1 FeN033mL 33353 Absorbance 023232 Standard 2 1 x10 3 M Excess Excess k 39 1 x103 M 3 Q a 1 low M 7 7 1Qquotquot II b Ll l gxlbg 8 quot 1 j OWN 3x 39 a x 539 le Qtlka 3 5 l nail J Table 5 Calculation of the equillbrium constant from data for solution number 5 Descrigtlcn son1 Feat Complex Equi39ibr39quot quot5 aquot l Initial I amp lehwm quotIMOquot A to Change x k H u 39 5 Elnal qu 5 0 4 me A 339MB am D V Table 6 alculatlon of the equilibrlum constant from data tor solution number 8 Desctipticn SCN39 Fe3 Complex numb 0 quot3 aml Initial 397 x 3quot M Q R 0 M 0 Change i x Jr 1 H H F39 I quot l llb 3 g 0 quot ma L W b m l Ull m 58 m m l 36 JD 32 3 1 Chemical39EqUilibria The Formation Of an lronThiocyanataComplex Mn mower Graph of absorbancevs mole fraction of Felll H Add HOV 39 e Q De can 33 34 In aquot Pam cm l AaxooauiaSQ 39 G D 39 Satisfactory completion of titrations 212 g Calculation of molarity 391 I4 Precision of the three titrations 1 l4 Total I H 010 CMD GC 39 G C D 0 9 Q J g 9an 7 0 Table 1 Standardization of the NaOH solution Titration1 Titration 2 Tltratlon3 Weighing bottle initial ma39ss g v Weighing bottle final mass g39 a 1 a we 1qu I Number of moles of KHP N I i 1 f Equivalent number of moles of NaOH He ggafp39 g f I t Final buret reading mL I to L L I mm L I ml Initial buret reading mL quotjwru j Q uQML 13 39 Volume of NaOH used mL chug l L Volume of NaOlI in liters 39 Dl OK i l at Molarity of NaOll solution M y 8 I a 539 amp a 39 39 ar39 quotV 053 eee Eh 39 139 1 a H 39 11 39 quotmum It I 390 d J 39l iv i J39 x i f r w i t u r I 39L39f v 1quot 11 jl H 1 J quot I r I 39t I391 an M r H a Aquot Ll cc 0 63 J I 0 ewy ea ml wwt xr CM3 x Preparation of the complex 2 39 C3 0bsewaticns Table 2 l 11 39 Q G GD Precision of the titrctions Table33amp4 3 x4 39 Accuracy of the result Table 4 023 5 39 CD 3 Tom 1390 r G l r O39 37 Table 1 Preparatidn of the cqmplex NIINl3 Ntl332 Mass of NiH206N032 used 8NX9 l f I l Number of moles MM 290795 t 0 1 a 3 mol Mass of NiNH35NO32 produced Ll H3 39 9 Number of moles MM 284887 39555niol Percent yield h 3 In Table 2 Gheervations during preparatlon t NINH36N035 v e r39 i l wewa mm Duo ml QQW we 6 w W Q0989 DXPlQ color wgmmgcwmxw w ac P l m The Preparation and Analy ls Of a Nickem39 AmminsPOmP39eX l 39 39 do o Table 3 Standardization ofthe hydrochloric acid solution x i1 iquot v I Titration1 H tration 2 Titrations Molarity ofthe NaOH solution a 1quot I H I I u I Final burstreading mL l q I i ML I Initial burst reading mL quotQ m L 39 I farL J 393 Volume of standardized NoonI used my or m L f tmL I 9 3911 8 ML Average uolume of NaOH used mL r1803 wt a I I Molarity of the HCI solution 1 39i39 Tahiej iin twn of the ammonia In the nickelili ammine complex 7 Titration1 I 1 I Titration2 titration I A m m r o ltle l M N web 0 lo imt 139 n Clme 9 lnitiail assessing mL 1 O m L j I ML Volume of standardized NaOH used mL x T W argon hilolarity oi the NaOHsolutidn a Moles of NaOH used a I i a ifquot b C I moles of excess HOI present on I C Q Number of moles of HCI in 20 mL 39 O O 5 39 Moles of HCI used to neutralize the NH 00 C90 O moles of ammonia present 6m ug J 30 6 L x 17031 mass of ammonia present E Y I bib Mass of l39liN032 i E 1 18270 moles of NiN032 V 9 Ratio of moles NH3 moles39lNiN032 quot 93945 s rq39 0390 2 it Average ratio ie n in NiNlI3IN032 L AI Ll to c tantal k g A i 0 e ff it LA v ew i D D D Trtrationtechnique 39 2 12 3 RI Precision in titrations k 1 1 4 Q Q G Accuracy of result 4 CMD CHD m 7m 39 39 9 Table 1 Determination of nickel in the c bmplex 39 Titration 39l I Titration 2 Titration 3 Weighing boIttle initial mass 9 all I I 3 3 s Weighing bottle final mass g a 7 3 Mass of nickel complex 9 II I I a I Final buret reading mL ttibIltg j 500quot 0 loneA Initial burei reading mL I VolumeoiEDTAaddeo mLIL Deena 335 53kg MolesoiEDTAadded I OOD39I gigU obIblojdJi I goDb39IlLPlr Equivalent moles of nickel 0 U1 i m I f I Mass at Ni2 in the complex g II 01 I51 titt39lqio O Rq Bug n LO 39 Ol H QQ QBQ Percent mass of Ni2in complex J OLD a II 7 T OI I L OIOI Average i amp i h 33 3436 2 51 eeee as 1 E I f l i I I 399 1 f A r f 19M 4 1 r i quot H 4139 1 c 3 quot 1 MT 15 stJ r 1 h I E t M i quotquot4 39 quot3quot J J 52 e1 1 P A L b 0 6 9 6 6 Hm 39 G 6 G lt9 G geese C2 23 e 2 T J 3 5 mm i GD GD GD pg A k quot9 Q 1 69 Qquot 59 e a 3 9 39 Graph 1 dalaaccuracy neatness I3 e Jr Graph 2 data accuracy best fit neatness IM V quoter Calculations and inter retation LES a 39 Total 110 L Table 2 Spectra of nickelllnitrate apd the niekelul ammlne complex Wavelength Nicke39lll nitrate ngkeuu aminlne complex Ditfer nee Transmittane Absorbance 39gTranemittance Absorhbance Abeorbance 500nm egrgggeagga gasp mWs39s 7gtW13 Wm li op o lira6amp3 1133901 emcee 69831751 520 ampL0 e 1005 W o l ssonm 39mlt3r5 4930 039lto Loewe 549m jj 00 lo AVG 5 336 Lgc ox 7oo IDwos Leo o Wj l Lwa sq 560m 73 Mam b fe LL00 Les15 Seeemegesw 0ca tn AW x3903 563 gem 0 1391mm LFlt 599an 65m 5 game L0 70 gm L39mtm I 600nm asrocf e 941ng 7 H6533 HCEAQPQ mm Ea Ammo 5 70 Law lpoo 620nm game aw 6215 l39a6Ho 1hour 630nm 3mm W b mm 11 HEM ween 640nm ampb l e m knewe MM f wx 3 5739 7 I Spectrophotometric Determination 353 39th lift Table 3 Abserbance vs mole fractlon at wavelength 510M Solutlon Mole fraction of ammonia 39l39ransmitta ce Avg ABE sorbance 1 I 096 I ma came ew 33 2 03994 Walt 3370 361 3 092 20 Qg cb 93 61 67 00 4 090 30 Scls f5 lts l lRQSQA o 5 use 5 swag 51 5 6 086 50595 609 aq b o 7 034 5046 571 8 032 Lila safe 5 5 39 M7Dc5 9 030 I waofo q m 733b3 10 I quot 073 Sim Sisfro quot saw 11 076 Stabblaek J F ii I 1 1 39 Table 4 Results from the graph of 39 Flgure 139 Typleal plot of absorbanee vs mole absorbsnce vs mole fraction fractien tor a eonibound of the type AzBrl l Mole fraction of ammonia at intersection mamp i quot Therefore mole fraCtion of Ni2 l E 3 El n 539 00 p t 39 Value of n in the formlhla l liNH3n2 f 39 l gr I I NJ 1 a I I 1 Mole fraction of A 10 V 1 A 391 i Q J w H It 58 W quot CA7 1 quotIquot I l 7 w 5 3g 39Qtoichidmetr dfthe NickelllAmmine Complex 39 ii I I 395 3 izr 139 I BINIii LA Mmm 6201 Graph 1 Spectra of Nickel l nitrate and the 1 Nickel l ammine complex a 0 9 to m mm If If Um quot 39o 63 3 t I u rquot 39 VJ 39 31 39d F d 39 p 39 39 quWQ 234x 50 wwwch t in i J 7 I Spectrophotometric Determination h J39 391 tit a mqu I d if 3 91 rquot39 122 J I39b I T a 1 a Mo t Vvuc kim 0399 thle 39 I a a quotI Q 39 I a Mamibe cc R a 6 39 5 Table Currentitlme mgasdrements quot Exaci iime Cufrent e a G I seconds amperes Q Of rmm m O 30 1 SH I QQOSK Hquot W 239 C9 C9 5 Hohfn 5 q 5 no mm 1900 8 lino Mum1quot Precision of mass lost and gained 1 7 D a 1km f Grth neai39h39egs 39 if g L O 90 N m Accuracy8 preci gn of area calcuiation 3 i3 j 90 W zgalculations Table 5 I 1 3 H I 39 Accuracy39of result Tabie 5 f3 100 5 1H A3 Total 0110 t 5 00 L39VW39 139 L sRb 3 39 001me bea ob NW Table 139Electrodemasses I O 7 Wu W 1 Cathbde I Anode I DH lSq M E A er electrolysis 5 89 1 Be39one electro39vSi I r KbQOg Mime 1005 mm WWI I Gaingin mass at cathode g 5 lag u E L S fmassatan de quotM i QWQO 5 Rex J J 9 M35 EMMDLD PM HoOh avowg 50m 5 f QIW 65 The D termlnation of the Charge on an Electron 7 Table 3 Summary of mass changes and calculated areas Names of coworkers Qathode Anode area In coulombs 3910 Me I Your data from39Tables r and4 l 3 85 A 50W v 733IOlt 43m Ema0 17705 43 36155 W 9 Sam m 5 xa 3 3 as C A355 ng t l 3 or 3 9 a C J u AwM39w Agni mung 3933351 L Averages 35 3 r5333 5535 g 9 Q I I Table 4 Calculation of the area under the current time graph the charge passedthrough the co I In coulombs gem I kc rtt ransom2152905 a l A aqq b A s quot H300 AA 5 Zia f u kc Ark3 grit A at 0 3 353519 A5 quot 39 OOD n k 1 m e lnAxrlaosx A oro g g r lCXBO39wA a Table 5 Results I j I that quot31 3 3 T g A 1 Your data Averages foryour group f Cathode j ample cathode 39 Anode Mass copper transferred average from Table 3 g c 5039 kSUBR ES SG 6355 moles of cooper transferred mol 1 Q 3 r Br 3 53 3J5 xrg gig x 2 moles of electrons transferred mcl lt q x4535 stem395 u 0395 1 31 x 602214 x 1023 number of electrons D HSL a 63 9 Charge passed through the cell from Table 3 C Kg lq Charge 0quot one mason i C r13 rl3393 5a6 we ed M I 0quot Percent error BIO I qugzj150o off 66 30 3 Ti 9 up u f i quot3de I 5 5 g I O Hquot 3931 A a 9 0 r00 9 IL x u m u t x 9 6 0 e 0 o at a an t a an O 3 K 5 hr I n Aft I 3 19 Array wade ch law Graph of current vs tlme kkx Mn PAquot The Determinathn of the Charge on an Electron q H39FV39II39I 1w wr Hr a It I In t I Liq utdirl 11quot at 3 DibE A q 0 O 3 H 2 5 390 u 0 o e 3 L nMLL G G lt9 G a a I o PreCISIon of standardization Table 1 313 g Precision of oxalate determination Table 2B 13 D Q Q g Accuracy Table 2 4 6 Total l10 0 9 9 6 9 Table 1 Standardization of the KMnO4 sol tlon Titration 1 Titration 2 Titration 3 I Weighing bottle initial mass 9 CEquot E k Elan 1 b L Weighing bottle final mass 9 t M 53 boq Mass of sodium oxalate g L K b q 39 e Number of moles of sodium oxalate 1 0i 4 D39L L 395 Equivalent number of moles of KMnO4 Z x QLk Z c3 55 0 nu X OL E Final buret reading mL 0quot LDC Initial buret reading mL D C5500 Volume of KMnO4 used mL ZA 0 b t L 07w 8 Correction ior blank titration mL 06 v 6L5quot Q 5 I E Net volume of KMnO4 used mL 1 3 q cs q 7 I Volume of KMnO4 in liters Q52Lq 39 0 3 t 0 Molarityof KMnO4 solution 39 slut9g 39 I Average 01261 2 79 10 I The Analysis of Oxalate by Redox Titration ii Wquot olHWb l lSmn obwmtll OQZEH 117 3 Jbbi2 Table 2 Determination of oxalate In the complex All data in this table apart from the calculation of the percent mass of oxalate must be completed in ink before the sample mass is entered by the instructor after which the percent mass of oxalate can be calculated Instructor39s signature A V V v Titration 1 Titration 2 Titration 3 333 33253 3353 Sample number i a i Mass i wmp39exlg Illi337 rllltl Final buret reading mL K0 citg I i i7 3 33 Initial buret reading mL 0 0 O 4 Q as O 0 Volume of KMnCi4 used mL 1 to 0i 6 i 2 Lg 5 Correction for blank titration mL 6 395 b 5 6395 Net volume of KMn04 used mL a Q7 Z 33 Molarity of Klian4 solution o 0 Number of moles of KMnO4 used 7S u 4 q tubu 140 Equivalent number of moles of oxalate J 5 i a 39 A Mass of oxalate in the sample 9 Percent mass of oxalate in the complex 61 ow i a 61 Q 3 15 39 5am A tw i il W M k5 a Q 7 1 Na 30 LoNC Gt A a o 2 Q 0 o e W lt3 G a G D Completion performance all KMnCi4 preparation 6212 D Q GD 9 Observations Table 3 i 12 3 g g g g g g g I Quality of product if M S ma39 7 9 9 Q C Table 1 Data and observations Molar mass of KMHO4 158034 gimol Mass of KNInCii L required to make 400 mL of a 0020 Msolution L I 5 p 9 Mass of KMnO4 actually used to make the solution L 9 Approximate molarity of the solution a it 3L5Li 13 23Ka 0amp Table 2 Preparation of the ironlll oxalate complex Mass of the ironllloxalate complex obtained 1 g Table 3 Observations Observations during the preparation PO grr r 3WCE w bwAr can t Lq rwva We bomxiem kmr39 aw we 2a 5 aem mtae 52 o amt qqerwo Eerw we a vac tellm rc wan oE iQC Sake inc we Qn rom was TWb ihE is wow xxxq are 0M gamermum m qurob E L Kldrx r mf ro todr mm m a 39 3quot me Appearance of the ironliloxalate complex th nk39 Came Pa t quot quotRu Wt Examined by lab instructor Instructor39s signature quot1 I a I I Ght betf39t r3 rap nea ness accuracy 5 I 3 C3 3 g Accuracyr of iron determination 3M 9 GD GD Empirical formula derivation and result 3 13 s gm 510 GD Table 2 Results of analysis 3 Mass of iron oxalate complex ago from Table 2 Experiment 10 lUk b g 3 A05quot Number of moles of iron 6 b39Wmol e 9321 Mass of iron in sample or 05 g Z r o 3quot Percent iron In complex quotl 730m fo Table 3 SpectronicZO absorbance readings ergo Sample Absorbance Concn of Felll H 1 6130 03 0 0 0M DH co39l a l3 two 4 NE 39 1 n 2350 5 D lquot ea anvil L to 730 2 be ix 039 U r 3quot Know he 1 3 LS 393 a 4 i 151 20 x104 M 5 3 3 3Tb j 5 1 7552 LEE MOquotquot M Concentration of Felll in 250 mL flask WWquot Ho39i Lot 916 x 5 1526 x UO M M Table 4 Gravimetric analysis of the iron oxalate complex 39 Mass of crucible and iron oxalate complex it v3 g bun 03 o 39I39I Mass of crucible l 0 38 9 5 Mass of complex 0 Ll Cl 397 g Mass of crucible and complex after first drying and cooling VL 1 K6 g 2 Second weighing of crucible V2 I L qu 9 Third weighing of crucible I 9 Loss of mass biol 9 Loss of mass as percentage of original mass of complex 85 11 I The Spectrophotometric Determination of Iron Table 5 Summary of analytlcal results J Percent iron this experiment 391 0 Percent oxalate Experiment 10 5 t A Percent water this experiment furl S Total iron oxalate and water 397 3 DSL6 Percent potassium by difference 2amp0 0 23 Table 6 Molar ratios divide by molar mass Mole Flatio Moles iron 5535 SD BL Moles oxalate 8802 1 bog5quot is Moles water 1801 Moles potassium 13910 9 8 to Empirical formula Tm C Figure 1 Picture of the structure of the iron oxalate complex ion bx P K 39 39 quot c 0 O O 0 H tag 0 t 86 m and the Gravimetric Determination of Water Q amn it Q m ba df Calibration curve for the spectrophotometrio determination of iron 2 mo u 1i qu COWCEK rKc Qor 6g R01 394 5 i O p 5 25 q 15 Abbot MK 87


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