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All complete CEM 161 Lab PDFs excluding 7&9. (Labs 1-6,8,10-13)

by: William Decker

All complete CEM 161 Lab PDFs excluding 7&9. (Labs 1-6,8,10-13) CEM 161

Marketplace > Michigan State University > Chemistry > CEM 161 > All complete CEM 161 Lab PDFs excluding 7 9 Labs 1 6 8 10 13
William Decker
GPA 3.71
Chemistry Laboratory 1
Amy Pollock

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These are all of my labs (Yes, I missed lab 7 and 9, my bad) that are all fully complete for reference or review before performing on of the CEM 161 Labs! Enjoy!
Chemistry Laboratory 1
Amy Pollock
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This 32 page Bundle was uploaded by William Decker on Tuesday February 3, 2015. The Bundle belongs to CEM 161 at Michigan State University taught by Amy Pollock in Fall2013. Since its upload, it has received 411 views. For similar materials see Chemistry Laboratory 1 in Chemistry at Michigan State University.


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Date Created: 02/03/15
Attebstiaib39 ii I 4 0 0 quot 6 th EE39QJM 39 D G G 6 CD CD CD lt2 a o C2 5amp3an QMHZ C3 Q D o o f 2 6 g I Completion aappearance of product 2 l2 6 Precision of the two experiments 3 l3 7a Accuracy of result 15 5 o W 310 I d 39 391 i i 1 a Table 1 Welghing data and calculations Your data Partner s data Experiment1 I Experiment2 Experiment3 Experimental Massoftesttube Q InitialImass of 2 iron nails I g I Q a Oil 0 39I 5 I Final mass of2 iron nails I1 I I I Mass of iron oxidized I I g I to E 39 OH I I Moles of iron oxidized Sag II It 53915 I6 I 7I 3 0 ca II 0 31 CT39 Mass of test tube a copper a a I Ia OH x t IQ II Repeat weighing i 39 Oq I39 6110 7 x Repeat weighing 7 39 Mass of copper reduced 0 I a u 5 I O v t Moles of copper reduced I I I15 W U I K SI 11039 39Mole ratio ironfcopper II I L0 K9 9 i J i 39 39H I I Total mass of iron oxidized for all 4 nails 0 as 1 5 Total mass of copper formed 39both experiments DI b C3 II CE 3 II 39 Total moles of iron oxidized I I I a U qM I L 31LC 3 I Total moles of copper reduced 35 3M I III 1amp0quot 1 aquot Overall mole ratio ironlcopper a I I Oxidation state of Fe produced in the reaction i 4 C 60mi dJ f 1rWr39 ng ld 39 W 39 W 0 Ui w3 chimi msgt 4 The Stoichiometry ofia Redox Reaction Table 2 Ob arvatlons of any reaction between the iron nails and the copperlt sulfate solution a 6701 Om i 04quot Grm bc 3 3 4quot 53 6 0M whet I gtV39 r emitgr 4 wmc 0413 5919 saidhm a x a w my 5ohh k Q c56 d M 1439 c hquotorn5 hum Table 3 Equation fer the reactlon between iron andyopperal sulfate f Wag gees rtowb ietrom r Lka 05qu was d mi 80393 mfsk eweW94 M311 WC di RRtemL geoth 5th sen J r 40 Aqobleqsso 0 e o o w o o l o J o 39 i am 1 oi l Wyeth 0 11V I Skew CUU L Densities of Iiguid39s ble 1 113 Densities of plastic samples Table 2 3 13 i Calculations of densities Table 3 3 l4 Total 8 310 Table 1 Data and calculations for the densities of the liquids Mass of10rnL 5 graduated cylinder 3 ca 1 Liquid Trial Mass 9 Volume mL Density 9 mL Average 1 MW LSD ML l g Nquot ISOpropyl alcohol 2 I q 1quot0 0 h n SINCE 3 SHWQB LiamL JV 5 5 SM AS 1 lSDtol ML 1 33 Saturated sodium 39 J 39 chloride solution 2 1 9 00 ML L A 3M 393 Libel5 Llme l m w Li W 1 6 53 El Bil ML r 5 wquot Potazsoim dide 2 Li Kpb3955 ml l 53 65 5 i a whim Woo L libel gal 5w 25quot 2 I 4 Separation of Flecyolable Plastics by Pens v Table 2 Densities of the plastic samples relative to the tour liquids Checktherdtsamples i 39 39 Saturated sodium Saturated potassium you were assigned Isopmpyl alCOhOI Distiled water chloride solution iodide solution Density from Table 1 L nk 4 100 9 mL1 13quot Plastic samples u sank floated sank oated sank floated sank floated 239 Egt l l39l l39l39l 59 J J v 13 I D u ITI Egtlt5gt 39 U 390 I11 5gt 0 39U a lt K5 J id KF 1 Klt 39U U Table 3 Data and Calculations 39 Checquot W 4 Samples Mass of liquid Volume of liquid Density of liquid Average density of liquid you were assngned mixture used mixture used mlxture used mixture used Plastic samples a 9 mL 9 nilF1 Density 0139 plastiC l 39n J A A 0 quotquot i wow v V 3939L z a VMJAQE yam m2 w x 1 Half jtbgo Omb St L WVVV voVwmWt I LWIUQ ampOm z m 1 so is gt9 3 quot got eq M if Eggs 9239 W 5Ll s 3 j I w lam 0393 W9 4 1 WWER stag NU E TSQ qu J 31mm we mm D lt4 222 5gt 43 26 A i to 0 3 u a 395 0 0gt 0 a 0 0 Smwmq CO N GD GD E I Graph neatness accuracyampbest t LM 53 liiioie fraction Table3 3 I3 Q A baichations Tobie 5 2 I3 Total I 10 Table 2 Measurements and calculations W 339 Exp W433i quot33 3533 Moles of Total 23931 13221 9quot 99 V 39 39 acid mL acid gramls Nchoa 03993 IiiaHICfJ3 cm cm quot3 0 None None 000 Zero 1 24 0419 J61 3590 20quot 5L9 33513 2 21 0366 93 395539 53A 310 3quot 30593 3535340 1 500 3 13 0314 Sup 30 533 313 319 19331 1amp3 0377 9 4 15 0262 QQiDQ ic b f 335 50 mo i118 MELLi J totem W 5 12 0209 Abtk ktx39bbq 69 l9 a 93 LOLLO LHQCE J wquot 01111 39 U PiafL 50a 7 6 1105 lm Miss 33931710 Subs 3007 I 5w 8 None None 100 Zero 33 m The Stoichiometry of the Reaction between Baking SOda and Vinegar Table 3 Mole fraction of sodium bicarbonate at the intersection Mole fraction of NaHCO3 at intersection 5 I r Mole fraction expected Mole ratio of reactants 3 0 Comments 3m mom sac RM airwm tm39mt 39 0 m mm quot1 A Table 4 Computer result Comments tbs moms rm Ma WWW lift the mfc amw 35quot M cchcJtx h 3 mg draws 65 Ms M new 3 3 Q53 3 x E Mole fraction of NaHCC3 at intersection r 539 g I i A 3 Table 5 mole ratio of products to reactants f 39 L Q Atmospheric Pressure C atm Room temperature 1 A as K i Volume of 002 54quot S 3 L Limiting reactant at the point chosen I M a Number of moles of limiting reactant h mol Number of moles of 002 from graph 0 mol W 39 a g 34 The Stoichiometry of the Reaction between Baking SOda and Vinegar i 39 db Graph of volume of carbo dloxide produced vs mole fraction of sodium bicarbonate M 35 is a a 5 1 Mt ghLROK o 9 Me ACD39s waifi39 p u ancocuase m 9 Uttlnm 39 ELK 5 CD D G CD D D D T C plet perfo a c LIZ om IOI39I rm n e 3 33 Graph neatness straight amp best fit f M D Calculations precision 8 accuracy LI I4 e Tota mm 39 r G 3 TD 9 Table 6 Average density from your own data quot quotD Table 1 Weighing data Average density 9 k00t07 gm 4 O E39 9 Written with correct number I I 3 39 THE 1 u sq 7r 9 of signi cant gures 9 o I g quot Deviation from mean l a a 95413 Instructor39s initials Tria2 x gq at Average U ls Table 2 Dimensions 95 430 D 9 O o LL 04 Cross section area S l I CM 3 39 a C l a 7 CM cm2 Length Q Li 393 on i KW aha ng 0quotquot Volume area x length 39939 5 l 0quot I C M3 cms Density mass I volume I 9 a i g glcma Table 3 Volume determined from water displacement Volume of water q q ems Volume of water with metal C 1 0 1t cm3 Difference volume of metal A O cm3 I Table 4 Data from other students FN 1 1 m k 1 L Mass 9 Vol cma Mass 9 394 Vol cm3 Mass g Vol em3 from Table1 from Table3 from Tabe1 from Tables from Tabe1 from Tabe3 3mm V550 Til clto m L 39139 33ml 506 s Bqti 5 3 1l05 V7 31 lgt Giigtb vec Qantas 3E1 lm s as 337 no Table 5 Density determination from graph Student Name A Rise mass U 9 Run volume 1 7 cm Slope density a gl39cm3 19 1 I I Determination of the Mass and Density of a Metal Sample i Graph of mass vs volume 53 it 13 c310 at 50 5 no 0JWC V 3 I Table 3 Preclpitatlon reactions Anibwampsq or t 0 o o o o i S39I Mm we 39 1 G D a a G G G D Owl D F Precipitation reactions Tables 3amp4 13 5 GB C5 Acidbase reactions Table 5 CZJZ Gas forming reactions Table 6 1 i2 Redox Reactions Table 7 3 13 o 9 e e 0 3 Q Total HO 9 Sodium sul te Potassium iodide NaZE 3 quot Kl Sodium phosphate Na3P04 NaHCO3 Sodium bicarbonate 39 Silver nitrate lgNO3 N Tquot Copperll nitrate CuN032 V R n a 12 NR Cobaltl nitrate 30lxii3r32 M R NR PW 2 r Nickelll nitrate NiN032 Miquot 7 NW Vi Table 4 Equations for two precipitation reactions Reaction between Write the overaii ohemicai equation the detailed ionic equation and the net ionic equation for each assigned reaction an ASNQ 4quot 4V 7amp3 KNOB 39 Am 10 Jr NOQchD JV Yi wn Ino Ag ten k A3935 Mam t 11qu 4 A4100 3 CO L N0 338 Sam Q DOL GECPOHZQ 5 Not if and CQCNO39SEQ age Q ogcm ibmanomfm 17 CIA Pan halt09 H J 306 Jr 3303 wp TV U 3 as 4399 m Chemical Reactions and Chemical Equations Table 5 Acidbase reactions Color of phenolphthalein in acid oo d COlor Of phenolphthalein in base D n L U I u Trial 1 Trial 2 Trial 3 Average Number of drops of 39 NaOHforHCl a O Number of drops of 39 NaOH for H2804 CD cg 9 Q Q 33 N OH I HCI Overaquotchem ca39m quot39 Nabwar MLth Nadine 4 Raf m a 1 reaction Detaiiedionrc equation k Gag HOGh w 2 ndE m l I r O Netionic equation l 0 Ms w 03ng 9 1 Overaiichemicaimuation i N 033 Ui JS N OH wrquot 39 quot 3 H2304 Detailed ionic equation 2wxma3m3 V O 0 Jr GAD reac on Netionicequatioia I 33O39ZQQ tr Og kchn 4 Q3 TM mart bkmota ennui3h wee mod lee5 15 lam Explanation M m whe gm DJEQ L 5 i5 m beukromlchim WentH cm i5 533 el Meale age gawk Table 6 Gasforming reactions Reaction between Report your observations detennine which gas is produced and write a compiete chemicai equation for the reaction Observations quot39 Marble chlp M were we xbmmmwed 3 a and HCI U sauna C C COB qui quot7 COB Jr H o nga a l Hydrogen peroxide Observams Eithde and KI ii I QHaOa r M if 0a 3930 Md Zinc and HCI 39Obsem mS 0 Camel Equation JV C W A ZKQQ 50 5 I a 39 Chemical Reactions and Chemical Equations m k rw mem Table 7 Oxidationreduction reactions Reaction between Report your oboervations and write a complete chemioei equation for the reaction Observations Zn and 804 Mr 4le acme went d91 Equation lg V 2 Ll Observations J Cu and Zn804 tng MKSA I Equation Zn quot 7 M 0 1 Color of bromine I 1 I v in oil Observations I E g u Chlorine gas and Observations l k t M m an Fa 39 Fluid bromide ion 39 39 Equation C 9 Jr ggji gt 173139 EQCA 5 Color of iodine in oil mm W Mimok GSA 0flVD e we I W cellar Chlorine gas and Observations m 4 lms 39od39d i quot 39 Ge l39 3 Veilcl JFK 39 39 vs Bromine and Observations e Tb M j C51 def m 1AM QWVP i w l are 61 i aex C 51 13 A A 19 O Lk Z O E G G G G G G G Precision of standardization of NaOH 212 Precision in titration of vinegar 31393 0 Accuracy of result 93 6 Titration technique ZJZ e E im39 9 quot Q Q Q Q 9 9 69 Table 1 Standardization of the NaOH solution Trial 1 Trial 2 Trial 3 Average Molarin of the HCI solution i R Final buret reading mL q A a 39 Initial buret reading mL 0 O O at 1 ULCS 5 Volume of NaOH required mL b q C1 q Molarity of the NaOH solution I v 0 idquot 39 Table 2 Titration of vinegar with standard NaOH solution Trial 1 Trial 2 Trial 3 Average Final buret reading mL l 13 l we 397 Z Initial buret reading mL 0 L39 50 p11 Volume of NaOH required mL 639 H q C lg t6 0 is or I H I new M 105 Aubotsuzso g5 39 Tx G lt1 G a D 6 C ff 2 ompletlon and pe ormance 2 Q Q Yield and appearance of product 11 14 G 0 Explanation of observations Table 2 l1 l4 Tota 0110 39 5 9 9 lt9 Table1 Weighing data 9 Mass of copper metal at the start g Mass of capper metal at the end H 397 1 9 Percent copper recovered q 0 Table 2 Description and explanation of your observations I Describe and explain your observations Mention any stage at which copper may have been lost Do not b j rewrite the equations from the introductlon Describe and explain what you see 0 1 The reaction of copper wrth l39lt tl lc acrd Erma 60 We Comm M anew f2 bb tot ow QU roads 3 QQ GampCQQ4 Tm CaPtDE r39 Meia4 m we Wma Meow ran aw 394 ka acids Mn buhbtmoi U l 2 The precipitation of copper l hydroxide Tm mmkkm 4va6 Cquot bquot We Wilmaw MdreSGAC Lg39si b tuo 6 5 50w 0133 3 The Prtit riio 1 WW oxide gmi m mmym e a vacnae Qrm a Narth dwe 05 cu W 00165quot Edv 39 1 16615 wove Ping3 m Roth peb Wk E39C 4 The preparation of copperll sulfate b MM 3 peeved to W Suiguno Lad be N waL 9 09quot we irem K39leD e We 42619 qu Ma W531 5 5 9 KQVu i39Wb l Msoanm Y39qsoi 5 The reduction of copperli with zinc 3 g 1 tom 1 mm W 2 Sawquot a minim a emoticth 009aquot a awquot 5 N Lquot WW3 w ction esteem exam mak com v53 111 awn able A vi to 0 5 U 7 3 O a 5 L xr39n equf Clt39fTbI1 3 ompelono ae 7 3 3 g Accuracy of results in TableZ Ll 4 GD 9 I Answers to questions in TatI93 3 3m We 5 I 9 9 Q Table1 g MOIE Cule vale c ons nonggmdg g cgairs Jmrradf3939ugnl211 at 39 thf egle 39 picture of EtKH uid I I Number of m i tio T polar or 39 the molecule i am mquotde pairs 99390 News quot1 mm 9939 P939a39 B181312 2 2 x 7 I dectrom I f j g linear linear Ziamaim 000 Be 1678 2 andmgpm 59gb nding J nonpolar 99239 3901391133 20 equot quotI quot39 3 knew T me w 1516 g Q 151 1 1L LU 2 It Wm b 5 Tao F F PCI gins aquot equot 39 umquot Qa R f bNAW T rmw cx u tu L T43 3143 quot3quot R61 H3 3 k tonsWit any who g D V I w TAM F 0 CE HUD Ha a 3 Pa wau g mace Fd 11 9st 3 WW 5 mm a g cnwm cf 22 WW g kcmx 429 500 r ig F 9 K 5W6 quotlk l H Sdbm39b 5915 13 F F 111 n lap F 0 X611 EMMA quot3ae 392 me Odmwr39ni chace vkemr c 1 ME mu 0 39339 MM sf da moawr Pd F 5 IF 1 9 1 aquot C 13 3 33 T V 5 1ka humquot gm m L ier 3 1M 3 5wm5 5115 wager i g Z WV W5 c m we wry omm im 9ka rtggg U LW B L11339 U dbQO tom mar 39 as O 1 Pg g no quot AD 395 0 mom 5 h ggm h Tab Mm realm u Pg 5 6V 0393 1 S 339quot Moms we mmxd Ex failsquot mmmzf 72 03 Othw m quot quotquot E immx d512 Wait Le Wm max VANV c 77 7 The Shapes of Molecules and Ions I Table 2 iMoiecule ygmlgg e lecons L nongngdg g cgalrs L 31392151 at thzhm egagle 1 I picture of g i Central Number of Nugpber oi Hybridization Polar or the mo39ecme 3 i 310quot bonding 93quot 91 clamsins 0quot 09quotquot339 atoll Qigpll39939 Aw we W as 5 a aly 3 Vito 3 3 dryaid Wu Mw a we 3le 1m x lllt no WI w mittJ wm y mi or We 10 to 1mm we mow u 1 613032175 3 U5 39 1 3 quot no mz w he vrohgsml m Vat 9 331 3 39l 0i MW 61gtquot 39WW39 5quot Baa1 541LE Z amt o long Wquot 9W7quot Witter fink T 3 la 1 3 de be mu m M b F EM swan Lwe 93 Wquot W CAMEAQS MWWJ squot l 6 A 1ch l 1 0 Lo Wfb 6W WM FmWF 0734 in mm no equot m m we 1quot 4 awmm is 31mm aria S quotwlr 39 S 1 clmosns 194 room or 9 91quot Miami Z 3 We 5 W wtquot lemlre m Fanquot W Slim 5 3 6 5 l demo be AM 0 HMZ at 1m3l all 5 971 quot Wquot THU KimmieA 492m 9 as g As s Ll JG t3 Agnew 51quot Tpnc or Table 3 gas all 39t e aggle gfemn the electror Iggomains in the mo cule SnCl 2 equal to 120 i xplain6 obo guru i a 5 Fa a ckl39a l 39 M 391 ms 3mm W Tl 0 ME mo 003 s c9ow 22 cW T W Q gore 3quot r 39 vxe al mun WW mlm sn our 09c it amami Describe the procedure you would follow to determine the shape of a molecule containing H terminal atoms 3 mold no ech Nu oak dam bdb rmd it two P5W M i it Mai 6 31 13 lquot W mm or Wk P 30quot5 E No toes2 me 9 M Wt twat W mocha u doublt a we Wit Lino Cad W mote Worm l zincht 78 A to CD irl 2 395 O 9 0 Mom Desm G G D G D D G D 3 C2 C2 o l 0 GD G Tbl 1 ZZZ 6 o 9 a e o m Tab39ez 3 3 games 313 0 0 Answers to questions Table 4 1 2 9 Total 10 110 Table 1 The pH reference set pH Color of Acidic Solution pH Color of Basic Solution Q 1 Li nk 22A 3 L 9a B h t 2 lags A ngr lL Ray 9 Rm 1 3 RatL Dial 0 Dorm m melee 4 Diana 1 Emmm Gwen 5 Utes blow 2 Lima Green 5 Wrote l Pay lit mo bright 1ng Neutral 7 iii 96 Table 2 The pH of the clear reagents Reagent Indicator color Estimated pH Acidbase classificatlon Distilled water may VAL kg 13 J 05 M sodium chloride kLAae kt 5 FKCJ 05 M sodium hydroxide Lime Gigf zo 05 M acetic acid 339 05 M hydrochloric acid 41A 05 M ed 39 r v r 3 mm bicarbonate 06 Z 33543 05 M potassium nitrate q G5C u 39 05 M ammonia Ewms Gym 65 05 M phosphoric acid 39 W Z RC as 9739 11 Red Cabbage an Indicator for Acids and Bases Table 3 The pH of household products Reagent Indicator color Estimated pH Acidbase classification Window cleaner m ea Washing soda Gig goebt Lemon juice lvcsmium Z Carbonated pop quot IL A Milk of Magnesia Maw Em 8 356 Bleach E593 m 395 Sugar micasle mi k at A tng ivch M s was seen ease lowest a ram Table 4 Questlons Question 1 The products listed in Table 3 can be divided into two main categories what are these two categories and what is common to all products in each category Tbs2 we M EMN 2 Qmmvs which 033 euaib 0 W M 9 93 66qu g b bk N LOrx oSQ one 3 qu Question 2 Choose one of the reagents in Table 3 that causes a color change in the indicator Is there any way to change the color of the indicator back to the original Which other reagent in Table 3 would you choose to do this What happens in the solution when you do this to M t d tea311quot LEW oicc To cm the actor of 39 W I smoke Cko ijaCIVJlWC h CQ CO lbw m k chst quotW1 Q t f Mix it U W tot x Koice 039 km to Em Mic QXngk 98 A Uriah 3 WZLS 0 0 o o 39iAlwm sds G D Q G D D D c 3 3 M G fM39th ca e lt4 D I ObservationsIBalanced equation Table 3 i 11 Data and units in Tabe2 Calculation of molar mass in Table4 212 Q Precision in the three experiments 213 9 9 3 9 Accuracy of the result error 2 Total 9 no Table 2 Data Experiment 1 Experiment 2 Experiment 3 Mass of aluminum i 39 Temperature of the water CIK 23 C 2 0 Actual I Corrected water level mL 7 up Volume of gas collected in L I39vozjsz 07 IL Atmos pressure in hPa torr 21 JL H l q Vapor pressure of water in torr 39 2 r Partial pressure of H2 in torriatrn quotI Eb 5 5 331 Number of moles of H2 q Lug bj xxpf 3 L AOquot 5 Table 3 Observations Observations on the contents of the test tube quotM zbku ri en WM m m Wumimom but AQrou g warn Wue wuod new in w stir5k quotram 17 cut mime was a agrmrkwr ma am Balanced equation for the reaction between aluminum and hydrochloric acid ZN 3r WM gtZAC5 JrTS Az 1 le SSVW QiWOlV 91 10 I Determination of the Atomic Mass of Aluminum Table 4 Calculatlons Experiment 1 Experiment 2 Experiment 3 1 39 3 l 51 no Moles of H2 produced Table 2 Fm 3amp0 vul L D AK 3 Moles of AI required in reaction W k 6 quot 1 d 0 3km 4t U i 391 X squot394 Mass ofAl Table 2 H v ovgg mcg c Q l l q J Molar mass of Al 39 395 9450 O 39ZK39 S A Average molar mass of Al 2 o 0 Actual molar mass of Al 2698154 g rrlol391 39 Percent error bblb 92 Auoosqaso 5 39 t L N 0 e lm Waller 233 3 2 g 3 2 SteW CW 533 0 Gaphs p ope placed t fl39 es m It ei 39 3 Neatness of data sheetsagraphs 1J2 Measurement of arm and ATwate quotz 12 P Calculations and accuracy ofR Q3 Total 9 I10 r as Table 1 Masses of the metal samples 39 39 39 Aluminum quotSniper 339quot I Unknownalloy Elsaqu 834753 isms at Table 2 Temperature data for metal samples l Aluminum Copper e 145Leac l 1 Unknownalloy Elapsed time 39 Temperature of water Temperature Bfwater Temperamre39hfiiivater Temperature at water minutes 39 in calorimeter In calorimeter in calorimeter in calorimeter 1 39 Mom aaam AQJ T orgrbc 2 930 C QQAOL QQKTC 3 860 C 11 12 13 57 I 6 I The Heat Capacityof Metals an it Table 3 Heat calculations Aluminum Copper d Lead Unknown alloy ATmetalfromgraph oC Ilgqto ac ma anew la 13quot c c 0 L 3 a o I i c Heat gained by cold water specific heat of water x mass of water x temperature change ATwater 4134 JK391g391 x 100 g x temperature change littmmIr Heat gained by cold water A 3 383 g 3 355Gq 5 Heat lost by metal heat gained by cold water Heat capacity of metal heat lost by metal I temperature change ATmetal Heat capacity of metal to eke3AA 51L l 3 Mass gf metal Table 1 l 63 Ss qo 3 sq 35 39 ezol 503 Speci c heat of metal heat capacity of metal 1 mass of meta 39i Speci c heat LaeflUsatf ma IOlC aLl LLa moan hilt31 qu VL L Speci cth l tracela 7 age la lci M1616 Molar mass of metal 2698 6355 2092 ebb L a Table 4 Results 1ISpeci c heat of unknown alloy from Table 3 5 guns 9 K Jquot i39 r 1 Molar mass of unknown alloy from Table 3 j g mol Slope of the line a e J K391rnol391 l w i la a f Calculated value of gas constant R 39 0 Q J W 3 i Accepted value of gas39 constant R J K391moll391 t 5 a 39 39 f 39 39 1 i 58 The Heat Capacity of Metals LL Bfitcm baggd Graph 1 Timetemperature calorimeter data for alumlnum m 300 IIIquot 39839 Temp arml39uf c I A O 39 otax w bb9 0 mlll 1 Twit l 39v LMMQ e53 6 I The Heat Capacity of Metals Graph 2 Timetemperature calorlmeter an 8 data for copper on CC r39quot l a gm 398 16 336353976 manta am t f QMPbpd L 9m ates 6 I h The Heat Capacity ofMetas LL 39 hm Graph 3 Timetemperature calorimeter data for lead 691 msulrgai 39TJW C aps c Lawn5 61 a The Heat Capacity of Metals Graph 4 Timetemperature calorimeter a data for an unknown alloy Othsk b Sto39Z KCnNuxaqri TML MWJEJA Cmimo e 6 I The Heat Capacity of Metals u 1 Bad W Graph 5 Graph of the molar mass vs the reciprocal of specific heat Cam HOV1L e i 5 quot zquot 5 lt36 6 BR Lt g m 3 l u 39 E lb ewaero wear 014133quot 63


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