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EMPIRICAL FORMULA WORKSHEET Date 4 Period Name 1. What is the empirical formula for a compound which contains 0.0134 g of iron, 0.00769 g of sulfur and 0.0115 g of oxygen? : Fe0.004g) Innf . 2 400 ui‘-&"%,i“*".o ] Al [ SS. 85“3 < S qoxo-9 "I - b{f Q.oxiy T iz SOy =3 < ;Q_LDD’-H:Q vngf s 2. 9o x4 "\j 3. Hoxmp-9 = 2. Find the empirical formula for a compound which contains 32.8% chromium and 67.2% chlorine. ,.-;.zxg\ { weed - 0 ©36% M b D.OL\ Lol - 1.%4 19?903 6.b32% T 1359530 S5y e et 3o i (ea) 3. NAME the compound which contains 0.463 g Tl (#81), 0.0544 g of carbon, 0.00685 g of hydrogen and 0.0725 g oxygen by finding its empirical formula. T+ 0.463) el voaag 000033578 \ el - o.00L53 ‘30‘4 3?3‘” 500337 N9 ”’ODSO . 0007 ¢ 0.95 C| iwek - o.0053 3 \| 1A 0\3( oo.OOQJ’?" -‘:l C’;.“;;Oz. He 0. WYS'QH | IM Q_Q_dgﬂ'_. m{l;“’h‘\ CN\OOXZJQ/:‘C« 'Qdo{ 4. What is the empmcal forn%la fora compound WhICh contains 67.1% zinc and the rest is oxygen? 100 -(o3}.| = 33.9% O FniloFla| (wol w = 1,026 . | Y%\O*( \ (05'36135_‘14 \. D‘).(p E&QQHM :éO'S'(p < 2 ,lQ ()aj o [. o2l 5. Barry Um has a sample of a compound which weighs 200 grams and contains only carbon, hydrogen, oxygen and nitrogen. By analysis, he finds that it contains 97.56 grams of carbon, 4.878 g of hydrogen, 52.03 g of oxygen and 45.53 g of nitrogen. Find its empirical formuia. 6147‘5'(3\“3'\»;@1 8!.2 P 0,6‘3 03_' 2 3452 ¢ 4.878) Lol - R 31:.0\11«1 i 830 TN %531\‘ ‘ng = 3-95'0-/><4 2. 25D M 4 3.a5b

6. The characteristic odor of pineapple is due to ethyl butyrate, an organic compound which contains only carbon, hydrogen and oxygen. If a sample of ethyl butyrate is known to contain 0.62069 g of carbon, 0.103448 g of hydrogen and 0.275862 g of oxygen, what is the empirical formula for ethyl butyrate? C10.b2009 | el -p osiLy _ STUOR T Fotay =3 ‘CsHMDK H. 01034484 | ligd =0.10242 _p o ( l'obﬂ To0. 0174 0 0.22580le | lmel ., 61324 - [ | “\1poogo EWIEYY 7. 300 grams of a compouhd which contains only carbon, hydrogen and oxygen is analyzed and found to contain the exact same percentage of carbon as it has oxygen. The percentage of hydrogen is known to be 5.98823%. Find the empirical formula of the compound. 100-5.9%323 = 3401 . 45> C ond 17% 0 C:13.004 [ st : 3.9(3 “Tioioe === =[.33 H‘,ifi3§‘é—3 | 1t : $. 929 _ YRS ET B STle(3i g3 X3 + Y3.00 \IVM@__ ~ - 91 Sluo.oo%° aa'laz‘;l' X3 LCV Hbon 8. 200.00 grams of an organic compound is known to contain 83.884 grams of carbon, 10.486 grams of hydrogen, 18.640 grams of oxygen and the rest is nitrogen. What is the empirical formula of the compound? .00 ~ (3‘3. ¥¥1 +10. 456+ 19. 0 ‘(o) =~ Jo. 99 C:Z38¥ |\med - g A8 (NIREAY | e = 209 - 3 0. %0 =S. 3 13-013¢ - Tos b x3 | l‘»f.ol&/\l\ LS 3 . X3 12,496 ¢ | Ll - ;o.‘y ¥ . H - |-D‘3H e FAx3 C'\S’H.za—OBNW o bion) Ll - | 1o -ix 3 o . 110.0040 T TL% 9. 300 grams t}an organic sample which contains only carbon, hydrogen and oxygen is : analyzed and found to contain 145.946 grams of carbon, 24.3243 grams of hydrogen and the rest is oxygen. What is the empirical formula for the compound? 23pD -~ [ 14§ .9‘(54' 24.3243) C. Hsh-qu‘(\ \l\"._f-e-—.: Q.15 - $xt L "lu.olic g..08 " L 24.3293 ) lmed_ . aypy H: ~TTolqF B 23X g—— 2 [39.32925 O J C3H, O 7 2 N - 120329 el 2108 - | x 2 ll‘o.OOj 8"08

EMPIRICAL AND MoOLECULAR FORMULA WORKSHEET 1. Anoxide of chromium is found to have the following % composition: 68.4 % Cr and 31.6 % O. Determine this compound’s empirical fornula. crb83lr o315 0:31:630 =975 21 X2 5200wl =lre lb.O@SMp" 308 31 05 2. The percent composition of @ compound was found to be 63.5 %0 silver, 8.2 % nitrogen, and 28.3 % oxygen. Determine the compound’s empirical formula. ' 3.8 _ | 223N _ 0585 _ Aj |03 ?-j»wp" Dc’,.ss?;fiaol N 11oTqmt’ "o 58S ol .28, 3a - | ‘j‘bq ~ A N 0.3 0:3-28—, - 1. 701 = I b 003 mel! SES | 3. A 170.00 g sample of an unidentified compound contains 29.84 g sodium, 67.49 ¢ chromiuny, and 72.67 g oxygen. What is the compound’s empirical formula? ' 4 Na:298% > 1.298 -, o2 2298 po -/ — JJ.‘!qgwf" 1, 849 z S5.004 . 318 ¥z 72. - 4.842 5 o [ | 017‘?5%%7-/ dhe =250 Na, €405 | 4. A 60.00 g sample of tetraethyl lead, a gasoline additive, is found to contain 38,43 o lead, 17.83 g carbon, and 3.74 g hydrogen. Find its empirical formula. Pbi3843¢ . , |955 C 1388 - | Ugs s o, B il th;'?&-l :-5"[3:%%5'3 =20 &L‘ H“’ng 5. A jC‘l«Om_})Omld containing 5.9265 % H and 040735 % O has a molar mass of 34.01468 g/mol. Determine the empirical and molecular formula of this compound. H'.5.92b85 _ - e (&0 -CFp 3.0l 0:84.0335, = 5. 8% 3,“"0'%’?% hY H- O lb.ooywe-' S. 63 | #.0I

6. The empirical mrmuja for trichloroisocyanuric acid, the active ingredient in mary household bleaches, is OCNCL, The molar mass of this compound is 232.41 g/mol. What is the molecular { omwla of trichloroisocyanuric acid? CONCl = ?’-}.V?JM"’ - i e 2334/ FFY> 7. Determine the molecular formula of a compound with an empirical formula of NHa and a formula mass of 32.06 amu. N#, = (603 gl 3,{:'?);:1 NLA. 8. The empirical formula of a hydrocarbon (compound that contains only C and H) is found to be CH. Laboratory procedures have found that the molar mass of the compound is 78 g/mol. What is the molecular formula of this compound? CH:= lS.OllrW‘e" _3:_2?__. 9. The molar mass of rmoime s 162.1 g/mol. 1t contains 74.0 % carbon, 8.7 % hydrogen, and 17.3 % nitrogen. Determine nicotine”s empirical formula and moiecular formula. e MO et 6.l o NG 23N o Ly /L»~--~~ii -'03 L. 31 - w,ol:{w/‘/ EYE L» 3. ‘35\»”(/ T TATEANR SN ER Tap s 1.oIg .24 IR L T 10. Phenyl magnesium bromide is used as a Grignard reagent in organic synthesis. Determine its empirical and molecular formula if its molar mass is 181.313 g/mol and it contains 39.7458 % C, 2.77956 % H_13.4050 % Mg, angd 44.0697 %% Br. C. 380 _3.30% M i‘ OS"SM L Rl et <l P b2y \C.DHMNZ-MF

Empirical and Molecular Formulas Worksheet Objectives: + be able to calculate empirical and molecular formula Empirical Formula | : 1) What is the empirical formula of a compotund that contains 0.783g of Carbon, 0.196g of Hydrogen and 0.521¢g of Oxygen? 03834 ¢ [ | 0.005 _ 0:0 ‘)9|qb“w~ap 2.033 C S g(zmé:é 0033"9(” l((gaos >.033 | 4 0.196aH] et . O [ 5 g C,H,0 [1.0lq "©-033 2) What is empirfcal formula of a compound which consists of 89.14% Au and 10.80% of O? Ay XQl“ls\\vw—? I ' [ Mo135 Su{q's*? " A J . lD-g% !lvv—o-e 0. i{’ - 2+ O Uao?fi 0.453 =15 3) What is empirical formula if compound consists of 21.2%N, 6,1%H, 24.2%S and 48.5%07? . o ) \M Q_‘j,g,b._.ul N alaaN| (wel.).S13 S f—’ﬂgfig 256 |4-6lg 0350 N N 0, LTI ‘90" l i «—g 4y séo]\wrf 3.63] - Molecular Fcrr%ula .00 o- -'7510 4) Empirical formula of a substance is CH,O. Molar mass is 180. What is-the mo%ecular formula? cW,O=730.03 80 2,0 3D.03 5) Sample (3.585g) contains 1.388g of C, 0.345g of H, 1.850g O and its molar mass is 62g. What is molecular formula of this substance? e e o 1.3883C - 0.USL - CH, 0 :E.Fl "uolamd Sch A D . ) Ly 3).04 L | C,H,O0,=m.F/ Liy = og%?% 009 Dr S Bukienica

Topic 7 Hydrate Worksheet #3 Solve the following problems. Show work to support your answer. 1. A hydrate of magnesium sulfate has a mass of 13.52 g. This sample is heated until no water remains. The MgSO, anhydrate has a mass of 6.60 g. Find the formula and name of the hydrate. g L S ':),H_ D mestum S W\&SO% .03 = 0. oi:g >| Mfi % z Mfifh&\\yo{/ /7_on 0.0 (an . 0.3%Y -:), B0 13.52 ~ (pbO (oQA HLO"’ "“““i.{g 2.A sample of copper (1I) sulfate hydrate has mass of 3.97 g. After heating, the CuSO, that remains has a mass of 2. S;;f Determme the correct formula and name of the hydrate. H,0° 3 99 -2 - } "lfi 7_{() 0.6M 6¥Y _ - < Vy.ozgvt™ 5loled 2598 =015 (e pasknk doate (JA& ‘{ 159, U(sﬂev’ 0.0159 ~ C,M&Ol{ S"H,z/o w‘)eé,\ St.(,o : M }l 3. When 5.00 g of FeCl; - xH,O are heated, 2.00 L ‘of H,O are driven off. Find the chemical formula and the name of the hydrate. §.00— 2.00 = 3.00 Fed 3 3.00a - 0.01§5.) 2.004H.0O_ o \\o% Fecly Toa. 20wt ook T2 ol " ool =b ('e,C(B LHO 4. A sample of the hydrate of sodium carbonate has a mass of 8.85 g. It loses 1. 28 g when heated. Find the formula and the name of the hydrate <. ?gg-— . 35’3 = 5?3 Na CD3 Nay Dy 3933 i 0031 .\ thpo: 1288 z0.0%1D T osAaRe! po3o T woz&M" Zamio =0 Na,Coy - H,0 5. A 16.4 g sample of hydrated calcium sulfate is heated until all the water is driven off. The calcium sulfate that remains has a mass of 13.0 g. Find the formula and the chemical name of the hydrate. |l ‘-(j - {3, DS 3.4 9 H'Z/D (oS0 : ' o @30y 13.08 200955 | " L 3dy 04889 ., (I O 1 3b, Ng 0.095S . oajwel 70455 6. When 8.00 g of Pb(C,H30,); - xH,O are heated, 1.14 g of HyO are drlven off F1 d the chemical formula and the name of the hydrate. &~ 1. NS .%o ] Pul( Lt 302)2 PG 307>a L‘A* = 0.02109 = | H,0: 1. Hﬂ . 0.6b33% =3 P‘OCQHSO-;)A “ ; 32S. 393 0.02109 'S, Dlspe’ 0. OND"‘ ¢ 5 HZD 7. A hydrate is determined to be 45.43% water and 54.57% CoCl,. Find the chemical formula and name for this hydrate. (*Hint — assume that there is 100 g total of hydrate compound) Coll,:54.53 =0:4203 _ [ (>U, (0 H, 0 1349, ?qs“‘*" 0.Yrd3 2t =l a7 D’)SMI 6. 4203

9.3“(3'05‘{3 E |.,:)’5 (o (I\U)s),‘ 8. When a 2.24 gram sample of a hydrate of calcium nitrate was heated, 0.54 grams of water was driven off. What is the formula of the hydrate of calcium nitrate? alMDy), i 13 - p.0104 Ca(NO3), - 3H, O 4. O"Swp 0.0|0Y . 0.543 - 0.02%93 _ “’*D ts'oz&wa' T %.0\04 =3 9. When a 5.0 gram sample of Cu(NO3), * x H,O is heated 3.9 grams of the anhydrous salt remains. What is the value of x? &=39 = ‘t% Z/D (o (ND3), é_fifigg :o.o:o?fi_\ PR A .00 - F. 5y 0.03034 &,.[NDQ;’SHLO 0elOY _ | H. O mt "o o.;o‘-;—qﬂ =3 | X =3 0. A hydrate of sodium sulfite, Na;SOj3 » x H,O, contains almost exactly 50% water by mass. What is the value of x? [Hint: assume you have 100.00 grams of the stuff.] ‘ — _o_.‘._éib_’_?..— - - f‘\“zéoa‘ 5‘;‘%&5@4 T 06-396%2 = X 7+ N47803 ‘ } HLD . &Da - 2335 w,0 * ?302 ' T o-396% " 11 A hydrate of sodium sulfate with the formula Na,SO, * x H,0, weighing 3.223 g, is heated to drive off the water of hydration. The anhydrous sodium sulfate weighs 1.421 g. What is the value of x? 2. 3239 143g 2 L. ‘&oajbto 3 N(\;SD;{ ’ lto HLO x =D

0. 00‘5‘8(036,02' O ,,P;“‘Combustion Analysis and Concentration Worksheet T \? 1. Combustion analysis of toluene a common organic solvent,gives 5.86 mg of COzand 1.37 mg of H20. If the compound only contains carbon and hydrogen K"'\7v'fi§t_7§_|/ts emﬂcal fc\:rmula’P - Py M o wel C =T 14404 [wetcdy T, 330 ¥ }8 b 40 |dmed H o™ 4: 02020 b - LIXOT | 14 %3 DH\??— Ladkon 0.14 =/ 2. Menthol is composed of C, H, and O. A 0.1005 g sample is combusted, producing 0.2829 g of CO2 and 0.1159 g of H20. What is the empirical formula for menthol? If the compound has a molar mass of 156 g/mol, what is its molecular formula? . 0.2839, 0, | \wel D2 | lwad € -QoowsvaC - 2 °°"“3M‘3l‘2°'_"& 0.6%%) R Sy ,kl"{ 0q (O ! Iwsd (O . —e10-9 s 19e{ q< »\S%Hzo\ lwel b O | Jned H Ol 8bwelH —> 0.0l fwd -0.003¢H B “"."’7" Ty. oaSH,,o}\MHz, = 0 qj“g.”fe "—B'}'\WL i 3 ~ 20 p.vooS - (o b} 35 4+0:013) 20.010330 B.F=Coth,O=ME 0" 0.010340L Ll O - (5. YY xtD el O =) N 1:0040 'qq xi0™" L”'Sb;" ool 3. Combustion of 2.78 mg of ethyl butyrate produces 6.32 mg of COz2 and 2.58 mg of H20. What is the empirical formula is the compound is composed of C, H, and O? .43 X0 ‘(XIZ o@\,(l 0.80063)q O} \vel Oz | el € . = |. %3@)(&0"’,\”%“'9 z0.0013qC o rnmas e T A Gp?-r: - = | q"“ooswz,\ \W\re(ﬂz_ ""C, 7V‘§)QO.{ i - iof e . 0.9025%H M— 2, 8b3XID el | S 2.83x107 x O :10.00a378 - (o 0O1F + 2.8 x /0 q) ?‘708’“0‘&,,1 waod = 49Ya5 Xl O b0 03 .q% 5 X(0S 1,0 ¢ -rlms m\v\@’“ hos ecrors o it 5.8 «4?0 H