CHEM 1101 Test 1 - Fall 1996

CHEM 1101 Test 1 - Fall 1996 - M1MZM3 4 Peter H.Perk...

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Unformatted text preview: M1MZM3 4 Peter H.Perk Marcus-_ s: e l I ' e 1 mam. Us“ 3‘1 CI-[EIUHSTRY l Hill-SECTION 14km Test # I Fall lfi‘ilfi LI}. BUTTDMLEY There are 20 equal}; weighed questions on this test. Pleas: circle the correct answer for the multiple choice questions. Please ask. lfyoude not understand The question. Please work this test Independently efynu: neighbors. notes and books. GOOD LUCK! _ ill _fl2 l 1_ _ _ l—E r-—z.—ea Ema}: —h{e vDJ-hv (It mmmfix); _h_ 411: E- 21 M=-z=(;— l }R M=hv=fi€ £4, ‘_—3 y 2 2 J' A, " v Hfinad lKlr'm'l'ml Pfiv’. = Pl‘sv'2 WT: = VZJTE P'v’ = nRT MTE..GAS..A.(d§fi§efi] = W3 RA TE..GAS..B.[drfiefl) med um: ' g Average KE per mole = MEET 22.4 L ideal gas = 1 mole at STP Psolvent : Xselvmt Pusnlwmt ATE: = Kb m ATf = 'Kf m n=gdh nV=nRT Pl=XlP"*'l P1=ffi~i2 P”2 _ _ CI Pz—kaz F's—(I'XJP 2 Avogedro's Number N, = film: at It)” m: = 9.1 x 13'“ kg Gas Constant R. = {IflBZElé litm—atmfmole-K mp = 1.6? 3: III” kg R = 3.3145 menle-K ml= 1.6? x lfl‘flkg mum I: =6.626xlfl‘1‘]*sec a. = 5.29:10'um - . zln'mism as 2-13110“! leflnrie=41341 lev= LE}: 10"] / usHsIou 1 PAGE 1 l. a solution contains 2.00 g of potassiu of water. What is the concentrat' KDH [i wiwl? uroxide {as = 50.11 g mol'li in 10.00 g of the solution exPressed in mass percent of a. 6.04% Gm]!!- h. 16.1% c. 20.0% d. 2. The element gallium has two naturally occurring isotopes. The Eirsr 1590a} has a relative mass of 60.925? and a fractional abundance of 0.004. and the second {TlGa} has a relative mass of 10.0209 and a fractional abundance of 0.395. Based on these values, the chemical relative atomic mass of gallium is ‘ili 00.7 4. 69.9 c. T0.1 d. 10.3 3. Compute the relative molecular mass of Zniflcozjz on the 120 soale.i.e molecular weight“ (a! 3-3 ' a. 123.4 *PZ" lro 1 b. 139.4 14 c. 143.4 I1J§}J 2: .25: 65 14.44 4. At 20“: the density of methanol [CH30H} is 0.?91 qiml. If a laboratory worker needs 215 g or methanol for an experimentIr how many liters should be used? / VERSIGN 1 PAGE 2 5. Propene gas {caflfi} burns completely in an oxygen atmosphere to produce carbon dioxide and water as the only products. If the reaction is described with a balanced chemical equation using the smallest whole number coefficients, the coetficient for water would be For the following question{sj, consider the production of ammonia gas through the reaction of nitrogen with hydrogen as described by thenbalanced equation “2 +3H2 aims m 6. How many grams of NH3 will be produced by the complete reaction of 3.91 g of H2? 25.1 g oneIII HT 6’ 50.2 g 15.3 g a. 1m g Hrol' at?" r. The followinoflquestionlsl concern the production of acetylene gas [Czflgl by the reaction of calcium-carbide {Ceca} reacts with water as described in the balanced equation Icacz + 2 £1204 caioH}: + can“ .9 «II-F "PH 5 xr‘bc K t T. I How many liters of CEHZ will be produced by the complete reaction of 23.5 g of I ‘II. ,-;-'- Ceca Iwith. 10.0 g of water? I melt-‘7- ZEN-(,1. RH::f a. 0.4451. éw'154aa‘ “aflfl'ifpoh: . H.555 L .531. Clfll—‘Efl Zak mfg/o”Fr ,LfLH'” .6; * CAD Fvfinflf‘ + (£0 Vcnflr‘ P VERSION 1 PAGE 3 B. If 13 g of CaCz reacts to produce 0.2fl0 mol of C232, the percentage yield of the reaction would be 35% 53* . 30% . 9M: 9 11% 9. Write the correct name or symbol in the blank space. norm- s ol Name Pb lead a 5.. I04! Magnesium [Jam Sodium _%_ Mercury 10. Write the correct name or formula in the spaces below. Name Formula Barium nitrate Potassium permanganate I a -‘r 63,4 no; gu.,g»‘1(|::flim~VL NP.th Diphorphouo pentaoxide E; gps VERSION 1 PAGE i 11. one mole of any element has a mass in grams equal to: a. avogradro's number the weight of a single atom che atomic mass . the atomic number e. the atomic mass divided by avogradro's number 12. How many atoms are there in 36 grams of carbon? a. 6.02 x 1033 o. 2.11 x 1025 .81 x 1o24 . 2.1a x 1o23 e. 1.31 x 1o23 13. Give the empirical formula of a compound which contains 52.2% carbon, 13.0% hydrogen and 34.8% oxygen. - (:b-LJD C) “14° C' Iloq 4: “LBSMJ 1'2, 44' 1.0: e 11.27 m' s:- a. O‘Iébfi 4 3413‘s” ‘3' ” 14. What is the molality of a solution which contains 15.fl 9 HCl in 100 g of water? 322:.” W WW d. 0.15U m e. l-Sfl m 15. a solution contains 2.oo g of potassium hydroxide in“ - 55.11 g mo1”1} in 10.00 g of water. What is the concentration of the solution expressed in mass percent of KOH I! win}? 1- .r M @533: 15' ~03“ K c. 20.01: :‘Sffflgf M?) o- 25-fii 12 a“! VERSION 1 PAGE 5 16. In order to prepare 0.250 L of a 0.115 M HaEr solution. a technician must mix a. 0.115 moles of NaBr with 0.250 L of H20. b. 0.115 moles of was: with 0.250 kg of H20. c. 0.02025 moles of NaEr and enough H20 to result in 0.250 kg or solution. c::> 0.02015 moles of East and enough H20 to result in 0.250 L of solution. mu! mfir u. )02.35%.r “‘3' I. 'W- .mfifim’ 1?. What volume of a 15.6 H H003 solution will be needed to prepare 350 mL of 2.00 M H1003? II9MQ; a. 22.2 mL h. 36.7 mL 13.4 mL “9 m“ I what is the percent nitrogen in in N205? o, 13%.1-y/fl 18 ct @ 24.1 W “3.05 N1 0; *3 * fichpaf- or - 7 - ' 25" 9; c. 13.: We in: d- :3: dz. *5 23-034.! m‘IS-i ' I 213913 19. Consider the reaction: 3 Cults} + 3 “03'1an =5.) 3 C11 {malgtaq} + ‘1 H20 + 2 mtg} Iflqfilmhfi 6.3 grams of on reacts with 100 ml or 1.0 H nitric acid. Which of the Eollowing statements are true. cal—flarfifld—uitflctecid react in a 1:1 mole ratio. 41.4:e-es-che"&tmctinqfireactant and 0.062 moles of Hfloa are left over. 3 is the limiting reactant and 0.052 moles of Cu are left over. .di_flu-ead-Hflo3*ere present in stoichiometric amountswneither in excess. e. 0.000 moles of water is produced. ’régli'lmbr "filo! ...
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This note was uploaded on 05/08/2008 for the course CHEM 1101 taught by Professor Bottomley during the Spring '08 term at Georgia Tech.

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CHEM 1101 Test 1 - Fall 1996 - M1MZM3 4 Peter H.Perk...

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