ࡱ> tvklmnopqrsUDq` bjbjqPqP ^::cSQz z z z R4R4R4T6$NNN>O$bR r"]^d_d_d_$hR4ataaz z d_d_<Ӂa@z d_3d_atp(& 46d_] A#TwN$I60,{w { {R4X1LvTDZ 8 D1dLLLaaaaO44D56z z z z z z     MARKS: 150 TIME: 3 hours This question paper consists of 16 pages and 4 data sheets. INSTRUCTIONS AND INFORMATION 1. 2. 3. 4. 5. 6. 7. 8.Write your centre number and examination number in the appropriate spaces on the ANSWER BOOK. Answer ALL the questions in the ANSWER BOOK. This question paper consists of TWO sections: SECTION A (25) SECTION B (125) You may use a non-programmable calculator. You may use appropriate mathematical instruments. Number the answers correctly according to the numbering system used in this question paper. Data sheets and a periodic table are attached for your use. Give brief motivations, discussions, et cetera where required. SECTION A QUESTION 1: ONE-WORD ITEMS Give ONE word/term for each of the following descriptions. Write only the word/term next to the question number (1.1 1.5) in the ANSWER BOOK. 1.1The resistance that a fluid offers to flow(1) 1.2A chemical substance that provides an alternative path of lower activation energy for a chemical reaction  (1) 1.3The acid produced during the contact process(1) 1.4The name of the electrode in a galvanic (voltaic) cell at which oxidation takes place(1) 1.5The industrial process for the production of ammonia(1) [5] QUESTION 2: MULTIPLE-CHOICE QUESTIONS Four options are provided as possible answers to the following questions. Each question has only ONE correct answer. Write only the letter (A D) next to the question number (2.1 2.10) in the ANSWER BOOK. 2.1Which ONE of the following pairs of compounds correctly represents the products formed during the COMPLETE combustion of octane? A B C DCO and H2O CO and H2 CO2 and H2 CO2 and H2O(2) 2.2Which ONE of the following pairs of reactants can be used to prepare the ester ethyl methanoate in the laboratory? A B C DEthane and methanoic aid Methanol and ethanoic acid Ethanol and methanoic acid Ethene and methanol(2) 2.3The structural formula of an organic compound is given below.  The IUPAC name of this compound is ... A B C D2,3-dimethylhept-5-yne. 5,6-dimethylhept-2-yne. 2,3-methylhept-2-yne. 5,6-dimethylhept-3-yne.(2) 2.4The type of compound formed when but-1-ene reacts with water in the presence of a suitable catalyst is a/an ... A B C Dalcohol. alkane. haloalkane. ester.(2) 2.5The equation below represents a chemical reaction at equilibrium in a closed container. H2(g) + I2(g) ! 2HI(g) DH < 0 Which ONE of the following changes will increase the yield of HI(g) in the above reaction? A B C DIncrease the temperature Decrease the temperature Increase the pressure by decreasing the volume Decrease the pressure by increasing the volume(2) 2.6A chemical reaction reaches equilibrium. Which ONE of the following statements regarding this equilibrium is TRUE? A B C D The concentrations of the individual reactants and products are constant. The concentrations of the individual reactants and products are equal. The concentrations of the individual reactants are zero. The concentrations of the individual products increase until the reaction stops. (2) 2.7The net (overall) cell reaction taking place in a certain cell is represented as follows: 2H2O(!) + electrical energy ! 2H2(g) + O2(g) Which ONE of the following statements best describes this cell? The cell is a/an &  A B C Delectrolytic cell in which an exothermic reaction occurs. electrolytic cell in which an endothermic reaction occurs. galvanic (voltaic) cell in which an exothermic reaction occurs. galvanic (voltaic) cell in which an endothermic reaction occurs.(2) 2.8When the net (overall) cell reaction in a galvanic (voltaic) cell reaches equilibrium, the emf of the cell is equal to ... A B C D+2,00 V. +1,00 V. 0,00 V. -1,00 V.(2) 2.9Copper is purified through electrolysis as represented in the simplified diagram below. Which ONE of the following statements is CORRECT for this process? A B C DCu is oxidised at the negative electrode. Cu is reduced at the positive electrode. Cu2+ ions are reduced at the positive electrode. Cu2+ ions are reduced at the negative electrode.(2) 2.10The major products formed in the chlor-alkali industry are ... A B C Dchlorine gas and sodium hydroxide. chlorine gas and sodium chloride. hydrogen chloride gas and sodium hydroxide. chlorine gas and hydrogen chloride gas. (2) [20] TOTAL SECTION A:25 SECTION B INSTRUCTIONS 1. 2. 3. 4.Start EACH question on a NEW page. Leave ONE line between two subquestions, for example between QUESTION 3.1 and QUESTION 3.2. Show the formulae and substitutions in ALL calculations. Round off your answers to TWO decimal places, where applicable. QUESTION 3 (Start on a new page.) Millions of organic compounds are known to date. Four of these compounds, represented by the letters P, Q, R and S, are shown in the table below. P methanal QR  S   3.1Write down the following: 3.1.1Structural formula of the functional group of P(2) 3.1.2Homologous series to which Q belongs(1) 3.1.3Structural formula of an isomer of Q(2) 3.1.4IUPAC name of R(2) 3.2S represents an alcohol. Classify this alcohol as primary, secondary or tertiary. (1) [8] QUESTION 4 (Start on a new page.) Knowledge of boiling points can be used to identify chemical compounds. The boiling points of four organic compounds, represented by the letters A, B, C and D, are given in the table below. COMPOUNDBOILING POINT (C)APropane-42BPentane36C2-methylbutane27,8DPentan-1-ol137 4.1Define the term boiling point.(2) 4.2Which ONE of A or B has the higher vapour pressure?(1) 4.3An unknown STRAIGHT CHAIN ALKANE has a boiling point of -0,5 C. Use the information in the table to identify this alkane and write down its IUPAC name.(2) 4.4B and C are structural isomers.  4.4.1Define the term structural isomer.(2) 4.4.2Explain why B has a higher boiling point than C. Refer to structure, intermolecular forces and energy in your explanation.(3) 4.5Explain the difference in the boiling points of B and D. Refer to intermolecular forces and energy in your explanation. (4) [14] QUESTION 5 (Start on a new page.) 5.1Prop-1-ene, an UNSATURATED hydrocarbon, and compound X, a SATURATED hydrocarbon, react with chlorine, as represented by the incomplete equations below. Reaction I : Prop-1-ene + C!2 ! Reaction II: X + C!2 ! 2-chlorobutane + Y 5.1.1Give a reason why prop-1-ene is classified as unsaturated.(1) 5.1.2What type of reaction (ADDITION or SUBSTITUTION) takes place in the following: (a)Reaction I(1) (b)Reaction II(1) 5.1.3Write down the structural formula of the product formed in ReactionI.(2) 5.1.4Write down the reaction condition necessary for Reaction II to take place.(1) 5.1.5Write down the IUPAC name of reactant X.(1) 5.1.6Write down the name or formula of product Y.(1) 5.22-chlorobutane can either undergo ELIMINATION or SUBSTITUTION in the presence of a strong base such as sodium hydroxide. 5.2.1Which reaction will preferably take place when 2-chlorobutane is heated in the presence of CONCENTRATED sodium hydroxide in ethanol? Write down only SUBSTITUTION or ELIMINATION. (1) 5.2.2Write down the IUPAC name of the major organic compound formed in QUESTION 5.2.1.(2) 5.2.3Use structural formulae to write down a balanced equation for the reaction that takes place when 2-chlorobutane reacts with a DILUTE sodium hydroxide solution.(6) 5.2.4Write down the name of the type of substitution reaction that takes place in QUESTION 5.2.3.(1) 5.3Haloalkanes are used in insecticides (insect killers). 5.3.1Write down ONE POSITIVE impact of insecticides on human development.(2) 5.3.2Write down ONE NEGATIVE impact of insecticides on humans.(2) [22] QUESTION 6 (Start on a new page.) Learners perform three investigations (A, B and C) to study three factors which affect the rate of chemical reactions. They use the reaction between solid calcium carbonate (CaCO3) and excess hydrochloric acid (HC!) solution, represented by the balanced equation below, in all three investigations. CaCO3(s) + 2HC!(aq) ! CaC!2(aq) + H2O(!) + CO2(g) EXCESS HYDROCHLORIC ACID is used and the calcium carbonate is COMPLETELY COVERED in all the investigations. 6.1INVESTIGATION A: The learners conduct two experiments using the conditions as shown in the table below.  Mass of CaCO3 (g)State of CaCO3Concentration of HC! (mol"dm-3)Temperature of HC! (C)Experiment 12powder0,225Experiment 22lumps0,225 6.1.1Which factor influencing reaction rate is investigated?(1) 6.1.2Write down an INVESTIGATIVE QUESTION for this investigation.(2) 6.1.3The learners now repeat Experiment 1, but use 4 g of calcium carbonate in excess acid, instead of 2 g. They find that the rate of the reaction INCREASES. Give a reason why the rate increases.(2) 6.2INVESTIGATION B: The learners conduct two experiments using the conditions as shown in the table below. Mass of CaCO3 (g)State of CaCO3Concentration of HC! (mol"dm-3)Temperature of HC! (C)Experiment 32lumps0,225Experiment 42lumps1,025 6.2.1Identify the independent variable in this investigation.(1) 6.2.2Write down a hypothesis for this investigation.(2) 6.2.3Is it fair to compare results obtained in Experiment 3 with that in Experiment 4? Give a reason for the answer.(2) 6.2.4The reactions in Experiments 3 and 4 both run to completion. How will the yield of CO2(g) in Experiment 3 compare to that in Experiment 4? Write down only LARGER THAN, SMALLER THAN or EQUAL TO and give a reason for the answer.(2) 6.3INVESTIGATION C: The learners conduct two experiments using the conditions as shown in the table below. Mass of CaCO3 (g)State of CaCO3Concentration of HC! (mol"dm-3)Temperature of HC! (C)Experiment 54powder0,225Experiment 64powder0,235 6.3.1How does the average kinetic energy of the particles in the reaction in Experiment 5 compare to that in Experiment 6? Write down only HIGHER THAN, LOWER THAN or EQUAL TO.(1) 6.3.2On the same set of axes, draw sketch graphs of the number of molecules versus the kinetic energy (Maxwell-Boltzmann distribution curves) for each of Experiment 5 and Experiment 6. Label the axes. Clearly label each graph as Experiment 5 or Experiment 6.(3) 6.4The graph below shows changes in the potential energy for the reaction between calcium carbonate and hydrochloric acid. 6.4.1Is this reaction endothermic or exothermic? Give a reason for the answer.(2) 6.4.2Use the relevant energy values, A, B and C, to write down an expression for each of the following: (a)The energy of the activated complex(1) (b)"H for the forward reaction(1) [20] QUESTION 7 (Start on a new page.) Fertilisers allow farmers to grow crops in the same soil year after year. However, environmental problems, such as eutrophication, are associated with the application of fertilisers. 7.1State ONE PRECAUTION that a maize farmer can take to prevent eutrophication.(1) Nitric acid is an important reactant in the production of ammonium nitrate, a nitrogen-based fertiliser. 7.2Write down the name of the industrial process for the production of nitric acid.(1) 7.3Write down a balanced equation for the preparation of ammonium nitrate from nitric acid.(3) A fertiliser company produces ammonia on a large scale at a temperature of 450C. The balanced equation below represents the reaction that takes place in a sealed container. N2(g) + 3H2(g) ! 2NH3(g) "H < 0 To meet an increased demand for fertiliser, the management of the company instructs their engineer to make the necessary adjustments to increase the yield of ammonia. In a trial run on a small scale in the laboratory, the engineer makes adjustments to the TEMPERATURE, PRESSURE and CONCENTRATION of the equilibrium mixture. The graphs below represent the results obtained.            7.4Identify the changes made to the equilibrium mixture at each of the following times: 7.4.1t1(2) 7.4.2t2(2) 7.4.3t3(2) 7.5At which of the above time(s) did the change made to the reaction mixture lead to a higher yield of ammonia? Write down only t1 and/or t2 and/or t3.(2) 7.6The engineer now injects 5 mol N2 and 5 mol H2 into a 5 dm3 sealed empty container. Equilibrium is reached at 450 C. Upon analysis of the equilibrium mixture, he finds that the mass of NH3 is 20,4 g. Calculate the value of the equilibrium constant (Kc) at 450 C . (9) [22] QUESTION 8 (Start on a new page.) The diagram below represents a galvanic (voltaic) cell functioning under standard conditions with magnesium and silver as electrodes. A voltmeter connected across the electrodes shows an initial reading of 3,17 V.  8.1State the energy conversion that takes place in this cell.(2) 8.2State TWO standard conditions under which this cell operates.(2) 8.3Identify the anode of this cell. Refer to the relative strength of reducing agents to explain how you arrived at the answer.(3) 8.4Write down the cell notation (symbolic notation) of this cell.(3) 8.5Write down the balanced equation for the net (overall) cell reaction that takes place in this cell. Omit the spectator ions.(3) 8.6How will an increase in the concentration of the Ag+ ions influence the current that the cell delivers? Write down only INCREASES, DECREASES or REMAINS THE SAME and explain the answer. (3) [16] QUESTION 9 (Start on a new page.) Electroplating is one of the uses of electrolysis. The diagram below shows an electrolytic cell that can be used to plate a copper spoon with silver.           9.1Define the term oxidation in terms of electron transfer.(2) 9.2What type of half-reaction takes place at the copper spoon? Write down only OXIDATION or REDUCTION.(1) 9.3Write down a half-reaction that explains the change that occurs on the surface of the copper spoon during electrolysis.(2) 9.4Name the metal that is labelled 'electrode'.(1) 9.5Give a reason why the concentration of the AgNO3(aq) remains constant during electrolysis. (2) [8] QUESTION 10 (Start on a new page.) A lead-acid battery (car battery) consists of six cells and has a battery capacity of 20 A"h. The half-reactions that take place in each cell and their respective standard reduction potentials are represented below: PbSO4(s) + H+(aq) + 2e-! Pb(s) + HSO4-(aq) E = -0,36 V PbO2(s) + 3H+(aq) + HSO4-(aq) + 2e-! PbSO4(s) + 2H2O(!) E = 1,7 V 10.1Are car batteries primary or secondary batteries?(1) 10.2Write down the equation for the net (overall) cell reaction that takes place in each cell of this battery.(3) 10.3Calculate the emf of the BATTERY, consisting of six cells, under standard conditions.(5) 10.4Calculate the maximum time that this battery will be able to supply a constant current of 5 A to an appliance connected to it. Assume that the capacity of the battery remains constant.(4) 10.5State TWO environmental risks associated with the irresponsible disposal of lead-acid batteries. (2) [15] TOTAL SECTION B: GRAND TOTAL:125 150 DATA FOR PHYSICAL SCIENCES GRADE 12 PAPER 2 (CHEMISTRY) GEGEWENS VIR FISIESE WETENSKAPPE GRAAD 12 VRAESTEL 2 (CHEMIE) TABLE 1: PHYSICAL CONSTANTS/TABEL 1: FISIESE KONSTANTES NAME/NAAMSYMBOL/SIMBOOLVALUE/WAARDEStandard pressure Standaarddruk EMBED Equation.3 1,013 x 105 PaMolar gas volume at STP Molre gasvolume by STDVm22,4 dm3"mol-1Standard temperature Standaardtemperatuur EMBED Equation.3 273 K TABLE 2: FORMULAE/TABEL 2: FORMULES  EMBED Equation.3  EMBED Equation.3  or/of  EMBED Equation.3 q = I EMBED Equation.3 t W = Vq EMBED Equation.3  /  EMBED Equation.3  or/of  EMBED Equation.3  /  EMBED Equation.3  or/of  EMBED Equation.3  /  EMBED Equation.3  TABLE 3: THE PERIODIC TABLE OF ELEMENTS 1 (I)2 (II)3  4 5 6  7 8 9 10 11 12 13 (III)14 (IV)15 (V)16 (VI)17 (VII)18 (VIII)2,11 H 12 He 41,03 Li 71,54 Be 92,05 B 112,56 C 123,07 N 143,58 O 164,09 F 1910 Ne 200,911 Na 231,212 Mg 241,513 A! 271,814 Si 282,115 P 312,516 S 323,017 C! 35,518 Ar 400,819 K 391,020 Ca 401,321 Sc 451,522 Ti 481,623 V 511,624 Cr 521,525 Mn 551,826 Fe 561,827 Co 591,828 Ni 591,929 Cu 63,51,630 Zn 651,631 Ga 701,832 Ge 732,033 As 752,434 Se 792,835 Br 8036 Kr 840,837 Rb 861,038 Sr 881,239 Y 891,440 Zr 9141 Nb 921,842 Mo 961,943 Tc 2,244 Ru 1012,245 Rh 1032,246 Pd 1061,947 Ag 1081,748 Cd 1121,749 In 1151,850 Sn 1191,951 Sb 1222,152 Te 1282,553 I 12754 Xe 1310,755 Cs 1330,956 Ba 13757 La 1391,672 Hf 17973 Ta 18174 W 18475 Re 18676 Os 19077 Ir 19278 Pt 19579 Au 19780 Hg 2011,881 T! 2041,882 Pb 2071,983 Bi 2092,084 Po 2,585 At 86 Rn 0,787 Fr 0,988 Ra 22689 Ac 58 Ce 14059 Pr 14160 Nd 14461 Pm 62 Sm 15063 Eu 15264 Gd 15765 Tb 15966 Dy 16367 Ho 16568 Er 16769 Tm 16970 Yb 17371 Lu 17590 Th 23291 Pa 92 U 23893 Np 94 Pu 95 Am 96 Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr TABEL 3: DIE PERIODIEKE TABEL VAN ELEMENTE TABLE 4A: STANDARD REDUCTION POTENTIALS TABEL 4A: STANDAARD- REDUKSIEPOTENSIALE Half-reactions/Halfreaksies EMBED Equation.3  (V)F2(g) + 2e(!2F(+ 2,87Co3+ + e(!Co2++ 1,81H2O2 + 2H+ +2e(!2H2O+1,77MnO EMBED Equation.3  + 8H+ + 5e(!Mn2+ + 4H2O+ 1,51C!2(g) + 2e(!2C!(+ 1,36Cr2O EMBED Equation.3  + 14H+ + 6e(!2Cr3+ + 7H2O+ 1,33O2(g) + 4H+ + 4e(!2H2O+ 1,23MnO2 + 4H+ + 2e(!Mn2+ + 2H2O+ 1,23Pt2+ + 2e(!Pt+ 1,20Br2(!) + 2e(!2Br(+ 1,07NO EMBED Equation.3  + 4H+ + 3e(!NO(g) + 2H2O+ 0,96Hg2+ + 2e(!Hg(!)+ 0,85Ag+ + e(!Ag+ 0,80NO EMBED Equation.3  + 2H+ + e(!NO2(g) + H2O+ -./>ef   $ yri_XQryryr hy5^J h/ 5^Jh<aJmH sH hDu5mH sH  hDu5^J hDu\^JhDuhDu5\^Jh<mH sH hWEmH sH  h\H5\hWEmH sH hWE5\aJhWE5PJ\ hWE5\hWECJ PJmH sH jhWECJ$UmHnHu hWECJ$&jhWECJUaJmHnHsH u hWEaJ     $a$gdWEgdWE  9r gdWE~ !"./>?@ABCD $Ifgdf.(gdDu$a$gdWEgdWEgdWE" # P Q  [ $ $Ifa$gdf.( $Ifgdf.([ \ SQOkd$$Ifl\S$x%(9!0f)4 la $Ifgdf.($ $Ifa$gdf.(    ! 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Equation.3  + 4H+ + 2e(!SO2(g) + 2H2O+ 0,17Cu2+ + e(!Cu++ 0,16Sn4+ + 2e(!Sn2++ 0,15S + 2H+ + 2e( !H2S(g)+ 0,142H+ + 2e(!H2(g)0,00Fe3+ + 3e(!Fe( 0,06Pb2+ + 2e(!Pb( 0,13Sn2+ + 2e(!Sn( 0,14Ni2+ + 2e(!Ni( 0,27Co2+ + 2e(!Co( 0,28Cd2+ + 2e(!Cd( 0,40Cr3+ + e(!Cr2+( 0,41Fe2+ + 2e(!Fe( 0,44Cr3+ + 3e(!Cr( 0,74Zn2+ + 2e(!Zn( 0,762H2O + 2e(!H2(g) + 2OH(( 0,83Cr2+ + 2e(!Cr( 0,91Mn2+ + 2e(!Mn( 1,18A!3+ + 3e(!A!( 1,66Mg2+ + 2e(!Mg( 2,36Na+ + e(!Na( 2,71Ca2+ + 2e(!Ca( 2,87Sr2+ + 2e(!Sr( 2,89Ba2+ + 2e(!Ba( 2,90Cs+ + e-!Cs- 2,92K+ + e(!K( 2,93Li+ + e(!Li( 3,05TABLE 4B: STANDARD REDUCTION POTENTIALS TABEL 4B: STANDAARD- REDUKSIEPOTENSIALE Half-reactions/Halfreaksies EMBED Equation.3  (V)Li+ + e(!Li( 3,05K+ + e(!K( 2,93Cs+ + e(!Cs( 2,92Ba2+ + 2e(!Ba( 2,90Sr2+ + 2e(!Sr( 2,89Ca2+ + 2e(!Ca( 2,87Na+ + e(!Na( 2,71Mg2+ + 2e(!Mg( 2,36A!3+ + 3e(!A!( 1,66Mn2+ + 2e(!Mn( 1,18Cr2+ + 2e(!Cr( 0,912H2O + 2e(!H2(g) + 2OH(( 0,83Zn2+ + 2e(!Zn( 0,76Cr3+ + 3e(!Cr( 0,74Fe2+ + 2e(!Fe( 0,44Cr3+ + e(!Cr2+( 0,41Cd2+ + 2e(!Cd( 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Mar. 2011 NSC Copyright reserved Please turn over Copyright reserved Please turn over Physical Sciences/P2  PAGE 16 DBE/Feb. Mar. 2011 NSC Copyright reserved PAGE  Physical Sciences/P2  PAGE 4 DBE/Feb. Mar. 2011 NSC Copyright reserved Physical Sciences/P2  PAGE 1 DBE/Feb. Mar. 2011 NSC Copyright reserved Please turn over Physical Sciences/P2  PAGE 2 DBE/Feb. Mar. 2011 NSC Copyright reserved Physical Sciences/P2  PAGE 4 DBE/Feb. Mar. 2011 NSC Copyright reserved Physical Sciences/P2  PAGE 3 DBE/Feb. Mar. 2011 NSC Copyright reserved Please turn over PHYSICAL SCIENCES: CHEMISTRY (P2) FEBRUARY/MARCH 2011 NATIONAL SENIOR CERTIFICATE salt bridge H H H O C GRAAD 12 H C H C H Atomic number Atoomgetal 29 Cu 63,5 1,9 Symbol Simbool Electronegativity Elektronegatiwiteit Approximate relative atomic mass Benaderde relatiewe atoommassa KEY/SLEUTEL copper spoon Cu Cu H CH3 C C C C Increasing reducing ability/Toenemende reduserende vermo Increasing oxidising ability/Toenemende oksiderende vermo H Increasing reducing ability/Toenemende reduserende vermo Mg2+(aq) Increasing oxidising ability/Toenemende oksiderende vermo CH3 H H H H CH3 B t1 NH3 Ag+(aq) H2 N2 Time (minutes) H Mg(s)  H ^bz$$M&#$/Ifa$$$M&#$/Ifa$$$M&#$/Ifa$^`fjtvƨȨ̨Шبڨܨި,.8:>@کʸhtNCJmH sH hjhUjh<UmHnHsH uh< j-h<CJH*^JaJh<CJaJh<CJH*^JaJh<CJH*^JaJh<CJ^JaJh<CJOJQJ^JaJ7YG5$$M&#$/Ifa$$$M&#$/Ifa$kd$$Ifl4\   6M064 laf4ƨȨ5kd$$Ifl4\   6M064 laf4$$M&#$/Ifa$$$M&#$/Ifa$Ȩܨ$$M&#$/Ifa$$$M&#$/Ifa$$$M&#$/Ifa$YG5$$M&#$/Ifa$$$M&#$/Ifa$kdW$$Ifl4\   6M064 laf4,.05* $$ !a$kd$$Ifl4\       6M064 laf4$$M&#$/Ifa$$$M&#$/Ifa$02468<>BDFHJLNPRTVXZ\^`bdfhjl $$ !a$lnprtvxz|~ $$ !a$9:ab$a$gdtN&`#$  9r %gdT r %  r %gdtNgds  9r %gdtNکܩ &(.9:abwx~Ⱦȱwjww`SOhf.(hThTCJmH sH hT0JCJaJhtNhT0JCJaJ!jhtNhT0JCJUaJhTCJmH sH htNCJaJh2-CJaJhibh2-CJaJh2-htNhtNCJmH sH h2-0JCJaJhtN0JCJaJh70JCJaJmHnHuhtNhtN0JCJaJ!jhtNhtN0JCJUaJҪӪ٪ڪ۪ܪ   !"()*+EFGYZklŸũşŸsşf\ŸhtNCJmH6sH6htNh2-CJmH sH h70JCJaJmHnHu h2-CJh2-CJmH6sH6htNhtNCJmH sH htN0JCJaJhtN0JCJaJmHnHuhtNhtN0JCJaJ!jhtNhtN0JCJUaJhtNCJmH sH h2- h2-0Jjh2-0JUhf.(hTCJaJ$  AFGkl  ?DE  9r %;  9r %gdtN  9r n<gdtN  9r &;gdtN  9r %gdtN 9r l(Ыѫ׫ث٫ګ   &'()CDE{|}~ĺĦߙՌߙİzvpe]hWECJaJhn7hWECJaJ hWECJhh2-mH6sH6 htNCJhf.(htNhtNCJmH sH htNhtN0JCJaJhtNCJmH sH h2-CJmH6sH6htNCJmH6sH6h2-htNh2-CJmH sH htN0JCJaJ!jhtNhtN0JCJUaJh70JCJaJmHnHu$E|}~ӬԬլ֬׬ج٬ڬ۬ܬݬެ߬gdgdh+$a$gdWE 9r ;ҬӬ"#$/0123457BCD^ghijklmnopqrstuvwҭ¾¾¾¾¾¾¾¾񩕩񩞏 h2-aJh2-5CJ aJ h2-56mH6sH6 h2-5 h3phn h3phn ^Jhn hn B*^JphhZ3hp5CJaJhD5CJaJ hWECJ hWEB*CJ phh2-hn7hWECJaJ5   gdp    !"$%&'(gd()*+,-./1245789:;<=>?@ABDEFGH$a$gdHIJKLMNOPQRSTUVWXYZ[\]^ghjkgd$a$gdWE$a$gdNEPkmnpqstvwӭ ()$a$gdҭӭ '()-457DGHKLOPQR_`abcdefghijklopqr鹵髡髓髓鉅鉅~sh2-5^JmH sH  h2-5^Jhn hn B*^Jphhph^=h^=H*^Jh^=B*^JphhpB*^JphhO{[hO{[B*^Jphhq h N5hhb6hx5h2-56aJmH6sH6 h2-5h2-h2-56mH6sH6 h2-5aJ()567DEFGKLOPRSTUVWXYZ[\]^_cdgdpgdzgdOdfgijlmnoqr,-.7gdpgdz$a$gdgdpɮʮ +,.027:VWtuⶨ➔ↂↂↂ➔hn hn B*^Jphh^=h]&h^=H*^Jh^=B*^JphhZ3hp5CJH*aJhZ3hp5CJaJhO{[hO{[B*^Jphh2-5^JmH sH  h2-5^Jh2-h2-56^JmH sH h2-56^JmH6sH6-789:uvwxyz{|}~$a$gd +gdgdzgdpȯɯʯ˯̯ίϯЯѯӯԯٯگۯܯݯޯ߯߿ߩߗ߿vjߗhUhhp5CJaJ jLjhh5CJUaJhh5CJaJhO{[hO{[B*^JphhB5h\5hB5hyh5hZ3hp5CJH*aJhZ3hp5CJaJhDh\5H*^JhDh\5h2-h%Dh +5CJ^JaJh%Dht65CJ^JaJ(¯ïįůƯǯȯ˯̯Яѯٯگݯgdpgd\ݯޯ "$&*,24:<gdpgdpgdzgd\ H Ag(s) O H 0 C! 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