Physical Sciences Grade 12 P2 North West November 2015 QP

Downloaded from hlayiso.com Education and Sport Development Department of Education and Sport Development Departement van Onderwys en Sportontwikkeling Lefapha la Thuto ie Tihabololo ya Metshameko NORTH WEST PROVINCE NATIONAL SENIOR CERTIFICATE MARKS: 150 TIME: 3 hours This question paper consists of 14 pages, 4 data sheets and 1 graph sheet. Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 2 NW/September 2015 NSC INSTRUCTIONS AND INFORMATION 1. 2. 10. 11. 12. Write your name in the appropriate space on your ANSWER BOOK. This question paper consists of TEN questions. Answer ALL the questions in the ANSWER BOOK, except for QUESTION 6.3 which should be answered on the included GRAPH SHEET. Write your name on this sheet in the space provided and insert it inside the back cover of your ANSWER BOOK. Start EACH question on a NEW page in the ANSWER BOOK. Number the answers correctly according to the numbering system used in this question paper. Leave ONE line between two subquestions, for example between QUESTION 2.1 and QUESTION 2.2. You may use a non-programmable calculator. You may use appropriate mathematical instruments. You are advised to use the attached DATA SHEETS. Show ALL formulae and substitutions in ALL calculations. Round off your final numerical answers to a minimum of TWO decimal places. Give brief motivations, discussions, et cetera where required. Write neatly and legibly. Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 3 NW/September 2015 NSC QUESTION 1: 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 (1.1-1.10) in the ANSWER BOOK, for example 1.11 D. 1.1. Consider the organic compounds below: (i) CsHs (ii) CsHy2 Which ONE of the following statements does NOT apply to these compounds? They ... A B Cc D both burn in oxygen. are both unsaturated. are both alkanes. are both hydrocarbons. (2) 1.2 TWO isomers of CsHi2 and their respective boiling points are shown below: an dy HoH HOH qa 4H | H—O—C——_H Boiling point = 27,8 °C H I Boiling point = 9,5 °C Which ONE of the following statements is CORRECT about the structural formula of compound Q above? it has: A B Cc D Less side chains and weaker intermolecular forces More side chains and weaker intermolecular forces Less side chains and greater intermolecular forces More side chains and greater intermolecular forces (2) Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 NW/September 2015 4 NSC 1.3 Activation energy can best be described as the minimum energy required to ... A make reactant molecules to collide. cause effective collisions. B Cc change the orientation of reactant molecules. D increase the kinetic energy of reactant molecules. (2) 1.4. Which ONE of the following reaction conditions is suitable for the dehydrohalogenation of haloalkanes? A No water should be present B Presence of the catalyst H2SO, Cc Strongly heated under reflux with ethanolic KOH/NaOH D React with aqueous sodium hydroxide or potassium hydroxide (2) 1.5 The table below shows pH ranges of some indicators in acid and basic solutions. INDICATORS pH RANGES Methy! orange 3,1-4,4 Methyl red 4,2-6,2 Bromothymol blue 6,0—7,8 Phenolphthalein 8,3 - 10,0 The indicator best suited for the titration of ethanoic acid against a solution of sodium hydroxide, is ... A _ methyl orange. B methyl red. C _bromothymol blue. D___ phenolphthalein. (2) 1.6 Which ONE of the following is the correct balanced equation for the combustion of sulphur (IV) dioxide? A 2802(g) + 202(g) — 2S0s(g) B 2S02(g) + 202(g) — SOsa(g) C S02(g) + 202(g) + 25802(g) D 280,(g) + O2(g) ~ 250s(9) (2) Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 5 NW/September 2015 NSC 1.7. Consider the following redox reaction: H2S(g) + 2FeCls(aq) —> 2FeClo(aq) + S(s) + 2HCl(aq) The oxidation half-reaction for the above reaction is ... HS — S+2H*+2e. Fe*+e — Fe. S$+2H*+2e -» HS. 50 0O DBD > Cl + 2e — 2Cr. (2) 1.8 Astrip of magnesium metal is placed in a zinc sulphate (ZnSOxz) solution. ZnSO, (aq) The reaction that takes place is represented by the equation below: Mg(s) + ZnSO.(aq) —> MgSO,(g) + Zn(s) According to the above reaction ... A Zn is the oxidising agent. B Mg is the oxidising agent. Cc Mg is reduced. D —_Znis oxidised. (2) Copyright reserved Please turn over

Physical Sciences/P2 1.9 Downloaded from hlayiso.com 6 NW/September 2015 NSC The following reversible reaction reaches equilibrium in a closed container: Hog) + bg) = 2HI(g) AH <0 Equilibrium was first established after 5 minutes. (The broken line represents the reverse reaction.) Rate of reaction > Time (minutes) 0 5 10 15 20 What change in the conditions was made at t = 10 minutes to cause the rate of both the forward and the reverse reactions to increase by the same amount? A Temperature was increased B A catalyst was added Cc Temperature was decreased D Pressure was increased 1.10 Which ONE of the following terms is TRUE about sulphuric acid? A Dilute acid B Weak acid Cc Diprotic acid D Triprotic acid [20] Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 NW/September 2015 7 NSC QUESTION 2 (Start on a new page.) Study the following organic compounds, represented by the letters A to F in the table below: H O 48 H H A ~“ —~ Propanoic acid H—C— r | OH H H \ H A B c ik I H 0 it OH H | | | | | H—C—C— HH) a—c—c— 0—C— Fa 1 r 1 H H H H H H HA D E F 2.1 Define the term functional isomers. (2) 2.2 Identify TWO FUNCTIONAL ISOMERS. Only write down the corresponding LETTERS for the correct answers. (2) 2.3 Compound B and C react in the presence of an organic acid. 2.3.1 Write down the structural formula of the main organic product. (2) 2.3.2 Name the ORGANIC product. (1) 2.4 Compound C undergoes an ELIMINATION reaction in the presence of concentrated sulphuric acid. Use structural formulae to write down a balanced equation for the reaction. (3) 2.5 Name the: 2.5.1 Specific type of ELIMINATION reaction taking place in QUESTION 2.4 (1) 2.5.2 Organic PRODUCT formed (1) 2.6 Write down the following: 2.6.1 The IUPAC name of compound A (2) 2.6.2 The homologous series to which compound D belongs (1) [15] Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 8 NW/September 2015 NSC QUESTION 3 (Start on a new page.) The table shows the data collected for three organic compounds A, B and C, with different functional groups, during a practical investigation. COMPOUND MELTING POINTS (°C) B CHsCH2OH -114 Cc CH3COOH 16,6 3.1. Name the following in this investigation: 3.1.1. The independent variable 3.1.2 The dependent variable 3.1.3 The control variable 3.2 Write down the homologous series to which compound C belongs. 3.3. Write down the general formula for compound A. 3.4 Describe the trend in the melting points from A to C, as shown in the table. 3.5 Explain the trend in QUESTION 3.4 above. Make reference to INTERMOLECULAR FORCES and ENERGY involved. QUESTION 4 (Start on a new page.) 41 A sample of the compound 2-bromo-2-methylpropane is dissolved in ethanol in the presence of diluted potassium hydroxide. 4.1.1. Write down the structural formula of 2-bromo-2-methylpropane. 4.1.2 Using structural formulae only, write a balanced equation for the reaction in QUESTION 4.1.1. 4.1.3 Indicate TWO reaction conditions for this chemical reaction. 4.1.4 Name the type of reaction that occurs in QUESTION 4.1.2. Copyright reserved Please turn over (1) (1) (1) (2) (2) (2) (5) [14] (3) (2) (2)

Downloaded from hlayiso.com Physical Sciences/P2 9 NW/September 2015 NSC 4.2 Polymers are large molecules consisting of repeating monomer units. 4.3 4.4 4.2.1 What is a condensation polymer? 4.2.2 Write down the structural formula for the monomer from which polyvinyl chloride is derived. 4.2.3 Give the name of the monomer. Classify the following as addition or condensation polymers: 4.3.1 Polyester 4.3.2 Polyvinylchloride State ONE use of polyvinyl chloride. QUESTION 5 (Start on a new page.) 5.1 5.2 5.3 5.4 Define an acid in terms of the Bronsted-Lowry theory. Consider the reaction below: HF + Hs0 # HgO* + F 6.2.1 Identify the reactant which acts as a Bronsted-Lowry base. 5.2.2 Write down the formula of the conjugate acid of the base identified in QUESTION 5.2.1. Sulphuric acid (H2SOx) is a strong acid. 5.3.1 Explain why sulphuric acid is considered a strong acid. 5.3.2 Calculate the pH of a 0,025 mol.dm® sulphuric acid solution. A certain solution X, has a pH of 12,8. 5.4.1. Which of the ions, OH’ or H* is in excess? 5.4.2 Acetic acid (CH3COOH) is added to solution X. Is the pH of the (2) (2) (2) (1) (1) (1) [18] (2) (1) (1) (2) (4) (1) solution going to INCREASE, DECREASE or REMAINS THE SAME? Copyright reserved Please turn over (1)

Downloaded from hlayiso.com Physical Sciences/P2 10 NW/September 2015 NSC 5.5 A learner accidentally spills 15 em? of 0,4 mol.dm® sulphuric acid solution in the laboratory. He adds 25 em? of 0,2 mol.dm? of sodium hydroxide to the spilled sulphuric acid in an attempt to neutralise it. The equation for the reaction is given below: H2SO4, + 2NaOQH — NaeSO4 + 2H20 Show by calculations that the addition of the sodium hydroxide solution will not neutralise the sulphuric acid spill. (6) [18] QUESTION 6 (Start on a new page.) The apparatus below is being used to investigate the effect of a certain factor on the rate of reaction of calcium carbonate powder and calcium carbonate chunks with a diluted hydrochloric acid solution. A known mass of calcium carbonate powder was added to an excess of diluted hydrochloric acid and the decrease in mass over a certain time interval was recorded. Readings were taken at 30 second intervals. The procedure was then repeated, this time using ‘chunks’ of the calcium carbonate. <+——— Beaker 6 o Hydrochloric acid CaCO; Chemical balance Experiment A: Reaction of calcium carbonate powder and hydrochloric acid Time (s) 0 | 1,0 | 2,0 | 30 | 4,0 | 5,0 | 6,0 | 7,0 Mass of calcium carbonate powder (g) 92 | 91,1 | 90,4 | 90,1 | 90 90 | 90 | 90 Decrease in mass (g) 0|09;}16/ 19 | 20 | 2,0 | 2,0 | 2,0 Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 1 NW/September 2015 NSC Experiment B: Reaction of calcium carbonate chunks and hydrochloric acid Time (s) 0 | 1,0 | 2,0 | 3,0 | 4,0 | 5,0 | 6,0 | 7,0 Mass of calcium carbonate chunks (g) 92 | 91,4} 91 | 90,6 | 90,3 | 90,1 | 90 | 90 Decrease in mass (g) 0105 /11,0; 1,4 | 1,7 | 1,9 | 20/20 6.1. Formulate an investigative question for this investigation. (2) 6.2 Write down a balanced chemical equation for the reaction between calcium carbonate and diluted hydrochloric acid. (3) 6.3 Using the tables above, draw TWO graphs on the GRAPH SHEET comparing the decrease in mass versus time for each of experiments A and B. Use the same set of axes and label the graphs A and B respectively. (6) 6.4 Which reaction reaches completion first? (1) 6.5 How does the loss in mass compare after the completion of both reactions? (1) 6.6 What conclusion can be drawn from this investigation? (2) [15] QUESTION 7 (Start on a new page.) Study the reversible reaction represented by the balanced equation below: Ho(g) + CO2(g) = H2O(g) + CO(g) Initially X moles of H2(g) is mixed with 0,3 moles of CO2(g) in a sealed 10 dm? container. When equilibrium was reached, the concentration of CO was 0,0: 7A 7.2 7.3 2 mol. dm and the equilibrium constant (K.) at that specific temperature was 4. State Le Chatelier’s principle. (2) Calculate the initial number of moles X of H2(g) that was in the container. (8) The reaction is now carried out at a much higher temperature. It is found that the value of K, decreases at this higher temperature. Is the forward reaction EXOTHERMIC or ENDOTHERMIC? Explain your answer. (4) [14] Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 12 NW/September 2015 NSC QUESTION 8 (Start on a new page.) The diagram represents a galvanic cell (A). A small light bulb connected in the external circuit glows brightly. Ni — [~~ Ag Ne) — —As'en porous plug 8.1. | State TWO conditions under which this cell will be a standard cell. (2) 8.2. Give the equation for the reaction which occurs at the Ag/Ag* half-cell. (2) 8.3. Which electrode is the anode? (1) 8.4. What happens to the emf of the cell as it continues to deliver current? (1) 8.5. Write down the overall reaction for this cell. (3) 8.6 If 0,4 moles of electrons flow to the cathode, what will be the decrease in mass of the anode? (3) 8.7. ASECOND galvanic cell (B) is constructed using: Mg(s) in Mg(NOs)2(aq) and Ag(s) in AgNO3(aq) Without any calculations, determine which of the TWO galvanic cells (A or B) will result in the highest potential difference. Explain your answer by referring to the relative strengths of the two reducing agents as well as the relative strengths of the two oxidising agents involved. (3) [15] Copyright reserved Piease turn over

Downloaded from hlayiso.com Physical Sciences/P2 13 NW/September 2015 NSC QUESTION 9 (Start on a new page.) Copper metal can be purified by electrolysis, using the cell shown below. 9.1 9.2 9.3 9.4 9.5 battery P te} CuS80,(aq) Define the term electrolysis. (2) Which electrode, P or Q, consists of the impure copper? Explain your answer. (3) Write down the half-cell reaction that takes place at electrode Q. (2) Explain why the concentration of the copper (II) sulphate solution remains constant if the only impurities are silver and platinum. (2) State TWO uses of copper. (2) [11] Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 14 NW/September 2015 NSC QUESTION 10 (Start on a new page.) Study the diagram below, illustrating the industrial preparation of nitric acid. NH3 A + H,0 Oz Oz; H20 Cc Oo. —— 10.1. Write down a balanced equation for the formation of product A. (3) 10.2 Name the catalyst used during the reaction in QUESTION 10.1. (1) 10.3. What NAME is given to the reaction in QUESTION 10.1? (2) 10.4 Give the FORMULA of product C. (1) 10.5 Name the process used to produce product C. (1) 10.6 Fertilisers enable plants to grow better and faster, thus improving food production. However, deficiency or excess of primary nutrients in plants can be detrimental to the environment and humans. State any TWO symptoms of a deficiency of Potassium as a primary nutrient in plants. (2) [10] TOTAL: 150 Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 15 NSC NW/September 2015 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/NAAM SYMBOL/SIMBOOL | VALUE/WAARDE TABLE 2: FORMULAE/TABEL 2: FORMULES m N n=— n=— M Na n m Vv -— /of = n=— c Vv or/o c MV v, Ca _ Ma =- * CyVy Ny pH = -log[H30*] Kw = [HgO*][OH]] = 1 x 10° at/by 298 K cell ‘oxidising agent reducing agent reduksie =a = Eathode - Erode / Fea = Eatode or/of a = Feuction ~ Fe vdation / Eee = = or/of Ee, =E° — Ee ~ Ee ‘anode ) ~ E ocsidasie 6 _ fe / Ee 7 E oksideermiddel — Ee reduseermiddel Copyright reserved Please turn over

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Downloaded from hlayiso.com Physical Sciences/P2 Increasing oxidising ability/ Toenemende oksiderende vermoé Copyright reserved NW/September 2015 Increasing reducing ability/Toenemende reduserende vermoé 17 NSC TABLE 4A: STANDARD REDUCTION POTENTIALS Half-reactions/Halfreaksies E® (v) Fpg)+2e = 2F + 2,87 Co*+e = Co* + 1,81 H202 + 2H*+2e = 2H2O +1,77 MnO] +8H*+5e7 = Mn™*+4H,O | +1,51 Ch(g)+2e = 2Cr + 1,36 cro” +14H*4+6e7 = 2Cr*+7H,0 + 1,33 O2(g)+4H*+4e7 = 2H20 + 1,23 MnO2+4H*+2e° = Mn*+2H20 + 1,23 PPt+2e Pt +1,20 Br(f)+2e = 2Br + 1,07 NO, +4H*+3e = NO(g)+2H20 | +0,96 Hg**+2e7 = Hg(2) + 0,85 Agi+e = Ag + 0,80 NO3 +2H*+e" = NO2(g)+H2O + 0,80 Fe*+e° = Fe +0,77 On(g) + 2H*+2e° = H2O2 + 0,68 lbt+2e = 2 + 0,54 Cutt+e° = Cu + 0,52 SO2+4H*+4e7° = S+2H20 + 0,45 2H20+O24+4e = 40H” + 0,40 Cu*+2e = Cu + 0,34 S04 +4H*+2e° = SO2(g)+2H20 | +0,17 Cu*+e = Cut + 0,16 Sn¥+2e° = Sn* +0,15 S+2H*+2e = H2S(g) + 0,14 2H*+2e" = H2(g) 0,00 Fe*+3e = Fe — 0,06 Pb**+2e° = Pb -0,13 Sn**+2e° = Sn ~ 0,14 Ni*+2e = Ni -0,27 Co*+2e° = Co ~ 0,28 Cd*+2e =. Cd ~0,40 Crt+e = Crt ~0,41 Fe+2e = Fe - 0,44 Crt+3e" = Cr ~0,74 Zn**42e = Zn - 0,76 2H20+2e7 = Ha(g) + 20H~ — 0,83 Cret+20 = Cr - 0,91 Mn**+2e = Mn —1,18 Abt+3e = At ~ 1,66 Mg*+2e = Mg ~ 2,36 Nat+e = Na -2,71 Ca*+2e = Ca — 2,87 SP*+2e = Sr - 2,89 Ba’t+2e = Ba - 2,90 Cs'+e = Cs + 2,92 Kr+e7 = K ~ 2,93 lite = Li — 3,05

Downloaded from hlayiso.com Physical Sciences/P2 1 Bo NW/September 2015 N TABLE 4B: STANDARD REDUCTION POTENTIALS Half-reactions/Halfreaksies E® (vy) litte = Li ~ 3,05 KY+e = K ~2,93 Cs*+e@ = Cs - 2,92 Ba*+2e = Ba — 2,90 SP+2e = Sr — 2,89 Ca*+2e = Ca ~ 2,87 Nat+e> = Na 2,71 Mg’*+2e = Mg — 2,36 Aft 430 = AL ~1,66 4 Mn*+2e = Mn ~1,18 ‘9 Crt+2e = Cr -0,91 = 2H20+2e = H2(g) +20H™ ~ 0,83 3 Zn*+2e = Zn 0,76 9 > Cr*+3e = Cr ~0,74 & 3 Fe4+2e" = Fe - 0,44 g g ce+e = Cr ~0,41 g 3 Cd*+2e = Cd — 0,40 2 3 Co%*+2e = Co ~ 0,28 eo $s Net42e = Ni ~0,27 8 8 Sn*+2e = Sn ~ 0,14 3 5 Pb 42e" 2 Pb -0,13 2 & Fe+3e = Fe ~ 0,06 3 2 2H*+2e = Hig) 0,00 § 8 S+2H'+2e = HAS(g) +0,14 £ Led Sn*+2e = Sn* + 0,15 2 £ Cut+e" = Cut + 0,16 e s SOF +4H"+2e° = SO2(g)+2H.O| +0,17 > > Cu%+2e = Cu +0,94 = ‘3 2H20+02+4e = 40H +0,40 o 3 SQ2+4H*+4e° = ~S+2H,0 + 0,45 > 3 Cuv+e = Cu + 0,52 ‘Oo > b+2e = at +0,54 3 7 O2(g) + 2H*+2e == H2O2 + 0,68 = $ Fe*+e = Fe* +0,77 > g NO3 +2H*+e = NOx(g)+H20 | +0,80 9 ~y Agit+e = Ag + 0,80 5 Hg*+2e = Hg(t) + 0,85 £ NO; +4H*+3e = NO(g)+2H20 | +0,96 Br(t)+2e° = 2Br + 1,07 Pht+2e = Pt +1,20 MnO2+ 4H? +2e° = Mn®*+2H2O +1,23 O2(g)+4H*+4e = 2H2O + 1,23 cro? +14H*+6e = 2Cr*+7H20 + 1,33 C(g)+2e = 200 + 1,36 MnO, +8H*+5e = Mn**+4H,0 +1,51 H2O2 + 2H*+2e = 2H20 +1,77 Co*+e = Co* +1,81 Fo(g)+2e = 2F + 2,87 Copyright reserved Please turn over

Downloaded from hlayiso.com Physical Sciences/P2 19 NW/September 2015 NSC GRAPH SHEET NAME: QUESTION 6.3 4 Copyright reserved

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