Physical Sciences Grade 12 P2 NSC June 2013 QP (Eng)

Downloaded from hlayiso.com basic education Department: Basic Education REPUBLIC OF SOUTH AFRICA SENIOR CERTIFICATE EXAMINATION PHYSICAL SCIENCE P2 CHEMISTRY HIGHER GRADE 2013 MARKS: 200 TIME: 2 hours PHYSICAL SCIENCE HG: Paper 2 3041E 30412E This question paper consists of 16 pages, 4 data sheets and 1 answer sheet. X@5 MI Capyriptt reserved JUN} ANA VO ATE A Ee:

Downloaded from hlayiso.com Physical Science/HG/P2 2 DBE/2013 SCE INSTRUCTIONS AND INFORMATION 1. Write your centre number and examination number in the appropriate spaces on the ANSWER BOOK. 2. Answer ALL the questions. 3. You may use a non-programmable calculator. 4. You may use appropriate mathematical instruments. by, Data sheets and a periodic table are attached for your use. 6. You may forfeit marks if you do not follow instructions. QUESTION 1 INSTRUCTIONS AND INFORMATION 1. Answer this question on the attached ANSWER SHEET. Write your centre number and examination number in the appropriate spaces. 2. Various options are given as possible answers to the following questions. Each question has only ONE answer. Choose the correct or best answer and make a cross (X) in the block (A-D) next to the question number (1.1-1.15) on the ANSWER SHEET. 3. Do not make any other marks on the ANSWER SHEET. Any calculations or writing that may be necessary when answering this question should be done in the ANSWER BOOK and must be deleted clearly by means of a line drawn across the page. 4. If more than ONE block is marked per question, no marks will be awarded for that answer. PLACE THE COMPLETED ANSWER SHEET INSIDE THE FRONT COVER OF YOUR ANSWER BOOK. EXAMPLE: QUESTION: The symbol for the SI unit of time is ... 0nOuU> t. h. s. m. B ANSWER: A Copyright reserved HAIMA ALO A Pease tn over GAUTENG

Downloaded from hlayiso.com Physical Science/HG/P2 3 DBE/2013 SCE 1.1 The temperature of a gas is ... A the heat of the gas. B_ the product of the pressure and volume of the gas. C ameasure of the number of moles of the gas. D ameasure of the average kinetic energy of the molecules of the gas. (4) 1.2 0,5 moles of an ideal gas are sealed in a 200 cm? flask at a pressure of 100 kPa. The flask is placed in hot water and the temperature of the gas gradually increases. Which graph represents the correct pV versus T relationship for the gas? A 4 B 4 pv pv ly T T Cc A D » pv pv ___ ly T T (4) 1.3 The relatively high boiling point of methanol, compared to the boiling point of methane, is due to the presence of ... in methanol. A_ ionic bonding B_ covalent bonding C_ hydrogen bonding D Van der Waals forces (4) Cor eaned LAAN NNN! es

Downloaded from hlayiso.com Physical Science/HG/P2 4 DBE/2013 SCE 1.4 Which ONE of the following is TRUE for the reaction of dichromate ions 1.5 1.6 1.7 (Cr,O?,) with sulphur dioxide (SO2) and hydrogen sulphide (H2S) respectively? A_ Sulphur (S) is formed in both cases. B Chromium ions (Cr**) are formed in both cases. CHS and SO? are the oxidising agent in both cases. D H2S is the reducing agent and SO; the oxidising agent. (4) In which ONE of the following reactions will chlorine gas NOT be a product? A NH,C((s) is heated B_ NaC0() is electrolysed C MnOz(s) + concentrated HC? D KMn0O,(s) + concentrated HC2 (4) The solution in test tube X has a PH less than 4. When it is added to a dilute aqueous solution of barium chloride, a precipitate forms. 0 v4 The solution in test tube X is probably ... NaOH(aq). H2SO,(aq). HC{(aq). NH3;(aq). <+;— BaCé,(aq) 00 WD D> ¢ 2 ¢>— Precipitate (4) When a dilute solution of ethanoic acid (CH3;COOH) is prepared in water, approximately 1% of the acid molecules ionise. When an amount of concentrated hydrochloric acid (HC?) is added to the solution, it is found that only 0,02% of the ethanoic acid molecules ionise. The difference in the degree of ionisation can best be attributed to ... the presence of a common ion. CH3COOH and HC? forming a conjugate acid-base pair. the precipitation reaction that takes place. 00QO 0 > acetic acid being a weak acid. (4) Conyhtesened LI A 0 Pose tum over

Downloaded from hlayiso.com Physical Science/HG/P2 5 DBE/2013 SCE 1.8 In the reaction X + HO + H30* + HSO; X represents ... A the acidSO? . B_ the acid H2SO,. C the baseSO7. D_ the base H2SOx. (4) 1.9 Which ONE of the following 0,1 mol.dm® solutions has the lowest pH? A HC? B NaOH C He2SO, D CH;COOH (4) 1.10 Consider the following chemical equilibrium in a closed container: CaCO3(s) = CaO(s) + CO2(g) AH > 0 The concentration of the COz at equilibrium can be increased by ... A_ adding more CaO(s). B_ adding more CaCO,(s). C_ increasing the pressure. D_ increasing the temperature. (4) 1.11 Consider the following reaction equation: N2(g) + 3H2(g) = 2NH3(g) AH = -92 kJ According to Le Chatelier's principle, the conditions of temperature and pressure at which the highest yield will be obtained, are ... TEMPERATURE PRESSURE A | low low B | high high C | high low D} low high (4) Cont mead A Posse tim oe

Downloaded from hlayiso.com Physical Science/HG/P2 6 DBE/2013 SCE 1.12 Which ONE of the following represents an unbalanced equation for a reaction that can take place spontaneously? A Fe* + Pb > Fe* + Pb* B Fe + Pb* + Fe* + Pb C Fe + Fe + Fe + Fe* D Fe* + Fe > Fe™* + Fe* (4) ae An electrochemical cell is constructed by using Cr| Cr°* and Hg|Hg* half- cells. A bulb connected to the cell glows dimly. The brightness of the bulb can be increased if the Cr| Cr** half-cell is replaced bya... (Refer to Table 4A or Table 4B.) A Hp/H* half-cell. B At| At half-cell. C Ag|Ag* half-cell. D Co|Co** half-cell. (4) 1.14 If the molecular formula of an ester is C2H,O2, the IUPAC name of the ester is ... A. ethyl ethanoate. B_ methyl ethanoate. C_ ethyl methanoate. D_ methyl methanoate. (4) ve A structural isomer of butane (C4H19) is ... A 2-methyl propane. B_ 2-methyl propene. C 2-methyl butene. D 2-methyl butane. (4) [60] Copa reser E01 0 Pee tum over

Downloaded from hlayiso.com Physical Science/HG/P2 U DBE/2013 SCE ANSWER QUESTIONS 2-9 IN THE ANSWER BOOK. INSTRUCTIONS AND INFORMATION 1. 2. 3. 4. Start EACH question on a NEW page in the ANSWER BOOK. Leave ONE line between two subquestions, for example between QUESTION 2.1 and QUESTION 2.2. Show the formulae and substitutions in ALL calculations. Number the answers exactly the same as the questions. QUESTION 2 (START ON A NEW PAGE.) 2.1 2.2 The gas syringe in the sketch below is filled with chlorine gas (Cfz), occupying a volume of 100 cm? at a temperature of 125 °C and a pressure of 120 kPa. 120 kPa | = 125°C | 100. cm? The plunger is now pressed in and the pressure in the gas syringe changes to 360 kPa while the temperature changes to 205 °C. Assuming that the gas behaves like an ideal gas, calculate the volume occupied by the gas under these conditions. The relationship between the volume (V) and the reciprocal (inverse) of the pressure (%) for the Cf(g) is investigated. The result is shown in the graph below. I Pp 2.2.1 Formulate (state in words) the gas law represented by the relationship in this graph. 2.2.2 For the above investigation, 5,0 g of chlorine gas (C22) is sealed ina container at a constant temperature of 15 °C. Calculate the gradient of the graph under the conditions stated. (5) (3) (5) Con eaned LALLA ese

Downloaded from hlayiso.com Physical Science/HG/P2 8 DBE/2013 SCE The experiment is now repeated for the same mass of gas in the same container, but at a temperature of 55 °C. 2.2.3 Redraw the graph on the previous page (for temperature equal to 15 °C) in the ANSWER BOOK. Using a dotted line, draw the graph which will represent the relationship at this higher temperature (55 °C) on the same set of axes. (2) 2.3 When the experiment in QUESTION 2.1 is repeated with the same number of moles of hydrogen fluoride (HF) instead of chlorine gas (C£2), the volume of the gas obtained differs. Refer to intermolecular forces to explain this deviation in volume. (4) [19] QUESTION 3 (START ON A NEW PAGE.) 3.1 Hydrogen sulphide gas (H2S) is prepared in the laboratory by the reaction of dilute hydrochloric acid and a sulphide compound. The H2S gas is then bubbled through a solution of iron(IIl)chloride (FeC?s) in a test tube. FeCé3(aq) _— 3.1.1 Write down the FORMULA of a sulphide compound that can be used in the preparation of H2S gas. (1) 3.1.2 State TWO observations that will be made in the test tube. (2) 3.1.3 Identify only the products responsible for the observations stated in QUESTION 3.1.2. (4) 3.1.4 Is this reaction an oxidation-reduction reaction? (Write only YES or NO.) (1) 3.1.5 Give a reason for your answer to QUESTION 3.1.4. (2) cored UA ALIN) = em cr

Downloaded from hlayiso.com Physical Science/HG/P2 9 DBE/2013 SCE 3.2 A learner prepares sulphur dioxide gas (SO2) using concentrated sulphuric acid (H2SO,) according to the following unbalanced equation: Cu(s) + H2SO4(2) — SO2(g) + CuSO,(aq) + H20(2) 7 Refer to the relative strengths of oxidising and reducing agents to explain why dilute sulphuric acid cannot be used. (3) 3.2.2 Write down the balanced equation for the: (a) Oxidation half-reaction (2) (b) | Reduction half-reaction (2) 3.3 A gas jar containing sulphur dioxide (SO) gas is placed on top of a gas jar containing hydrogen sulphide (H2S) gas. The separation between the two gas jars is removed, allowing the gases to mix. A reaction readily takes place if a small amount of water is present. SO2(g)- [> separation H2S(g}4> water en 3.3.1 What is the function of the water in this reaction? (1) 3.3.2 Why is the gas jar containing SO2 placed on top of the gas jar containing H2S, and not the other way round? (2) 3.3.3 Besides the formation of water, what else can be observed during this reaction? (2) 3.3.4 The reaction that takes place is a redox reaction. Write down the NAME of the oxidising agent. (2) 3.3.5 Which ONE of the two reactants has a 'rotten egg’ smell? (1) [25] Conn eon i feats

Downloaded from hlayiso.com Physical Science/HG/P2 10 DBE/2013 SCE QUESTION 4 (START ON A NEW PAGE.) 4.1 A learner pours a solution of sodium iodide (Nal) into test tube A and adds a solution of silver nitrate (AgNOs) to it. AgNO; (aq) 4.1.1 Describe what is observed in test tube A. (2) 4.1.2 Write down a balanced equation to explain the observation made in QUESTION 4.1.1. (3) The learner now pours a solution of sodium iodide (NaI) into test tube B and adds chlorine water and trichloromethane (chloroform) to it. The test tube is thoroughly shaken and the contents separate into two layers. Chlorine water Chloroform Water__» | B Chloroform___» Two products are formed in test tube B, each dissolving in one of the two layers. 4.1.3 Write down the NAME or FORMULA of the product that dissolved in the: (a) Trichloromethane (chloroform) layer (1) (b) Water layer (1) 4.1.4 What is the final colour of the chloroform layer? (1) Copa resend EH 0 Pease moe

Downloaded from hlayiso.com DBE/2013 Physical Science/HG/P2 ad SCE 4.2 The industrial preparation of nitric acid (HNO3) can be represented by the following diagram: Ammonia (NH3) ————_——> Catalyst chamber Oxygen Process 1 x [om | Oxygen Process2) ——————=}_- Process 3. => _ HNO3 7 Name the substance that can be used as catalyst in Process 1. 4.2.2 Name the substance (X) that is added to perform Process 3. (1) (1) 4.2.3 Water is one of the products formed during Process 1. Write down the FORMULA or NAME of the other product. 4.2.4 Write down the FORMULA of the product formed in Process 2. QUESTION 5 (START ON A NEW PAGE.) 5.1 The sketch below represents the potential energy diagram for the reaction Ha(g) + Ia(g) = 2HI(g). Potential energy (2) (2) [14] Reaction coordinate 5.1.1 What is the value of the heat of reaction (AH) for the reaction? 5.1.2 | What is the value of the activation energy for the reaction? (2) (1) 5.1.3 What is the value of the activation energy for the reaction 2HI(g) — H2(g) + I2(g)? (1) 5.1.4 What change was made to obtain the curve represented by the broken line? 5.1.5 Is the reaction in QUESTION 5.1 exothermic or endothermic? (1) (1) Cont cred AE NAN.

Downloaded from hlayiso.com Physical Science/HG/P2 12 DBE/2013 SCE 5.2 A 2 g sample of zinc, the surface of which has been cleaned, is added to 30 cm* hydrochloric acid solution with a concentration of 2 mol.dm®. Curve A below represents the volume of hydrogen gas formed versus time. ry V(H2) Give a possible reason for: 5.2.1 The increase in the reaction rate before t, (1) 5.2.2 The decrease in the reaction rate after t, (1) A second experiment is performed using a different sample of zinc and a different sample of hydrochloric acid. The same mass of zinc and the same volume of hydrochloric acid are used. The result of this experiment is given by curve B. 5.2.3 State TWO factors that could possibly have contributed to the higher reaction rate represented by curve B. (2) [10] cor ened UU

Downloaded from hlayiso.com Physical Science/HG/P2 13 DBE/2013 SCE QUESTION 6 (START ON A NEW PAGE.) 12,2 g of ammonium carbonate ((NH4)2COs) is sealed in a 0,50 dm? measuring flask. Pressure A pressure gauge is attached to the flask. rT The flask is then placed in an oven and heated to a temperature of 800 °C. After some time equilibrium is reached in the flask according to the following equation: (NHa)2CO3(s) = 2NH3(g) + H2O (g) + CO2(g) AH>0O 6.1 6.2 6.3 6.4 6.5 gauge Oven ———> How can it be observed that equilibrium had been reached? (1) Sketch a graph of mass (vertical axis) versus time (horizontal axis) to show how the mass of (NH4)2CO3 changes with time until equilibrium is established. (2) When equilibrium was established at 800 °C, the mass of (NH4)2COs3 present in the flask was equal to 0,52 g. Calculate the equilibrium constant (Kc) at 800 °C for this reaction. (8) During a power failure the temperature of the oven drops to 500 °C. What effect does the decrease in temperature have on: (Write only INCREASES, DECREASES or STAYS THE SAME.) 6.4.1. The rate of the forward reaction (1) 6.4.2 The mass of (NH,4)2CO3 (1) 6.4.3. The value of Kc (1) Give a reason for your answer to QUESTION 6.4.3 by using Le Chatelier's principle. (3) [17] Cont esored LCA ANN! es

Downloaded from hlayiso.com Physical Science/HG/P2 14 DBE/2013 SCE QUESTION 7 (START ON A NEW PAGE.) 7.1 A learner prepares a potassium hydroxide (KOH) solution to titrate against a sulphuric acid (H2SOx,) solution at 25 °C. The balanced equation for the reaction between potassium hydroxide and sulphuric acid is: 2KOH(aq) + H2SO.(aq) > KzSO.(aq) + 2H2O(2) (5) (6) (1) (1) (3) (1) (2) [24] _ Calculate the mass of potassium hydroxide (KOH) needed to prepare 400 cm? of a 0,15 mol.dm™® KOH solution. 7.1.2 25 cm® of the solution prepared in QUESTION 7.1.1 is used to neutralise 30 cm® of the sulphuric acid solution. Calculate the concentration of the H2SO, solution. 7.1.3 When only one drop of the sulphuric acid solution still had to be added to reach the equivalence point (end point) of the titration, the concentration of the OH’ in the mixture was 1,23 x 10% mol.dm*®. Calculate the pH of the solution at this specific point. 7.2 An aqueous solution of ammonia is investigated. 7.2.1 State whether the pH of this solution will be GREATER THAN 7, EQUAL TO 7 or LESS THAN 7. 7.2.2 Give a reason for your answer to QUESTION 7.2.1. 7.2.3 Write down a balanced equation to explain your answer to QUESTION 7.2.2. 7.2.4 If a few crystals of ammonium chloride are added to the ammonia solution, will the pH of the solution INCREASE, DECREASE or REMAIN THE SAME? 7.2.5 Give a reason for your answer to QUESTION 7.2.4. igh d PI Cony oar NO A eos tm over

Downloaded from hlayiso.com Physical Science/HG/P2 15 DBE/2013 SCE QUESTION 8 (START ON A NEW PAGE.) An electrochemical (galvanic) cell, set up under standard conditions, is represented as follows: Cr(s) | Cr°*(aq) | | Ag*(aq) | Ag(s) A voltmeter is connected across the terminals of the cell. 8.1 Which electrode is the cathode of this cell? (1) 8.2 Write down the balanced equation for the: 8.2.1 Oxidation half-reaction (2) 8.2.2 Reduction half-reaction (2) 8.2.3 Overall cell reaction (2) 8.3 How will the concentration of the chromium ions [Cr**(aq)] change while the cell is in operation? Write only INCREASE, DECREASE or REMAINS THE SAME. (1) 8.4 Write down the FORMULA of an electrolyte that can be used in the Ag’ | Ag half-cell. (1) 8.5 Calculate the emf of this cell. (4) 8.6 When the concentration of the silver ions [Ag*(aq)] is changed to 2 mol.dm®, it is found that the emf increases. Give an explanation for this. (2) [15] Cont esoved NAN Pease tum over

Downloaded from hlayiso.com Physical Science/HG/P2 16 DBE/2013 SCE QUESTION 9 (START ON A NEW PAGE.) 9.1 9.2 9.3 Two possible reactions of organic compounds with bromine are shown below. a eT C—=C——C—H + Bre > y ! H H H B it ft ot + Brg > | i | 9.1.1 Which ONE of the reactions (A or B) will take place more readily? 9.1.2 What is the kind of reaction in QUESTION 9.1.1 called? 9.1.3 What is the IUPAC name of the organic reactant in B? Many organic compounds have structural isomers. 9.2.1 How do two structural isomers differ from each other? 9.2.2 Write down the structural formula of ONE structural isomer of the compound but-1-ene. 9.2.3 Write down the general formula for the homologous series of which but-1-ene is a member. The ester methyl ethanoate can be prepared by the reaction of an alcohol and a carboxylic acid in the presence of a catalyst. Give the NAME of the: 9.3.1 Alcohol used to prepare methyl ethanoate 9.3.2 Carboxylic acid used to prepare methyl ethanoate 9.3.3 Catalyst used in the preparation of methyl ethanoate TOTAL: Conyresened A A (2) (2) (2) (1) (2) (2) (2) [16] 200

Downloaded from hlayiso.com u DBE/2013 Physical Science/HG/P2 SCE DATA FOR PHYSICAL SCIENCE PAPER 2 (CHEMISTRY) GEGEWENS VIR NATUUR- EN SKEIKUNDE VRAESTEL 2 (CHEMIE) TABLE 1: PHYSICAL CONSTANTS TABEL 1: FISIESE KONSTANTES Avogadro's constant Avogadro-konstante Na orlof L 6,02 x 107° mot" Molar gas constant Molére gaskonstante R 8,31 J.K" molt Standard pressure Standaarddruk p® 1,013 x 10° Pa Molar gas volume at STP Molére gasvolume by STD Vn 22,4 dm®.mol" Standard temperature Standaardtemperatuur Tia 273 K TABLE 2: FORMULAE TABEL 2: FORMULES PV) _ PV2 CVn Na T; T, CV_ Mp pV =nRT K, =(H*][OH7]=1074 at/by 298 K na H = -log[H* M pH = —log[H"] n E%cen ad E* oxidising agent ~ EF educing agent |. V E* cel = EC’ oxsideermiddel = EF’ eduseermiddel =” 0 e* MV E% elt = E cathode - E* anode Eset 2 EF’ katode i E* anode Copyright reserved CUT AMATO UTA UA A Please turn over

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Downloaded from hlayiso.com Physical Science/HG/P2 3 DBE/2013 SCE TABLE 4A: STANDARD REDUCTION POTENTIALS/ TABEL 4A: STANDAARD- REDUKSIEPOTENSIALE Half-reactions/Halfreaksies E°/Volt Fo +2@ =. 2F +2,87 H202 + 2H* + 2e = 2H,O +1,77 MnO, + 8H* + 5e = Mn** + 4H,0 +1,51 Au** + 3e = Au +1,42 Ch +2e = 2C8 +1,36 CreO7* + 14H*+ Ge = 2Cr* + 7HO (+133 O2 + 4H* | 4c, 20 +123 MnO + 4H* + 2e = Mn** + 2H,0 +1,21 pt?* +2e = Pt +1,20 Bro + 2e€ = 2Br +1,09 NO; + 4H* + 3e = NO + 2H,0 +0,96 29) Ag* ss +0,80 19 eB} f | NOs + 2H* +e = NO, +H,0 +0,80 2 7 Hg** + 2e = Hg +0,79 3 2 Fe* eo) ae +0,77 7 2 Oz + 2H* + 2e = HO. +0,68 3 5 lo way Ap +0,54 o SO, + 4H" + 4e = S + 2H,0 +0,45 § 3 2H,O +O, + 4e = 40H’ +0,40 3 s Cu** + 2e = Cu +0,34 g ® SO,7 + 4H* + 2e = SO2 + 2H,O +0,17 2 2 Cu?" Se | Gi +0,16 5 = Sn* er. Ge +0,15 iS g S + 2H’ + 2e = HS +0,14 g 3 2H* +2e = He (0,00 g & Fe* + 3e = Fe -0,04 = 3 Pb2* + 2e€ = Pb 0,13 r=) 7 Sn?* ¢.2e.-. on -0,14 2 | Ni?* +2e = Ni -0,25 o £ Co** + 2e€ = Co -0,28 £ 2 Ca?* +2e = Cd -0,40 s 7 Fe* + 2e = Fe -0,44 3 9 cr* + 3e = Cr -0,74 oI 2 Zn** +2e = Zn -0,76 5 9 2H20 + 2e = H+ 20H -0,83 a o Mn?* + 2e = Mn -1,18 ¥ 5 2 At +3e - Al -1,66 £ Mg”* + 2e = Mg -2,37 Na* +e = Na -2,71 Ca?* + 2e = Ca -2,87 sr* +2e = Sr -2,89 Ba** +2e = Ba -2,90 Cs* +e = Cs -2,92 K* +e = K -2,93 Lit poo -3,05 Cony reserved NAN Please tu over

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Downloaded from hlayiso.com Physical Science/HG/P2 Increasing oxidising ability/Toenemende oksiderende vermoé TABLE 4B: STANDARD REDUCTION POTENTIALS/ TABEL 4B: STANDAARD- REDUKSIEPOTENSIALE 4 SCE Half-reactions/Halfreaksies E°/Volt Li* ay = -3,05 Kt fe «k -2,93 Cs* +e = Cs -2,92 Ba?* +2e = Ba 2,90 sr* +2e = Sr 2,89 Ca?* +2e = Ca 2,87 Na +e = Na 2,71 Mg?* +2e = Mg 2,37 Ag +3e - AL -1,66 Mn?* + 2e = Mn -1,18 2H20 + 2e = Hp) + 20H -0,83 Zn2* +2e€ = Zn -0,76 Cr** + ce, -. Gr -0,74 Fe** + 20, | fe -0,44 Cd?* +2e = Cd -0,40 Co** + 2e = Co -0,28 Ni?* +2e = Ni -0,25 Sn?* +2e = Sn -0,14 Pb2* + 2e = Pb -0,13 Fe* +3e = Fe -0,04 2H* + 2e = He (0,00 S + 2H’ + 2e = HS +0,14 Sn* + 2e = Sn* +0,15 Cu* +e = Cur +0,16 SO,7 + 4H* + 2e = SO, + 2H,0 +0,17 Cu* +2e = Cu +0,34 2H20 + Op +4e 2 40H +0,40 SO2 + 4H* +4e = S + 2H,0 +0,45 lo +2e = ar +0,54 O2 + 2H* + 2e = HO. +0,68 Fe* +e = Fe +0,77 Hg?* +2e = Hg +0,79 NO3 + 2H* +e = NO + H,0 +0,80 Ag* +e = Ag +0,80 NOs + 4H* + 3e = NO + 2H,0 +0,96 Bro + 2e€ = 2Br +1,09 Pt? 2 2e0 | Pt +1,20 MnO, + 4H* + 2e = Mn + 2H,0 +1,21 Oz + 4H* + 4e = 2H,O +1,23 CrO7* + 14H* + Ge = 2Cr* + 7H,O (41,33 Clo +2e = 2Cr +1,36 Au* +3e = Au +1,42 MnO, + 8H* + 5e = ~=Mn** + 4H,O +1,51 H202 + 2H* + 2e = 2H20 +1,77 Fo + 2e = 2F +2,87 Copyright reserved GAUTENG DBE/2013 Increasing reducing ability/Toenemende reduserende vermoé

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Downloaded from hlayiso.com Physical Science/HG/P2 DBE/2013 SCE ANSWER SHEET CENTRE NUMBER: EXAMINATION NUMBER: 1.1 A B Cc D 1.2 A B Cc D 1.3 A B Cc D 1.4 A B Cc D 1.5 A B Cc D 1.6 A B Cc D 17 A B Cc D 1.8 A B Cc D For the use of the marker 1.9 A B Cc D Vir die gebruik van die nasiener Marks obtained 1.10 A B Cc D Punte behaal 1.11 A B Cc D Marker's initials 4.12 A B e D Nasiener , se paraaf 1.13 A B Cc D Marker's number Nasiener 1.14 A B Cc D se nommer 1.15 A B Cc D (15 x 4) [60] coowintesonea NN LLL