# Physical Sciences Grade 11 P2 2015 QP (Eng) > Grade 11 Physical Sciences Paper 2 question paper from the National Exemplar November Exam 2015 (English), 18 pages. Read online or download the free PDF. - Page: https://www.hlayiso.com/library/physical-sciences-p2-grade-11-nov-2015-eng/07d5e6a0-0856-4a03-a529-fc367bcebb29 - Updated: 2026-09-27 - Subject: Physical Sciences - Grade: Grade 11 - Document type: Question paper - Year: 2015 - Exam period: National Exemplar November Exam - Paper: 2 - Curriculum: CAPS - Pages: 18 Breadcrumbs: [Home](https://www.hlayiso.com/) › [Library](https://www.hlayiso.com/library) › [Grade 11](https://www.hlayiso.com/library/grade-11) › [Physical Sciences](https://www.hlayiso.com/library/grade-11/physical-sciences) › [Physical Sciences Grade 11 P2 2015 QP (Eng)](https://www.hlayiso.com/library/physical-sciences-p2-grade-11-nov-2015-eng/07d5e6a0-0856-4a03-a529-fc367bcebb29) ## About this document Physical Sciences · Grade 11 · National Exemplar November Exam · 2015. Question paper, 18 pages. Read online or download the PDF. Read it free online on the page above; download the PDF from there. ## Document text Text extracted from the PDF. Layout, diagrams and tables may not survive extraction. ### Page 1 Downloaded from hlayiso.com NATIONAL SENIOR CERTIFICATE GRADE 11 PHYSICAL SCIENCES: CHEMISTRY (P2) NOVEMBER 2015 MARKS: 150 TIME: 3 hours This question paper consists of 13 pages, 4 data sheets and 1 answer sheet. Copyright reserved Please turn over ### Page 2 Downloaded from hlayiso.com Physical Sciences/P2 2 DBE/November 2015 CAPS – Grade 11 INSTRUCTIONS AND INFORMATION 1. Write your name and class (for example 11A) in the appropriate spaces on the ANSWER BOOK. 2. This question paper consists of TEN questions. Answer QUESTION 4.2 and QUESTION 4.3 on the attached ANSWER SHEET. Answer ALL the other questions in the ANSWER BOOK. 3. Start EACH question on a NEW page in the ANSWER BOOK. 4. Number the answers correctly according to the numbering system used in this question paper. 5. Leave ONE line between two subquestions, for example between QUESTION 2.1 and QUESTION 2.2. 6. You may use a non-programmable calculator. 7. You may use appropriate mathematical instruments. 8. You are advised to use the attached DATA SHEETS. 9. Show ALL formulae and substitutions in ALL calculations. 10. Round off your final numerical answers to a minimum of TWO decimal places. 11. Give brief motivations, discussions et cetera where required. 12. Write neatly and legibly. Copyright reserved Please turn over ### Page 3 Downloaded from hlayiso.com Physical Sciences/P2 3 DBE/November 2015 NSC – Grade 11 QUESTION 1: MULTIPLE-CHOICE QUESTIONS Four options are provided as possible answers to the following questions. Each question has only ONE correct answer. Choose the answer and write only the letter (A–D) next to the question number (1.1–1.10) in the ANSWER BOOK, for example 1.11 E. 1.1 According to the Arrhenius theory, all bases … A are proton donors. B are proton acceptors. C form H 3 O+ ions in solution. D form OH‾ ions in solution. (2) 1.2 The number of neutrons in an atom of 157 N is ... A 5 B 7 C 8 D 15 (2) 1.3 Which ONE of the following has the strongest forces between its molecules? A F2 B Cℓ 2 C Br 2 D I2 (2) 1.4 Which ONE of the following has a tetrahedral shape? A H3 O + B NH +4 C CO 2 D AℓCℓ 3 (2) Copyright reserved Please turn over ### Page 4 Downloaded from hlayiso.com Physical Sciences/P2 4 DBE/November 2015 NSC – Grade 11 1.5 Two moles of H 2 gas at STP occupy a volume of ... A 2 dm3 B 11,2 dm3 C 22,4 dm3 D 44,8 dm3 (2) 1.6 Which ONE of the following statements CORRECTLY describes the characteristics of an endothermic reaction? A ΔH is positive and the products have less potential energy than the reactants. B ΔH is positive and the products have more potential energy than the reactants. C ΔH is negative and the products have less potential energy than the reactants. D ΔH is negative and the products have more potential energy than the reactants. (2) 1.7 Which ONE of the following balanced equations represents a redox reaction? A H+(aq) + OH-(aq) → H 2 O(ℓ) B Mg(s) + CuSO 4 (aq) → Cu(s) + MgSO 4 (aq) C 2NaCℓ(aq) + Pb(NO 3 ) 2 (aq) → 2NaNO 3 (aq) + PbCℓ 2 (s) D H 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) → BaSO 4 (s) + 2HNO 3 (aq) (2) 1.8 During the extraction of gold, zinc powder is added to a solution of gold cyanide to produce gold according to the following balanced equation: Zn(s) + 2NaAu(CN) 2 (aq) → 2Au(s) + Zn(CN) 2 (aq) + 2NaCN(aq) The oxidising agent in this reaction is ... A Au+ B Zn C Na+ D CN − (2) Copyright reserved Please turn over ### Page 5 Downloaded from hlayiso.com Physical Sciences/P2 5 DBE/November 2015 NSC – Grade 11 1.9 The volume of a gas at a certain temperature and pressure is V. If the temperature is doubled and the pressure is halved, the volume of the gas will be … A 4V B 2V C V D ½V (2) 1.10 Two identical containers, M and N, are shown below. Container M contains H 2 (g) and container N contains CO 2 (g). Both gases are at a temperature of 25 °C and a pressure of 101,3 kPa. M N H2(g) CO2(g) 25 °C 25 °C 101,3 kPa 101,3 kPa Consider the following statements: (i) The average kinetic energy of the molecules is the same in both containers. (ii) Container M contains more gas molecules than container N. (iii) The mass of the gas in container N is greater than the mass of the gas in container M. Which of the above statements is/are CORRECT? A (i) only B (iii) only C (i) and (ii) only D (i) and (iii) only (2) [20] Copyright reserved Please turn over ### Page 6 Downloaded from hlayiso.com Physical Sciences/P2 6 DBE/November 2015 NSC – Grade 11 QUESTION 2 (Start on a new page.) Molecules such as CO 2 and H 2 O are formed through covalent bonding. 2.1 Define the term covalent bonding. (2) 2.2 ONE of the above molecules has lone pairs of electrons on the central atom. Draw the Lewis diagram for this molecule. (2) 2.3 H 3 O+ is formed when H 2 O forms a dative covalent bond with an H+ ion. 2.3.1 Draw the Lewis diagram for H 3 O+. (1) 2.3.2 State TWO conditions for the formation of such a bond. (2) 2.4 The polarity of molecules depends on the DIFFERENCE IN ELECTRONEGATIVITY and the MOLECULAR SHAPE. 2.4.1 Define the term electronegativity. (2) 2.4.2 Calculate the difference in electronegativity between: (a) C and O in CO 2 (1) (b) H and O in H 2 O (1) 2.4.3 Explain the difference in polarity between CO 2 and H 2 O by referring to the polarity of the bonds and the shape of the molecules. (6) [17] Copyright reserved Please turn over ### Page 7 Downloaded from hlayiso.com Physical Sciences/P2 7 DBE/November 2015 NSC – Grade 11 QUESTION 3 (Start on a new page.) 3.1 The boiling point of compounds A to E are given in the table below. COMPOUND FORMULA BOILING POINT (°C) A CH 4 –164 B C2H6 –89 C C 5 H 12 36 D C 6 H 14 69 E C 20 H 42 343 3.1.1 Define the term boiling point. (2) 3.1.2 Calculate the molecular mass of compound D. (1) 3.1.3 In what phase is compound B at 25 °C? (1) 3.1.4 Name the type of intermolecular force present in compound A. (1) 3.1.5 Explain why the boiling point increases from compound A to E. (3) 3.1.6 How does the vapour pressure of compound B compare to the vapour pressure of compound C? Write down only HIGHER THAN, LOWER THAN or EQUAL TO. (1) 3.2 Consider the boiling points of the compounds in the table below. SUBSTANCE BOILING POINT (°C) H2S –60 NH 3 –33 H2O 100 3.2.1 Which ONE of the substances in the table above has the weakest forces between its molecules? (1) 3.2.2 Name the type of intermolecular force found between NH 3 molecules. (1) 3.2.3 Explain the following statement: Although the shape of the molecules of H 2 S and H 2 O is similar, there is a remarkable difference in their boiling points. (4) [15] Copyright reserved Please turn over ### Page 8 Downloaded from hlayiso.com Physical Sciences/P2 8 DBE/November 2015 NSC – Grade 11 QUESTION 4 (Start on a new page.) A learner investigates the relationship between the pressure and volume of an enclosed DIATOMIC gas at 25 °C. He records the volume of the gas for different pressures in the table below. PRESSURE VOLUME 1 (kPa) (cm3) (cm-3) V 40 43 0,02 80 27 0,04 100 22 (a) 120 18 (b) 4.1 Write down the name of the gas law being investigated. (1) Answer QUESTION 4.2 and QUESTION 4.3 on the attached ANSWER SHEET. 1 Two values in the table, (a) and (b), have not been calculated. 4.2 V Calculate these values. (1) 1 4.3 Draw a graph of pressure versus on the attached ANSWER SHEET. (4) V 4.4 Use the graph to determine the volume of the gas at 68 kPa. (2) 4.5 The mass of the enclosed DIATOMIC gas is 2,49 x 10-2 g. 4.5.1 Use the conditions at a pressure of 100 kPa and calculate the molar mass of the enclosed gas. (6) 4.5.2 Write down the molecular formula of the enclosed gas. (1) 4.6 The sketch graph below shows the relationship between volume and temperature for an ideal gas. Volume (cm3) Temperature (K) 4.6.1 Redraw the above graph in the ANSWER BOOK. On the same set of axes, use a BROKEN LINE to sketch the graph that will be obtained for the diatomic gas above. (1) 4.6.2 Fully explain why this diatomic gas deviates from ideal behaviour. (3) [19] Copyright reserved Please turn over ### Page 9 Downloaded from hlayiso.com Physical Sciences/P2 9 DBE/November 2015 NSC – Grade 11 QUESTION 5 (Start on a new page.) The fizz produced when an antacid dissolves in water is caused by the reaction between sodium hydrogen carbonate (NaHCO 3 ) and citric acid (H 3 C 6 H 5 O 7 ). The balanced equation for the reaction is: 3NaHCO 3 (aq) + H 3 C 6 H 5 O 7 (aq) → Na 3 C 6 H 5 O 7 (aq) + 3CO 2 (g) + 3H 2 O(ℓ) 5.1 Write down the FORMULA of the substance that causes the fizz when the antacid dissolves in water. (1) A certain antacid contains 1,8 g of H 3 C 6 H 5 O 7 and 3,36 g of NaHCO 3 . The antacid is dissolved in 100 cm3 distilled water in a beaker. 5.2 Define 1 mole of a substance. (2) 5.3 Calculate the number of moles of NaHCO 3 in the antacid. (3) 5.4 Determine, using calculations, which substance is the limiting reagent. (4) 5.5 Calculate the mass of the reactant in excess. (3) 5.6 Calculate the mass decrease of the beaker contents on completion of the reaction. (3) [16] QUESTION 6 (Start on a new page.) 6.1 Sodium thiosulphate, Na 2 S 2 O 3 (s), reacts with 200 cm3 of a hydrochloric acid solution, HCℓ(aq), of concentration 0,2 mol·dm-3 according to the following balanced equation: Na 2 S 2 O 3 (s) + 2HCℓ(aq) → 2NaCℓ(aq) + S(s) + SO 2 (g) + H 2 O(ℓ) 6.1.1 Define the term concentration of a solution. (2) 6.1.2 Calculate the number of moles of HCℓ(aq) added to the sodium thiosulphate. (3) 6.1.3 Calculate the volume of SO 2 (g) that will be formed if the reaction takes place at STP. (3) Copyright reserved Please turn over ### Page 10 Downloaded from hlayiso.com Physical Sciences/P2 10 DBE/November 2015 NSC – Grade 11 6.2 Menthol, the substance we can smell in mentholated cough drops, is composed of carbon (C), hydrogen (H) and oxygen (O). During combustion of a 9,984 g sample of menthol, it is found that 28,160 g of CO 2 (g) and 11,520 g of H 2 O(g) is produced. 6.2.1 Calculate the mass of carbon (C) in the CO 2 . (4) 6.2.2 Use relevant calculations to determine the empirical formula of menthol. (7) 6.2.3 The molar mass of menthol is 156 g·mol-1. Determine the molecular formula of menthol. (2) [21] QUESTION 7 (Start on a new page.) A barium hydroxide solution, Ba(OH) 2 (aq), reacts with a nitric acid solution, HNO 3 (aq), according to the following balanced equation: Ba(OH) 2 (aq) + 2HNO 3 (aq) → Ba(NO 3 ) 2 (aq) + 2H 2 O(ℓ) The potential energy graph below shows the change in potential energy for this reaction. Potential energy A (kJ⋅mol-1) B 116 kJ⋅mol-1 C Course of reaction 7.1 Is this reaction ENDOTHERMIC or EXOTHERMIC? Give a reason for the answer. (2) 7.2 Use energy values A, B and C indicated on the graph and write down an expression for each of the following: 7.2.1 The energy of the activated complex (1) 7.2.2 The activation energy for the forward reaction (1) 7.2.3 ∆H for the reverse reaction (1) 7.3 Calculate the amount of energy released during the reaction if 0,18 moles of Ba(OH) 2 (aq) reacts completely with the acid. (3) [8] Copyright reserved Please turn over ### Page 11 Downloaded from hlayiso.com Physical Sciences/P2 11 DBE/November 2015 NSC – Grade 11 QUESTION 8 (Start on a new page.) When sulphuric acid reacts with water, it ionises in two steps, as shown in the two balanced equations below. I: H 2 SO 4 (aq) + H 2 O(ℓ) → H 3 O+(aq) + HSO −4 (aq) + II: HSO −4 (aq) + H 2 O(ℓ) → H 3 O (aq) + SO 24 − (aq) 8.1 Define an acid in terms of the Lowry-Brønsted theory. (2) 8.2 Write down the FORMULA of: 8.2.1 The conjugate base of HSO −4 (aq) (1) 8.2.2 The conjugate acid of HSO −4 (aq) (1) 8.2.3 A substance that acts as ampholyte in these reactions (1) 8.3 A few drops of bromothymol blue indicator are added to a potassium hydroxide solution in a beaker. A dilute sulphuric acid solution is now gradually added to this solution until the colour of the indicator changes. Write down the: 8.3.1 Type of reaction that takes place (Write down only REDOX, PRECIPITATION or NEUTRALISATION.) (1) 8.3.2 Balanced equation for the reaction that takes place (3) 8.3.3 Colour change of the indicator (2) 8.3.4 NAME of the salt formed in this reaction (1) [12] Copyright reserved Please turn over ### Page 12 Downloaded from hlayiso.com Physical Sciences/P2 12 DBE/November 2015 NSC – Grade 11 QUESTION 9 (Start on a new page.) 9.1 Oxidation numbers make it easier to determine whether an element or a substance is oxidised or reduced during a chemical reaction. 9.1.1 Define the term oxidation with reference to oxidation numbers. (2) 9.1.2 Calculate the oxidation number of chromium in Cr2O72 − . (1) 9.1.3 Calculate the oxidation number of oxygen in H 2 O 2 . (1) 9.2 Consider the UNBALANCED equation below: - Fe2+(aq) + Cℓ 2 (g) → Fe3+(aq) + Cℓ 9.2.1 Define the term reducing agent with reference to electron transfer. (2) From the above equation, write down the: 9.2.2 FORMULA of the reducing agent (1) 9.2.3 FORMULA of the oxidising agent (1) 9.2.4 Reduction half-reaction (2) 9.2.5 Oxidation half-reaction (2) 9.2.6 Balanced net redox reaction (2) [14] Copyright reserved Please turn over ### Page 13 Downloaded from hlayiso.com Physical Sciences/P2 13 DBE/November 2015 CAPS – Grade 11 QUESTION 10 (Start on a new page.) The simplified diagram below shows a blast furnace used for the extraction of iron from iron ore. P represents a reactant added to the blast furnace. Q and R represent products that leave the blast furnace. Raw materials Iron ore Limestone Coke Waste Waste gases gases out out P R Q Limestone and coke are added to the blast furnace, as shown in the diagram above. Write down the function of: 10.1.1 Limestone (1) 10.1.2 Coke (1) 10.2 Write down the NAME of the substance represented by: 10.2.1 P (1) 10.2.2 Q (1) 10.2.3 R (1) 10.3 Write down the NAME or FORMULA of ONE waste gas formed during the extraction of iron from iron ore. (1) 10.4 The balanced equation for the extraction of iron from iron ore is: Fe 2 O 3 (s) + 3CO(g) 2Fe(s) + 3CO 2 (g) Write down the: 10.4.1 Function of carbon monoxide in this reaction (1) 10.4.2 FORMULA of the substance that is reduced (1) [8] TOTAL: 150 Copyright reserved ### Page 14 Downloaded from hlayiso.com Physical Sciences/P2 DBE/November 2015 CAPS – Grade 11 DATA FOR PHYSICAL SCIENCES GRADE 11 PAPER 2 (CHEMISTRY) GEGEWENS VIR FISIESE WETENSKAPPE GRAAD 11 VRAESTEL 2 (CHEMIE) TABLE 1: PHYSICAL CONSTANTS/TABEL 1: FISIESE KONSTANTES NAME/NAAM SYMBOL/SIMBOOL VALUE/WAARDE Avogadro's constant NA 6,02 x 1023 mol-1 Avogadro-konstante Molar gas constant R 8,31 J∙K-1∙mol-1 Molêre gaskonstante Standard pressure pθ 1,013 x 105 Pa Standaarddruk Molar gas volume at STP Vm 22,4 dm3∙mol-1 Molêre gasvolume by STD Standard temperature Tθ 273 K Standaardtemperatuur TABLE 2: FORMULAE/TABEL 2: FORMULES p1V1 p 2 V2 = pV = nRT T1 T2 m N n= n= M NA V n m n= c= OR/OF c= Vm V MV Copyright reserved ### Page 15 Downloaded from hlayiso.com Physical Sciences/P2 DBE/November 2015 CAPS – Grade 11 TABLE 3: THE PERIODIC TABLE OF ELEMENTS/TABEL 3: DIE PERIODIEKE TABEL VAN ELEMENTE 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 (I) (II) (III) (IV) (V) (VI) (VII) (VIII) 1 Atomic number 2 KEY/SLEUTEL Atoomgetal 2,1 H He 1 4 3 4 29 5 6 7 8 9 10 Electronegativity Symbol 1,0 Li 1,5 Be Elektronegatiwiteit 1,9 Cu Simbool 2,0 B 2,5 C 3,0 N 3,5 O 4,0 F Ne 7 9 63,5 11 12 14 16 19 20 11 12 13 14 15 16 17 18 0,9 Na 1,2 Mg Approximate relative atomic mass 1,5 Aℓ 1,8 Si 2,1 P 2,5 S 3,0 Cℓ Ar 23 24 Benaderde relatiewe atoommassa 27 28 31 32 35,5 40 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 0,8 K 1,0 Ca 1,3 Sc 1,5 Ti 1,6 V 1,6 Cr 1,5 Mn 1,8 Fe 1,8 Co 1,8 Ni 1,9 Cu 1,6 Zn 1,6 Ga 1,8 Ge 2,0 As 2,4 Se 2,8 Br Kr 39 40 45 48 51 52 55 56 59 59 63,5 65 70 73 75 79 80 84 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 0,8 Rb 1,0 Sr 1,2 Y 1,4 Zr Nb 1,8 Mo 1,9 Tc 2,2 Ru 2,2 Rh 2,2 Pd 1,9 Ag 1,7 Cd 1,7 In 1,8 Sn 1,9 Sb 2,1 Te 2,5 I Xe 86 88 89 91 92 96 101 103 106 108 112 115 119 122 128 127 131 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 0,7 Cs 0,9 Ba La 1,6 Hf Ta W Re Os Ir Pt Au Hg 1,8 Tℓ 1,8 Pb 1,9 Bi 2,0 Po 2,5 At Rn 133 137 139 179 181 184 186 190 192 195 197 201 204 207 209 87 88 89 0,7 Fr 0,9 Ra Ac 58 59 60 61 62 63 64 65 66 67 68 69 70 71 226 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 140 141 144 150 152 157 159 163 165 167 169 173 175 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 232 238 Copyright reserved ### Page 16 Downloaded from hlayiso.com Physical Sciences/P2 DBE/November 2015 CAPS – Grade 11 TABLE 4A: STANDARD REDUCTION POTENTIALS TABEL 4A: STANDAARD-REDUKSIEPOTENSIALE θ Half-reactions/Halfreaksies E (V) F 2 (g) + 2e− ⇌ 2F− + 2,87 3+ 2+ Co + e− ⇌ Co + 1,81 + H 2 O 2 + 2H +2e− ⇌ 2H 2 O +1,77 − + 2+ MnO 4 + 8H + 5e− ⇌ Mn + 4H 2 O + 1,51 Cℓ 2 (g) + 2e− ⇌ 2Cℓ− + 1,36 2− + 3+ Cr 2 O 7 + 14H + 6e− ⇌ 2Cr + 7H 2 O + 1,33 + − O 2 (g) + 4H + 4e ⇌ 2H 2 O + 1,23 + 2+ MnO 2 + 4H + 2e− ⇌ Mn + 2H 2 O + 1,23 2+ Pt + 2e− ⇌ Pt + 1,20 Br 2 (ℓ) + 2e− ⇌ 2Br− + 1,07 − + NO 3 + 4H + 3e− ⇌ NO(g) + 2H 2 O + 0,96 Increasing reducing ability/Toenemende reduserende vermoë 2+ − Hg + 2e ⇌ Hg(ℓ) + 0,85 + Ag + e− ⇌ Ag + 0,80 Increasing oxidising ability/Toenemende oksiderende vermoë − + NO 3 + 2H + e− ⇌ NO 2 (g) + H 2 O + 0,80 3+ − 2+ Fe + e ⇌ Fe + 0,77 + O 2 (g) + 2H + 2e− ⇌ H2O2 + 0,68 I 2 + 2e− ⇌ 2I− + 0,54 + Cu + e− ⇌ Cu + 0,52 + SO 2 + 4H + 4e− ⇌ S + 2H 2 O + 0,45 2H 2 O + O 2 + 4e− ⇌ 4OH− + 0,40 2+ Cu + 2e− ⇌ Cu + 0,34 2− + SO 4 + 4H + 2e− ⇌ SO 2 (g) + 2H 2 O + 0,17 2+ + Cu + e− ⇌ Cu + 0,16 4+ 2+ Sn + 2e− ⇌ Sn + 0,15 + S + 2H + 2e− ⇌ H 2 S(g) + 0,14 + 2H + 2e− ⇌ H 2 (g) 0,00 3+ Fe + 3e− ⇌ Fe − 0,06 2+ Pb + 2e− ⇌ Pb − 0,13 2+ Sn + 2e− ⇌ Sn − 0,14 2+ Ni + 2e− ⇌ Ni − 0,27 2+ Co + 2e− ⇌ Co − 0,28 2+ Cd + 2e− ⇌ Cd − 0,40 3+ 2+ Cr + e− ⇌ Cr − 0,41 2+ Fe + 2e− ⇌ Fe − 0,44 3+ Cr + 3e− ⇌ Cr − 0,74 2+ Zn + 2e− ⇌ Zn − 0,76 2H 2 O + 2e− ⇌ H 2 (g) + 2OH− − 0,83 2+ Cr + 2e− ⇌ Cr − 0,91 2+ Mn + 2e− ⇌ Mn − 1,18 3+ Aℓ + 3e− ⇌ Aℓ − 1,66 2+ Mg + 2e− ⇌ Mg − 2,36 + Na + e− ⇌ Na − 2,71 2+ Ca + 2e− ⇌ Ca − 2,87 2+ Sr + 2e− ⇌ Sr − 2,89 2+ Ba + 2e− ⇌ Ba − 2,90 + - Cs + e ⇌ Cs - 2,92 + − K +e ⇌ K − 2,93 + Li + e− ⇌ Li − 3,05 Copyright reserved ### Page 17 Downloaded from hlayiso.com Physical Sciences/P2 DBE/November 2015 CAPS – Grade 11 TABLE 4B: STANDARD REDUCTION POTENTIALS TABEL 4B: STANDAARD-REDUKSIEPOTENSIALE θ Half-reactions/Halfreaksies E (V) + Li + e− ⇌ Li − 3,05 + K + e− ⇌ K − 2,93 + Cs + e− ⇌ Cs − 2,92 2+ Ba + 2e− ⇌ Ba − 2,90 2+ Sr + 2e− ⇌ Sr − 2,89 2+ Ca + 2e− ⇌ Ca − 2,87 + Na + e− ⇌ Na − 2,71 2+ Mg + 2e− ⇌ Mg − 2,36 3+ Aℓ + 3e− ⇌ Aℓ − 1,66 2+ Mn + 2e− ⇌ Mn − 1,18 2+ Cr + 2e− ⇌ Cr − 0,91 2H 2 O + 2e− ⇌ H 2 (g) + 2OH− − 0,83 2+ Zn + 2e− ⇌ Zn − 0,76 3+ Cr + 3e− Cr Increasing oxidising ability/Toenemende oksiderende vermoë ⇌ − 0,74 2+ Fe + 2e− ⇌ Fe − 0,44 3+ 2+ Cr + e− ⇌ Cr − 0,41 Increasing reducing ability/Toenemende reduserende vermoë 2+ Cd + 2e− ⇌ Cd − 0,40 2+ Co + 2e− ⇌ Co − 0,28 2+ Ni + 2e− ⇌ Ni − 0,27 2+ Sn + 2e− ⇌ Sn − 0,14 2+ Pb + 2e− ⇌ Pb − 0,13 3+ Fe + 3e− ⇌ Fe − 0,06 + 2H + 2e− ⇌ H 2 (g) 0,00 + S + 2H + 2e− ⇌ H 2 S(g) + 0,14 4+ 2+ Sn + 2e− ⇌ Sn + 0,15 2+ + Cu + e− ⇌ Cu + 0,16 2− + SO 4 + 4H + 2e− ⇌ SO 2 (g) + 2H 2 O + 0,17 2+ − Cu + 2e ⇌ Cu + 0,34 2H 2 O + O 2 + 4e− ⇌ 4OH− + 0,40 + SO 2 + 4H + 4e− ⇌ S + 2H 2 O + 0,45 + Cu + e− ⇌ Cu + 0,52 I 2 + 2e− ⇌ 2I− + 0,54 + O 2 (g) + 2H + 2e− ⇌ H2O2 + 0,68 3+ 2+ Fe + e− ⇌ Fe + 0,77 − + NO 3 + 2H + e− ⇌ NO 2 (g) + H 2 O + 0,80 + − Ag + e ⇌ Ag + 0,80 2+ Hg + 2e− ⇌ Hg(ℓ) + 0,85 − + NO 3 + 4H + 3e− ⇌ NO(g) + 2H 2 O + 0,96 − − Br 2 (ℓ) + 2e ⇌ 2Br + 1,07 2+ Pt + 2 e− ⇌ Pt + 1,20 + 2+ MnO 2 + 4H + 2e− ⇌ Mn + 2H 2 O + 1,23 + O 2 (g) + 4H + 4e− ⇌ 2H 2 O + 1,23 2− + 3+ Cr 2 O 7 + 14H + 6e− ⇌ 2Cr + 7H 2 O + 1,33 − − Cℓ 2 (g) + 2e ⇌ 2Cℓ + 1,36 − + 2+ MnO 4 + 8H + 5e− ⇌ Mn + 4H 2 O + 1,51 + H 2 O 2 + 2H +2 e− ⇌ 2H 2 O +1,77 3+ 2+ Co + e− ⇌ Co + 1,81 F 2 (g) + 2e− ⇌ 2F − + 2,87 Copyright reserved Text truncated here. 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