Physical Sciences Grade 11 P2 November Mock Exam 2 2026 QP

Mock hlayiso mock exams Practice Series: Grade 11 Exam Preparation WWW.HLAYISO.COM NATIONAL SENIOR CERTIFICATE GRADE 11 PHYSICAL SCIENCES: CHEMISTRY (P2) NOVEMBER EXAMINATION 2026 (MOCK) MARKS: 150 TIME: 3 hours This question paper consists of 12 pages and 4 data sheets. Copyright reserved Please turn over

Physical Sciences/P2 2 Hlayiso/Mock 2026 NSC Mock INSTRUCTIONS AND INFORMATION 1. Write your name and class (or examination number) in the appropriate spaces on the ANSWER BOOK. 2. This question paper consists of NINE questions. Answer ALL the 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, e.g. between QUESTION 2.1 and QUESTION 2.2. 6. You may use a non-programmable calculator. 7. You may use appropriate mathematical instruments. 8. Show ALL formulae and substitutions in ALL calculations. 9. Round off your FINAL numerical answers to a minimum of TWO decimal places. 10. Give brief motivations, discussions, etc. where required. 11. You are advised to use the attached DATA SHEETS. 12. Write neatly and legibly. Copyright reserved Please turn over

Physical Sciences/P2 3 Hlayiso/Mock 2026 NSC Mock QUESTION 1: MULTIPLE-CHOICE QUESTIONS Various 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 numbers (1.1 to 1.10) in the ANSWER BOOK, e.g. 1.11 E. 1.1 Which ONE of the following molecules has an OCTAHEDRAL shape? A CH4 B SF6 C PCℓ5 D BF3 (2) 1.2 The bond with the GREATEST ionic character is found in … A KF. B HF. C CF4 . D F2 . (2) 1.3 ION-DIPOLE forces are the strongest forces between the particles in … A solid sodium chloride. B pure liquid water. C a solution of sodium chloride in water. D a solution of iodine in tetrachloromethane (CCℓ4 ). (2) 1.4 Which ONE of the following gas samples occupies the LARGEST volume at STP? A 4 g of helium (He) B 4 g of hydrogen (H2 ) C 16 g of oxygen (O2 ) D 22 g of carbon dioxide (CO2 ) (2) 1.5 The number of MOLECULES in 4,4 g of carbon dioxide (CO2 ) is … A 1,81× 1023 B 6,02× 1023 C 2,65× 1024 D 6,02× 1022 (2) Copyright reserved Please turn over

Physical Sciences/P2 4 Hlayiso/Mock 2026 NSC Mock 1.6 A gas is sealed in a rigid steel cylinder and then heated. According to the kinetic molecular theory, the pressure of the gas increases because the gas molecules … A become larger. B increase in number. C move faster and collide with the walls more often and with greater force. D experience stronger intermolecular forces. (2) 1.7 Which ONE of the following CORRECTLY describes the effect of adding a catalyst to a reaction? ACTIVATION ENERGY HEAT OF REACTION (∆H) A Increases Remains the same B Decreases Decreases (2) C Increases Increases D Decreases Remains the same 1.8 The CONJUGATE ACID of the hydrogen sulphate ion (HSO–4 ) is … A H2 SO4 B SO2– 4 C H3 O+ D H2 O (2) 1.9 Which ONE of the following species can act as an AMPHOLYTE? A NH+4 B SO2– 4 C H2 PO–4 D Cℓ– (2) Copyright reserved Please turn over

Physical Sciences/P2 5 Hlayiso/Mock 2026 NSC Mock 1.10 Consider the reaction represented by the balanced equation below: Cℓ2 (g) + 2KBr(aq) → 2KCℓ(aq) + Br2 (aq) Which ONE of the following is the OXIDISING AGENT in this reaction? A Cℓ2 B KBr C KCℓ D Br2 (2) [20] QUESTION 2 (Start on a new page.) Consider the following substances: CO2 BF3 OF2 H2 O CH4 2.1 Define the term polar covalent bond. (2) 2.2 Draw Lewis diagrams for: 2.2.1 CO2 (2) 2.2.2 OF2 (2) 2.3 Use the VSEPR model to write down the molecular shape of: 2.3.1 CO2 (1) 2.3.2 BF3 (1) 2.3.3 OF2 (1) 2.4 The bonds in a BF3 molecule are polar. 2.4.1 Calculate the electronegativity difference for the B–F bond. Use the answer to classify the bond. (2) 2.4.2 Explain why the BF3 molecule is NON-POLAR, although its bonds are polar. (3) 2.5 The O atom in a water molecule can form a dative covalent bond with a hydrogen ion (H+ ), but the C atom in a methane (CH4 ) molecule cannot. Explain this difference. (2) Copyright reserved Please turn over

Physical Sciences/P2 6 Hlayiso/Mock 2026 NSC Mock 2.6 The table below gives the bond lengths and bond energies of three carbon–carbon bonds. BOND BOND LENGTH (pm) BOND ENERGY (kJ·mol–1 ) C–C 154 348 C=C 134 614 C≡C X 839 2.6.1 Define the term bond energy. (2) 2.6.2 Use the data in the table to state the relationship between bond length and bond energy. (1) 2.6.3 Is X GREATER THAN or SMALLER THAN 134 pm? Explain the answer by referring to the number of shared electron pairs. (3) [22] Copyright reserved Please turn over

Physical Sciences/P2 7 Hlayiso/Mock 2026 NSC Mock QUESTION 3 (Start on a new page.) The melting points and boiling points of the hydrides of the Group 15 elements are given in the table below. HYDRIDE MOLAR MASS MELTING POINT BOILING POINT (g·mol–1 ) (◦ C) (◦ C) NH3 (ammonia) 17 –78 –33 PH3 (phosphine) 34 –133 –88 AsH3 (arsine) 78 –116 –62 SbH3 (stibine) 125 –88 –17 3.1 Define the term vapour pressure. (2) 3.2 Consider the hydrides PH3 , AsH3 and SbH3 ONLY. 3.2.1 Describe the trend in their boiling points. (1) 3.2.2 Explain this trend by referring to MOLECULAR SIZE, the STRENGTH of the intermolecular forces and ENERGY. (3) 3.3 NH3 has the SMALLEST molar mass, yet it has a HIGHER boiling point than PH3 and AsH3 . Explain this observation by referring to the TYPE of intermolecular forces. (3) 3.4 Which hydride in the table has the HIGHEST vapour pressure at any given temperature? Give a reason for the answer by referring to the data in the table. (2) 3.5 Write down the PHASE of SbH3 at –50 ◦ C. (1) 3.6 Ammonia gas dissolves very easily in water. Explain this observation by referring to the intermolecular forces between the particles involved. (3) [15] Copyright reserved Please turn over

Physical Sciences/P2 8 Hlayiso/Mock 2026 NSC Mock QUESTION 4 (Start on a new page.) Learners investigate the relationship between the volume and the temperature of the air enclosed in a gas syringe. The syringe is sealed and placed in a water bath. The water is heated slowly and the volume of the air is read off on the syringe scale at different temperatures. The plunger moves freely. The results are shown in the table below. Temperature (◦ C) 0 20 40 60 80 Volume (cm3 ) 40,0 42,9 45,9 48,8 51,7 4.1 Write down an investigative question for this investigation. (2) 4.2 Explain why the plunger must be able to move freely. (2) 4.3 State Charles’ law in words. (2) 4.4 A graph of volume versus temperature in ◦ C is a straight line. When the graph is extrapolated, it cuts the temperature axis at one particular temperature. Write down the VALUE and the NAME of this temperature. (2) 4.5 Calculate the volume of the enclosed air when the water bath reaches 100 ◦ C. (3) In a different experiment, 0,325 g of an unknown DIATOMIC gas fills a 250 cm3 container at a pressure of 101,3 kPa and a temperature of 27 ◦ C. 4.6 Use a calculation to identify the gas. Choose from N2 , O2 , F2 or Cℓ2 . (5) 4.7 Will the gas in QUESTION 4.6 behave MORE like an ideal gas at 300 K or at 100 K (at the same pressure)? Explain the answer. (2) [18] QUESTION 5 (Start on a new page.) Sorbic acid is used as a preservative in foods such as cheese and bread. It contains only carbon, hydrogen and oxygen. When 1,12 g of pure sorbic acid is burnt completely in excess oxygen, 2,64 g of carbon dioxide (CO2 ) and 0,72 g of water (H2 O) are the only products formed. 5.1 Define the term molar mass. (2) 5.2 Use the information above to determine the EMPIRICAL formula of sorbic acid. (6) 5.3 The molar mass of sorbic acid is 112 g·mol–1 . Determine its MOLECULAR formula. (2) 5.4 Calculate the number of oxygen ATOMS in the 1,12 g sample of sorbic acid. (3) [13] Copyright reserved Please turn over

Physical Sciences/P2 9 Hlayiso/Mock 2026 NSC Mock QUESTION 6 (Start on a new page.) Learners add different masses of magnesium ribbon to separate 50,0 cm3 samples of the SAME hydrochloric acid solution. In each case they measure the total volume of hydrogen gas produced, converted to STP. The balanced equation for the reaction is: Mg(s) + 2HCℓ(aq) → MgCℓ2 (aq) + H2 (g) Their results are shown in the graph below. Volume of H2 at STP (cm3 ) 336 224 112 0 0 0,12 0,24 0,36 0,48 0,60 Mass of magnesium added (g) 6.1 Define the term one mole of a substance. (2) 6.2 Write down the minimum mass of magnesium needed to react with ALL the hydrochloric acid in a 50,0 cm3 sample. (1) 6.3 Which reactant is the LIMITING REAGENT when 0,60 g of magnesium is added? Give a reason for the answer by referring to the graph. (2) 6.4 Use the graph to calculate the concentration of the hydrochloric acid. (5) 6.5 Use a calculation to show that the volume of hydrogen gas produced when 0,12 g of magnesium is added is 112 cm3 at STP. (3) 6.6 In a separate experiment, 20 cm3 of propane gas (C3 H8 ) is mixed with 150 cm3 of oxygen gas and ignited. The balanced equation for the reaction is: C3 H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2 O(ℓ) All volumes are measured at the same temperature and pressure, and the water formed condenses to a liquid of negligible volume. Calculate the TOTAL volume of gas present in the container when the reaction is complete. (5) [18] Copyright reserved Please turn over

Physical Sciences/P2 10 Hlayiso/Mock 2026 NSC Mock QUESTION 7 (Start on a new page.) Ammonia is manufactured from nitrogen and hydrogen in the presence of an iron catalyst. The balanced equation for the reaction is: N2 (g) + 3H2 (g) → 2NH3 (g) ∆H = –92 kJ·mol–1 For this question, assume that the activation energy of the UNCATALYSED forward reaction is 230 kJ·mol–1 . 7.1 Define the term heat of reaction. (2) 7.2 Is this reaction EXOTHERMIC or ENDOTHERMIC? Give a reason for the answer. (2) 7.3 Explain, in terms of the energy involved in BOND BREAKING and BOND FORMATION, why this reaction has the type of heat of reaction stated in QUESTION 7.2. (2) 7.4 Calculate the activation energy of the uncatalysed REVERSE reaction. (2) 7.5 Draw a sketch graph of potential energy versus course of reaction for the FORWARD reaction. No values are required. Clearly indicate the following on the graph: • The heat of reaction (∆H) • The activation energy (EA ) of the uncatalysed reaction • The pathway of the CATALYSED reaction, drawn as a dotted (broken) line (3) [11] Copyright reserved Please turn over

Physical Sciences/P2 11 Hlayiso/Mock 2026 NSC Mock QUESTION 8 (Start on a new page.) 8.1 Define a base according to the Arrhenius theory. (2) 8.2 The hydrogen carbonate ion (HCO–3 ) reacts with water according to the equation below: HCO–3 (aq) + H2 O(ℓ) ⇌ H2 CO3 (aq) + OH– (aq) Is HCO–3 acting as an ACID or a BASE in this reaction? Give a reason for the answer. (2) 8.3 A learner wants to determine the percentage of magnesium hydroxide (Mg(OH)2 ) in an antacid tablet. The other substances in the tablet do not react with acids. She places 0,50 g of the crushed tablet in a flask and adds 100 cm3 of hydrochloric acid of concentration 0,10 mol·dm–3 . The acid is in EXCESS. When all the magnesium hydroxide has reacted, the EXCESS hydrochloric acid is exactly neutralised by 24,0 cm3 of a sodium hydroxide solution of concentration 0,10 mol·dm–3 according to the equation: HCℓ(aq) + NaOH(aq) → NaCℓ(aq) + H2 O(ℓ) 8.3.1 Write down a balanced chemical equation for the reaction between magnesium hydroxide and hydrochloric acid. (3) 8.3.2 Calculate the number of moles of hydrochloric acid ADDED to the tablet. (2) 8.3.3 Write down the NAME and the FORMULA of the salt formed in the reaction in QUESTION 8.3.1. (2) 8.3.4 Calculate the percentage by mass of magnesium hydroxide in the tablet. (7) [18] Copyright reserved Please turn over

Physical Sciences/P2 12 Hlayiso/Mock 2026 NSC Mock QUESTION 9 (Start on a new page.) 9.1 Define a reducing agent in terms of electron transfer. (2) 9.2 A piece of burning magnesium ribbon is placed in a gas jar filled with carbon dioxide. It continues to burn, and white magnesium oxide and black specks of carbon form. The balanced equation for the reaction is: 2Mg(s) + CO2 (g) → 2MgO(s) + C(s) Write down the FORMULA of the OXIDISING AGENT in this reaction. Explain the answer by referring to oxidation numbers. (3) 9.3 Hydrogen sulphide gas (H2 S) is bubbled through an acidified solution of potassium dichromate (K2 Cr2 O7 ). The orange solution turns green as Cr3+ ions form, and a yellow precipitate of sulphur (S) appears. 9.3.1 Determine the oxidation number of Cr in Cr2 O2– 7 . (1) 9.3.2 Determine the oxidation number of S in H2 S. (1) Use the Table of Standard Reduction Potentials to write down the: 9.3.3 Oxidation half-reaction (2) 9.3.4 Reduction half-reaction (2) 9.3.5 Balanced net ionic equation for the reaction (3) 9.3.6 FORMULA of the reducing agent (1) [15] TOTAL: 150 Copyright reserved Please turn over

Physical Sciences/P2 1 Hlayiso/Mock 2026 NSC Mock DATA FOR PHYSICAL SCIENCES GRADE 11 PAPER 2 (CHEMISTRY) TABLE 1: PHYSICAL CONSTANTS NAME SYMBOL VALUE Avogadro’s constant NA 6,02× 1023 mol–1 Molar gas constant R 8,31 J·K–1 ·mol–1 Standard pressure pθ 1,013× 105 Pa Molar gas volume at STP Vm 22,4 dm3 ·mol–1 Standard temperature Tθ 273 K Charge on electron e –1,6× 10–19 C TABLE 2: FORMULAE p1 V1 p2 V2 = pV = nRT T1 T2 m N n= n= M NA V n m n= c= or c = Vm V MV ca Va na Q Q = n= or n = cb Vb nb e qe Copyright reserved Please turn over

Physical Sciences/P2 2 Hlayiso/Mock 2026 NSC Mock TABLE 3: THE PERIODIC TABLE OF ELEMENTS 1 2 13 14 15 16 17 18 (I) (II) 3 4 5 6 7 8 9 10 11 12 (III) (IV) (V) (VI) (VII) (VIII) 1 2 Atomic number 2,1 H He 1 KEY 4 29 3 4 5 6 7 8 9 10 1,0 1,5 Electronegativity 1,9 Cu Symbol 2,0 2,5 3,0 3,5 4,0 Li Be B C N O 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 1,5 Aℓ 1,8 Si 2,1 P 2,5 S 3,0 Cℓ Ar Approximate relative atomic mass 23 24 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 226 58 59 60 61 62 63 64 65 66 67 68 69 70 71 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 Please turn over

Physical Sciences/P2 3 Hlayiso/Mock 2026 NSC Mock TABLE 4A: STANDARD REDUCTION POTENTIALS Half-reactions Eθ (V) F2 (g) + 2e– ⇌ 2F– + 2,87 Co3+ + e– ⇌ Co2+ + 1,81 H2 O2 + 2H+ + 2e– ⇌ 2H2 O + 1,77 MnO–4 + 8H+ + 5e– ⇌ Mn2+ + 4H2 O + 1,51 Cℓ2 (g) + 2e– ⇌ 2Cℓ– + 1,36 Cr2 O2– + – 3+ 7 + 14H + 6e ⇌ 2Cr + 7H2 O + 1,33 + – O2 (g) + 4H + 4e ⇌ 2H2 O + 1,23 MnO2 + 4H+ + 2e– ⇌ Mn2+ + 2H2 O + 1,23 Pt2+ + 2e– ⇌ Pt + 1,20 Br2 (ℓ) + 2e– ⇌ 2Br– + 1,07 NO–3 + 4H+ + 3e– ⇌ NO(g) + 2H2 O + 0,96 Hg2+ + 2e– ⇌ Hg(ℓ) + 0,85 Ag+ + e– ⇌ Ag + 0,80 NO3 + 2H+ + e– ⇌ NO2 (g) + H2 O – + 0,80 Fe3+ + e– ⇌ Fe2+ + 0,77 O2 (g) + 2H+ + 2e– ⇌ H2 O2 + 0,68 Increasing strength of oxidising agents I2 + 2e– ⇌ 2I– Increasing strength of reducing agents + 0,54 Cu+ + e– ⇌ Cu + 0,52 SO2 + 4H+ + 4e– ⇌ S + 2H2 O + 0,45 2H2 O + O2 + 4e– ⇌ 4OH– + 0,40 Cu2+ + 2e– ⇌ Cu + 0,34 SO4 + 4H+ + 2e– ⇌ SO2 (g) + 2H2 O 2– + 0,17 Cu2+ + e– ⇌ Cu+ + 0,16 Sn4+ + 2e– ⇌ Sn2+ + 0,15 S + 2H+ + 2e– ⇌ H2 S(g) + 0,14 2H+ + 2e– ⇌ H2 (g) 0,00 Fe3+ + 3e– ⇌ Fe – 0,06 Pb2+ + 2e– ⇌ Pb – 0,13 Sn2+ + 2e– ⇌ Sn – 0,14 Ni2+ + 2e– ⇌ Ni – 0,27 Co2+ + 2e– ⇌ Co – 0,28 Cd2+ + 2e– ⇌ Cd – 0,40 Cr3+ + e– ⇌ Cr2+ – 0,41 Fe2+ + 2e– ⇌ Fe – 0,44 Cr3+ + 3e– ⇌ Cr – 0,74 Zn2+ + 2e– ⇌ Zn – 0,76 2H2 O + 2e– ⇌ H2 (g) + 2OH– – 0,83 Cr2+ + 2e– ⇌ Cr – 0,91 Mn2+ + 2e– ⇌ Mn – 1,18 Aℓ3+ + 3e– ⇌ Aℓ – 1,66 Mg2+ + 2e– ⇌ Mg – 2,36 Na+ + e– ⇌ Na – 2,71 Ca2+ + 2e– ⇌ Ca – 2,87 Sr2+ + 2e– ⇌ Sr – 2,89 Ba2+ + 2e– ⇌ Ba – 2,90 Cs+ + e– ⇌ Cs – 2,92 K+ + e– ⇌ K – 2,93 Li+ + e– ⇌ Li – 3,05 Copyright reserved Please turn over

Physical Sciences/P2 4 Hlayiso/Mock 2026 NSC Mock TABLE 4B: STANDARD REDUCTION POTENTIALS Half-reactions Eθ (V) Li+ + e– ⇌ Li – 3,05 K+ + e– ⇌ K – 2,93 Cs+ + e– ⇌ Cs – 2,92 Ba2+ + 2e– ⇌ Ba – 2,90 Sr2+ + 2e– ⇌ Sr – 2,89 Ca2+ + 2e– ⇌ Ca – 2,87 Na+ + e– ⇌ Na – 2,71 Mg2+ + 2e– ⇌ Mg – 2,36 Aℓ3+ + 3e– ⇌ Aℓ – 1,66 Mn2+ + 2e– ⇌ Mn – 1,18 Cr2+ + 2e– ⇌ Cr – 0,91 2H2 O + 2e– ⇌ H2 (g) + 2OH– – 0,83 Zn2+ + 2e– ⇌ Zn – 0,76 Cr3+ + 3e– ⇌ Cr – 0,74 Fe2+ + 2e– ⇌ Fe – 0,44 Cr3+ + e– ⇌ Cr2+ – 0,41 Increasing strength of oxidising agents Cd2+ + 2e– ⇌ Cd Increasing strength of reducing agents – 0,40 Co2+ + 2e– ⇌ Co – 0,28 Ni2+ + 2e– ⇌ Ni – 0,27 Sn2+ + 2e– ⇌ Sn – 0,14 Pb2+ + 2e– ⇌ Pb – 0,13 Fe3+ + 3e– ⇌ Fe – 0,06 2H+ + 2e– ⇌ H2 (g) 0,00 S + 2H+ + 2e– ⇌ H2 S(g) + 0,14 Sn4+ + 2e– ⇌ Sn2+ + 0,15 Cu2+ + e– ⇌ Cu+ + 0,16 SO4 + 4H+ + 2e– ⇌ SO2 (g) + 2H2 O 2– + 0,17 Cu2+ + 2e– ⇌ Cu + 0,34 2H2 O + O2 + 4e– ⇌ 4OH– + 0,40 SO2 + 4H+ + 4e– ⇌ S + 2H2 O + 0,45 Cu+ + e– ⇌ Cu + 0,52 I2 + 2e– ⇌ 2I– + 0,54 O2 (g) + 2H+ + 2e– ⇌ H2 O2 + 0,68 Fe3+ + e– ⇌ Fe2+ + 0,77 NO–3 + 2H+ + e– ⇌ NO2 (g) + H2 O + 0,80 Ag+ + e– ⇌ Ag + 0,80 Hg2+ + 2e– ⇌ Hg(ℓ) + 0,85 NO–3 + 4H+ + 3e– ⇌ NO(g) + 2H2 O + 0,96 Br2 (ℓ) + 2e– ⇌ 2Br– + 1,07 Pt2+ + 2e– ⇌ Pt + 1,20 MnO2 + 4H+ + 2e– ⇌ Mn2+ + 2H2 O + 1,23 O2 (g) + 4H+ + 4e– ⇌ 2H2 O + 1,23 Cr2 O2– + – 3+ 7 + 14H + 6e ⇌ 2Cr + 7H2 O + 1,33 Cℓ2 (g) + 2e ⇌ 2Cℓ– – + 1,36 MnO–4 + 8H+ + 5e– ⇌ Mn2+ + 4H2 O + 1,51 H2 O2 + 2H+ + 2e– ⇌ 2H2 O + 1,77 Co3+ + e– ⇌ Co2+ + 1,81 F2 (g) + 2e– ⇌ 2F– + 2,87 Copyright reserved