Physical Sciences Grade 11 P2 November Mock 2026 QP (Eng)

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 The shape of an ammonia (NH3 ) molecule is … A linear. B trigonal planar. C trigonal pyramidal. D tetrahedral. (2) 1.2 Which ONE of the following molecules is NON-POLAR, although it contains POLAR bonds? A H2 O B CO2 C HCℓ D NH3 (2) 1.3 The STRONGEST intermolecular force between hydrogen chloride (HCℓ) molecules is … A covalent bonding. B hydrogen bonding. C ion-dipole forces. D dipole-dipole forces. (2) 1.4 Which ONE of the following substances has the HIGHEST boiling point? A H2 O B H2 S C CH4 D Ne (2) Copyright reserved Please turn over

Physical Sciences/P2 4 Hlayiso/Mock 2026 NSC Mock 1.5 A fixed mass of an ideal gas is kept at CONSTANT PRESSURE. The Kelvin temperature of the gas is doubled. The volume of the gas will … A halve. B double. C increase four times. D remain the same. (2) 1.6 The number of moles of OXYGEN ATOMS in 0,5 mol of copper(II) sulphate pentahydrate, CuSO4 ·5H2 O, is … A 2,0 B 2,5 C 4,5 D 9,0 (2) 1.7 Under which ONE of the following combinations of conditions does a real gas deviate MOST from ideal gas behaviour? TEMPERATURE PRESSURE A High Low B Low High (2) C High High D Low Low 1.8 Which ONE of the following processes is ENDOTHERMIC? A Photosynthesis B Combustion of methane C Neutralisation of an acid by a base D Condensation of steam (2) 1.9 Which ONE of the following species can act as an AMPHOLYTE? A NH+4 B Cℓ– C HCO–3 D H3 O+ (2) Copyright reserved Please turn over

Physical Sciences/P2 5 Hlayiso/Mock 2026 NSC Mock 1.10 The oxidation number of manganese (Mn) in potassium permanganate, KMnO4 , is … A +2 B +4 C +6 D +7 (2) [20] Copyright reserved Please turn over

Physical Sciences/P2 6 Hlayiso/Mock 2026 NSC Mock QUESTION 2 (Start on a new page.) 2.1 Define the term covalent bond. (2) 2.2 Draw Lewis diagrams for the following molecules: 2.2.1 H2 O (2) 2.2.2 NH3 (2) 2.3 An NH3 molecule reacts with a hydrogen ion (H+ ) to form an ammonium ion (NH+4 ). 2.3.1 Name the type of bond that forms between NH3 and H+ . (1) 2.3.2 Write down the shape of the NH+4 ion. (1) 2.4 Water is a polar molecule. 2.4.1 Define the term electronegativity. (2) 2.4.2 Use electronegativity values to calculate the electronegativity difference for the O–H bond and hence classify this bond. (2) 2.4.3 Explain why the water molecule is POLAR. Refer to the bonds and the shape of the molecule. (3) 2.5 The graph below shows how the potential energy of two hydrogen atoms changes as they approach each other to form an H2 molecule. Potential energy (kJ·mol–1 ) 74 –436 Distance between nuclei (pm) 2.5.1 Define the term bond length. (2) 2.5.2 Use the graph to write down the bond length and the bond energy of the H–H bond. (2) 2.5.3 The bond length of the Cℓ–Cℓ bond is greater than that of the H–H bond. How will the bond energy of the Cℓ–Cℓ bond compare with that of the H–H bond? Choose from GREATER THAN, SMALLER THAN or EQUAL TO. Explain the answer. (3) [22] Copyright reserved Please turn over

Physical Sciences/P2 7 Hlayiso/Mock 2026 NSC Mock QUESTION 3 (Start on a new page.) Learners investigate the relationship between the type of intermolecular forces and the boiling points of four substances with SIMILAR molar masses. The results are shown in the table below. SUBSTANCE FORMULA MOLAR MASS (g·mol–1 ) BOILING POINT (◦ C) A CH4 16 –162 B NH3 17 –33 C H2 O 18 100 D HF 20 20 3.1 Define the term intermolecular forces. (2) 3.2 Define the term boiling point. (2) 3.3 For this investigation, write down the: 3.3.1 Independent variable (1) 3.3.2 Dependent variable (1) 3.4 Name the STRONGEST type of intermolecular force between the molecules of: 3.4.1 Substance A (1) 3.4.2 Substance B (1) 3.5 Explain the difference in the boiling points of substances A and C by referring to the TYPE and STRENGTH of the intermolecular forces and the ENERGY involved. (4) 3.6 Which substance, A, B, C or D, has the HIGHEST vapour pressure at 25 ◦ C? Give a reason for the answer. (2) 3.7 Write down the PHASE of substance D at 25 ◦ C. (1) [15] QUESTION 4 (Start on a new page.) Learners use the apparatus below to investigate the relationship between the pressure and the volume of a fixed mass of air enclosed in a syringe. The temperature of the air is kept constant at 25 ◦ C throughout. pressure gauge volume scale trapped air push Copyright reserved Please turn over

Physical Sciences/P2 8 Hlayiso/Mock 2026 NSC Mock The results are shown in the table below. Pressure (kPa) 80 100 120 150 200 Volume (cm3 ) 30 24 20 X 12 4.1 State Boyle’s law in words. (2) 4.2 Write down TWO variables that are kept constant in this investigation. (2) 4.3 Calculate the value of X in the table. (3) 4.4 1 . Describe the shape of The learners plot a graph of pressure versus volume the graph that they will obtain. (1) 4.5 Calculate the number of moles of air in the syringe. (4) 4.6 The plunger is now fixed when the volume of the air is 24 cm3 and the air is heated to 75 ◦ C. Calculate the new pressure of the air. (3) 4.7 At very high pressures the air no longer behaves like an ideal gas. Explain this deviation from ideal gas behaviour. (3) [18] Copyright reserved Please turn over

Physical Sciences/P2 9 Hlayiso/Mock 2026 NSC Mock QUESTION 5 (Start on a new page.) 5.1 A compound used in the food industry contains 40,0% carbon, 6,7% hydrogen and 53,3% oxygen by mass. The molar mass of the compound is 180 g·mol–1 . 5.1.1 Define the term empirical formula. (2) 5.1.2 Determine the empirical formula of the compound. (5) 5.1.3 Determine the molecular formula of the compound. (2) 5.2 A 4,99 g sample of hydrated copper(II) sulphate, CuSO4 ·xH2 O, is heated until all the water of crystallisation has been driven off. The mass of the anhydrous CuSO4 that remains is 3,19 g. Calculate the value of x. (4) [13] QUESTION 6 (Start on a new page.) 6.1 Define the term limiting reagent. (2) 6,5 g of zinc granules are added to 150 cm3 of hydrochloric acid of concentration 1,2 mol·dm–3 . The balanced equation for the reaction is: Zn(s) + 2HCℓ(aq) → ZnCℓ2 (aq) + H2 (g) 6.2 Use calculations to determine which reactant is the LIMITING REAGENT. (5) 6.3 Calculate the volume of hydrogen gas produced at STP. (3) 6.4 Calculate the mass of the reactant that is in EXCESS when the reaction stops. (3) 6.5 A 15 g sample of IMPURE limestone (calcium carbonate) reacts completely with excess dilute hydrochloric acid according to the equation below. The impurities do not react with the acid. CaCO3 (s) + 2HCℓ(aq) → CaCℓ2 (aq) + H2 O(ℓ) + CO2 (g) 2,8 dm3 of carbon dioxide gas is collected at STP. Calculate the percentage purity of the limestone. (5) [18] Copyright reserved Please turn over

Physical Sciences/P2 10 Hlayiso/Mock 2026 NSC Mock QUESTION 7 (Start on a new page.) The potential energy diagram below represents the reaction between gases A2 and B2 to form AB: A2 (g) + B2 (g) → 2AB(g) Potential energy (kJ) Q 320 2AB 150 A2 + B2 60 0 Course of reaction 7.1 Is this reaction EXOTHERMIC or ENDOTHERMIC? Give a reason for the answer. (2) 7.2 Define the term activation energy. (2) 7.3 Use the diagram to write down the value of the: 7.3.1 Activation energy for the forward reaction (1) 7.3.2 Heat of reaction (∆H) (1) 7.4 Point Q represents the activated complex. Define the term activated complex. (2) 7.5 The molar mass of AB is 30 g·mol–1 . Calculate the energy absorbed or released when 75 g of AB is formed. State whether the energy is ABSORBED or RELEASED. (3) [11] QUESTION 8 (Start on a new page.) 8.1 Define an acid according to the Lowry-Brønsted theory. (2) 8.2 Ammonia reacts with water according to the following equation: NH3 (g) + H2 O(ℓ) ⇌ NH+4 (aq) + OH– (aq) 8.2.1 Write down the TWO conjugate acid-base pairs in this reaction. (4) 8.2.2 Water acts as an ACID in the reaction above. Write down a balanced equation for a reaction in which water acts as a BASE when it reacts with hydrogen chloride gas. (2) Copyright reserved Please turn over

Physical Sciences/P2 11 Hlayiso/Mock 2026 NSC Mock 8.2.3 Write down ONE word for a substance, like water, that can act as either an acid or a base. (1) 8.3 A learner prepares a standard solution of sodium hydroxide by dissolving 2,0 g of NaOH crystals in water in a 250 cm3 volumetric flask and filling the flask to the mark. 8.3.1 Define the term standard solution. (2) 8.3.2 Calculate the concentration of the sodium hydroxide solution. (3) 25 cm3 of this sodium hydroxide solution exactly neutralises 20 cm3 of a sulphuric acid solution. The balanced equation for the reaction is: H2 SO4 (aq) + 2NaOH(aq) → Na2 SO4 (aq) + 2H2 O(ℓ) 8.3.3 Calculate the concentration of the sulphuric acid solution. (4) [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 oxidation in terms of oxidation numbers. (2) 9.2 Determine the oxidation number of: 9.2.1 S in H2 SO4 (1) 9.2.2 Mn in MnO2 (1) 9.3 When an acidified potassium permanganate solution is added to a solution containing iron(II) ions, Fe2+ (aq), the purple colour of the permanganate ions (MnO–4 ) disappears and iron(III) ions, Fe3+ (aq), form. Use the Table of Standard Reduction Potentials to write down the: 9.3.1 Oxidation half-reaction (2) 9.3.2 Reduction half-reaction (2) 9.3.3 Balanced net ionic equation for the reaction (3) 9.3.4 FORMULA of the oxidising agent (1) 9.4 A strip of zinc is placed in a blue copper(II) sulphate solution. The following reaction takes place: Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) Use OXIDATION NUMBERS to explain why zinc is regarded as the REDUCING AGENT in this reaction. (3) [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