Physical Sciences Grade 11 P2 North West November 2024 QP

PROVINCIAL ASSESSMENT GRADE 11 PHYSICAL SCIENCES P2 NOVEMBER 2024 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 NW/November 2024 Grade 11 INSTRUCTIONS AND INFORMATION: 1. Write your name on the ANSWER BOOK provided. 2. This question paper consists of NINE questions. Answer ALL 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 sub-questions, for example between QUESTION 2.1 and QUESTION 2.2. 6. You may use a non-programmable calculator. 7. You are advised to use the attached DATA SHEETS. 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, et cetera where required. 11. Write neatly and legibly. Copyright reserved Please turn over

Physical Sciences/P2 3 NW/November 2024 Grade 11 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 B. 1.1 The type of bond which occurs when two atoms share one or more electron pairs will always be ... A ionic. B polar. C metallic. (2) D covalent. 1.2 The molecular shape of NH3 is ... A linear. B trigonal planar. C angular. D trigonal pyramidal. (2) 1.3 Which ONE of the following chlorides will most likely have the most ionic character? A LiCℓ B CsCℓ C BeCℓ2 D CaCℓ2 (2) 1.4 A solution of calcium chloride (CaCℓ2) is added to bromine (Br2) water. The force of attraction that exists between CaCℓ2 particles and Br2 is called a(n) … interaction. A ion-dipole B ion-induced dipole C dipole induced dipole D dipole-dipole (2) Copyright reserved Please turn over

Physical Sciences/P2 4 NW/November 2024 Grade 11 1.5 How many moles of copper (II) oxide are there in 52,8 g of the substance? A 0,369 mole B 0,664 mole C 1,51 mole D 2,71 mole (2) 1.6 The boiling point of CH4 is much lower than that of HF. Which ONE of the following best explains this difference in boiling points? A HF molecules are more polar than CH4 molecules. B CH4 molecules are more polar than HF molecules. C There are London forces between CH4 molecules. D There are dipole-dipole forces between CH4 molecules. (2) 1.7 A fixed amount of gas occupies a volume V exerts a pressure P at a constant temperature. If the volume is doubled, the new pressure of the gas will be ... A 1⁄ P 4 B 1⁄ P 2 C P D 4P (2) 1.8 Consider the incomplete chemical equation below. X + 2HNO3 ⟶ Zn(NO3)2 + H2O + CO2 Which ONE of the following is represented by X in the above equation? A ZnCO3 B ZnHCO3 C ZnCO2 D Zn(OH)2 (2) Copyright reserved Please turn over

Physical Sciences/P2 5 NW/November 2024 Grade 11 1.9 Which ONE of the following statements is TRUE for an EXOTHERMIC reaction? A More energy is released than absorbed. B More energy is absorbed than released. C Heat of reaction (ΔH) is positive. D Energy of the products is greater than the energy of the reactants. (2) 1.10 Consider the reaction represented by the balanced ionic equation below. Cr2O72-(aq) + 14H+(aq) + 3S2-(aq) → 2Cr3+(aq)+ 3S(s) + H2O(ℓ) Which ONE of statements below is true when this reaction takes place. A The oxidation number of sulphur does not change. B S2- is reduced by the Cr2O72-(aq). C H+(aq) oxidises the S2-(aq). D S2-(aq) is oxidised by the Cr2O72-(aq). (2) [20] Copyright reserved Please turn over

Physical Sciences/P2 6 NW/November 2024 Grade 11 QUESTION 2 (Start on a new page.) A chemical bond is defined as a mutual attraction between two atoms resulting from the simultaneous attraction between their nuclei and the outer electrons. Answer the following questions in terms of chemical bonding. 2.1 Define the term electronegativity. (2) 2.2 Show by means of electronegativity what type of bond will be formed between the elements in each of the following substances. 2.2.1 LiF (2) 2.2.2 Cℓ2 (2) 2.3 Consider the following molecules and answer the questions that follow: CO2 , C2H2 and CH4 2.3.1 Define the term valence electrons. (2) 2.3.2 How many valence electrons does carbon have. (1) Draw the Lewis structure for the following molecules: 2.3.3 CO2 (2) 2.3.4 CH4 (2) 2.4 Write down the molecular shape of the following molecules. 2.4.1 CO2 (1) 2.4.2 CH4 (1) 2.5 The bond length between the carbon atoms in C2H4 and C2H6 are compared. 2.5.1 Define the term bond length. (2) 2.5.2 Fully explain why the bond length of the bond between the carbon atoms in C2H4 is shorter than that in C2H6. (3) 2.5.3 What is the relationship between the bond length and bond energy. (2) 2.5.4 How will the bond energy of the bond between the carbon atoms in C2H4 compare to that in C2H6? Choose from SMALLER THAN, GREATER THAN or EQUAL TO. (1) 2.6 Explain the difference between a polar molecule and a non-polar molecule, using the compounds CHCl3 and CCl4 as examples. (4) [27] Copyright reserved Please turn over

Physical Sciences/P2 7 NW/November 2024 Grade 11 QUESTION 3 (Start on a new page.) During an investigation, the MELTING POINTS of the hydrogen halides were determined. The results of the investigation are shown in the graph below. 3.1 Define the term melting point. (2) 3.2 The melting points of HBr and HCℓ are compared. 3.2.1 What is the relationship between strength of the intermolecular forces and melting point? (2) 3.2.2 Explain the difference in the melting points of HBr and HCℓ by referring to the MOLECULAR MASS, STRENGTH OF INTERMOLECULAR FORCES and ENERGY. (3) 3.3 Which ONE of the hydrogen halides in the graph above has the lowest vapour pressure. (1) 3.4 Explain in terms of INTERMOLECULAR FORCES why solid iodine (I2) does not dissolve in water. (2) [10] Copyright reserved Please turn over

Physical Sciences/P2 8 NW/November 2024 Grade 11 QUESTION 4 (Start on a new page.) The relationship between pressure and the volume of an enclosed gas at 30 oC is investigated, by varying the pressure on the gas and then observing the corresponding volume occupied by the gas in each case. The results obtained are shown in the table below. p (kPa) V (cm3) 128,5 35 180 25 220 V 330 20 4.1 STATE the gas law being investigated. (2) 4.2 For this investigation write down the: 4.2.1 Independent variable. (1) 4.2.2 TWO controlled variables. (2) 4.3 Calculate the value represented by the letter V in the table. (3) 4.4 Hydrogen and helium are very close to ideal gases. 4.4.1 Write down TWO properties of an ideal gas. (2) 4.4.2 Write down the TWO conditions under which real gases behave more like an ideal gas. (2) 4.5 Explain, in terms of the kinetic molecular theory, the effect that an increase in the temperature of a gas will have on its pressure at constant volume. (2) [14] Copyright reserved Please turn over

Physical Sciences/P2 9 NW/November 2024 Grade 11 QUESTION 5 (Start on a new page.) One of the steps in the preparation of sulphuric acid in the industry is represented by the following reaction: 2SO2(g) + O2(g) → 2SO3(g) The graph below shows the energy change during this reaction. 5.1 Write down the type of reaction represented by above graph. Choose from EXOTHERMIC or ENDOTHERMIC. Explain your answer. (2) 5.2 Calculate the change in enthalpy for this reaction. (2) Vanadium pentoxide is added as a catalyst in the above reaction. 5.3 How will the addition of the catalyst affect the following? Write down only INCREASES, DECREASES or REMAIN THE SAME. 5.3.1 Activation energy. (1) 5.3.2 Heat of reaction. (1) 5.4 At 68 kJ∙mol-1 an activated complex is formed. 5.4.1 Define the term activated complex. (2) 5.4.2 Write down the activation energy for the reverse reaction. (2) 5.5 Calculate the volume of SO3 gas formed in the container when 50 cm3 of SO2 reacts completely with oxygen. (2) [12] Copyright reserved Please turn over

Physical Sciences/P2 10 NW/November 2024 Grade 11 QUESTION 6 (Start on a new page.) Nicotine, an alkaloid in the nightshade family of plants that is mainly responsible for the addictive nature of cigarettes, contains 74,02 % C, 8,71 % H and 17,27 % N. 6.1 Define the term empirical formula. (2) 6.2 Determine the empirical formula of nicotine. (5) It was found experimentally that 40,57 g of nicotine contains 0,25 mol nicotine. 6.3 Determine the molecular formula of nicotine? (5) [12] QUESTION 7 (Start on a new page.) A 12 g sample of IMPURE solid calcium carbonate, CaCO3, reacted with 150 cm3 of a 2 mol·dm-3 excess hydrochloric acid, HCℓ, according to the following balanced equation: CaCO3(s) + 2HCℓ(aq) → CaCℓ2(aq) + H2O(ℓ) + CO2(g) The graph below shows how the mass of CO2 changes with time at STP. 7.1 Define the term limiting reagent. (2) 7.2 Write down the NAME or FORMULA of the limiting reagent in the above reaction. (1) 7.3 Calculate the: 7.3.1 Maximum volume of CO2 produced. (4) 7.3.2 Percentage purity of calcium carbonate. (6) 7.3.3 Moles of HCℓ in excess. (5) [18] Copyright reserved Please turn over

Physical Sciences/P2 11 NW/November 2024 Grade 11 QUESTION 8 (Start on a new page.) 8.1 Define a Brønsted-Lowry base. (2) 8.2 Calculate the pH of a 0,1 mol·dm-3 of HCℓ (3) 8.3 Write down the FORMULA for the conjugate base of HCℓ. (1) - 8.4 Why is HSO4 regarded as an ampholyte? (2) - 8.5 Write down a balanced chemical equation for the reaction of HSO4 with water to form the hydronium ion. (3) 8.6 A solution of potassium hydroxide(KOH) is prepared by dissolving 7,9 g of potassium hydroxide in 250 cm3 of distilled water. 8.6.1 Calculate the concentration of potassium hydroxide solution. (3) During titration 25 cm3 of the above solution is neutralised by 40 cm3 of a DILUTE sulphuric acid solution according to the balanced equation: H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O 8.6.2 Calculate the concentration of the DILUTE acid. (4) The DILUTE acid in QUESTION 8.6.2 was prepared by adding 10 cm3 of CONCENTRATED acid to 490 cm3 distilled water. 8.6.3 Calculate the concentration of the CONCENTRATED acid. (4) [22] Copyright reserved Please turn over

Physical Sciences/P2 12 NW/November 2024 Grade 11 QUESTION 9 (Start on a new page.) A mixture containing Aluminium and Manganese oxide was heated to initiate the following redox reaction: 2Aℓ + 3MnO → Aℓ2O3 + 3Mn 9.1 Define the term reduction in terms of oxidation numbers. (2) 9.2 Write down the oxidation numbers of the following substances: 9.2.1 Mn in MnO (1) 9.2.2 Aℓ in Aℓ2O3 (1) 9.3 Identify an oxidising agent in the above-mentioned reaction. Explain your answer by referring to oxidation numbers. (3) 9.4 Consider the following reaction: - H+ + Cu +NO3 → H2O + Cu2+ + NO Write down the: 9.4.1 Oxidation half reaction. (2) 9.4.2 Reduction half reaction. (2) 9.4.3 Balanced net ionic equation. (4) [15] TOTAL: 150 Copyright reserved Please turn over

Physical Sciences/P2 1 NW/November 2024 Grade 11 DATA FOR PHYSICAL SCIENCES GRADE 11 PAPER 2 (CHEMISTRY) TABLE 1: PHYSICAL CONSTANTS NAME SYMBOL VALUE Standard pressure p 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 Avogadro’s constant NA 6,02 × 1023 mol-1 TABLE 2: FORMULAE m n pH= -log[H3O+] n= or c= or M V Kw = [H3O+][OH-] = 1x10-14 N m at 298K n= or c= NA MV V ca Va na n= = Vm cb Vb nb Copyright reserved Please turn over

Physical Sciences/P2 32 NW/November 2024 Grade 11 TABLE 4A: STANDARD REDUCTION POTENTIALS Half-reactions/Halfreaksies Eθ (V) F2(g) + 2e ⇌ 2F + 2,87 Co3+ + e ⇌ Co2+ + 1,81  ⇌ + 2H2O +1,77 H2O2 + 2H +2e  ⇌ 2+ MnO 4 + 8H+ + 5e Mn + 4H2O + 1,51   Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36 2 Cr2O 7 + 14H+ + 6e ⇌ 2Cr3+ + 7H2O + 1,33 O2(g) + 4H+ + 4e ⇌ 2H2O + 1,23 MnO2 + 4H+ + 2e ⇌ Mn2+ + 2H2O + 1,23 Pt2+ + 2e ⇌ Pt + 1,20   Br2(ℓ) + 2e ⇌ 2Br + 1,07  NO 3 + 4H+ + 3e ⇌ NO(g) + 2H2O + 0,96  Hg(ℓ) ⇌ 2+ + 0,85 Hg + 2e Increasing oxidising ability/Toenemende oksiderende vermoë Ag+ + e ⇌ Ag + 0,80 Increasing reducing ability/Toenemende reduserende vermoë  NO 3 + 2H+ + e ⇌ NO2(g) + H2O + 0,80  ⇌ 3+ 2+ Fe +e Fe + 0,77 O2(g) + 2H+ + 2e ⇌ H2O2 + 0,68   I2 + 2e ⇌ 2I + 0,54  ⇌ + Cu + 0,52 Cu + e SO2 + 4H+ + 4e ⇌ S + 2H2O + 0,45 2H2O + O2 + 4e ⇌ 4OH + 0,40  ⇌ 2+ Cu + 2e Cu + 0,34 2 SO 4 + 4H+ + 2e ⇌ SO2(g) + 2H2O + 0,17 Cu2+ + e ⇌ Cu + + 0,16 Sn4+ + 2e ⇌ Sn2+ + 0,15  ⇌ + H2S(g) + 0,14 S + 2H + 2e 2H+ + 2e ⇌ H2(g) 0,00 Fe3+ + 3e ⇌ Fe  0,06 Pb2+ + 2e ⇌ Pb  0,13 Sn 2+ + 2e  ⇌ Sn  0,14 Ni2+ + 2e ⇌ Ni  0,27 Co2+ + 2e ⇌ Co  0,28 Cd 2+ + 2e  ⇌ Cd  0,40 Cr3+ + e ⇌ Cr2+  0,41 Fe2+ + 2e ⇌ Fe  0,44 Cr3+ + 3e ⇌ Cr  0,74 Zn 2+ + 2e  ⇌ Zn  0,76 2H2O + 2e ⇌ H2(g) + 2OH  0,83 Cr2+ + 2e ⇌ Cr  0,91 Mn2+ + 2e ⇌ Mn  1,18 Aℓ 3+ + 3e  ⇌ Aℓ  1,66 Mg2+ + 2e ⇌ Mg  2,36 Na+ + e ⇌ Na  2,71 Ca2+ + 2e ⇌ Ca  2,87 2+ Sr + 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 32 NW/November 2024 Grade 11 TABLE 4B: STANDARD REDUCTION POTENTIALS Half-reactions/Halfreaksies 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 2H2O + 2e ⇌ H2(g) + 2OH  0,83 Zn2+ + 2e ⇌ Zn  0,76 Increasing oxidising ability/Toenemende oksiderende vermoë Increasing reducing ability/Toenemende reduserende vermoë 3+ Cr + 3e  ⇌ Cr  0,74 Fe2+ + 2e ⇌ Fe  0,44 Cr3+ + e ⇌ Cr2+  0,41 Cd2+ + 2e ⇌ Cd  0,40 Co2+ + 2e ⇌ Co  0,28 Ni2+ + 2e ⇌ Ni  0,27 2+ Sn + 2e  ⇌ Sn  0,14 Pb2+ + 2e ⇌ Pb  0,13 Fe3+ + 3e ⇌ Fe  0,06 2H+ + 2e ⇌ H2(g) 0,00  ⇌ + S + 2H + 2e H2S(g) + 0,14  ⇌ 4+ 2+ Sn + 2e Sn + 0,15 Cu2+ + e ⇌ Cu+ + 0,16 2 SO 4 + 4H+ + 2e ⇌ SO2(g) + 2H2O + 0,17 Cu2+ + 2e ⇌ Cu + 0,34   2H2O + O2 + 4e ⇌ 4OH + 0,40 SO2 + 4H+ + 4e ⇌ S + 2H2O + 0,45 Cu+ + e ⇌ Cu + 0,52 I2 + 2e ⇌ 2I + 0,54  ⇌ + O2(g) + 2H + 2e H2O2 + 0,68  ⇌ 3+ 2+ Fe + e Fe + 0,77  NO 3 + 2H+ + e ⇌ NO2(g) + H2O + 0,80  ⇌ + Ag + e Ag + 0,80 Hg2+ + 2e ⇌ Hg(ℓ) + 0,85  NO 3 + 4H+ + 3e ⇌ NO(g) + 2H2O + 0,96 Br2(ℓ) + 2e ⇌ 2Br + 1,07  ⇌ 2+ Pt + 2 e Pt + 1,20 MnO2 + 4H+ + 2e ⇌ Mn2+ + 2H2O + 1,23 O2(g) + 4H+ + 4e ⇌ 2H2O + 1,23 2 Cr2O 7 + 14H+ + 6e ⇌ 2Cr3+ + 7H2O + 1,33 Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36  ⇌ 2+ MnO 4 + 8H+ + 5e Mn + 4H2O + 1,51 H2O2 + 2H+ +2 e ⇌ 2H2O +1,77  ⇌ Co2+ 3+ Co + e + 1,81   F2(g) + 2e ⇌ 2F + 2,87 Copyright reserved Please turn over

Physical Sciences/P2 4 NW/November 2024 Grade 11 THE PERIODIC TABLE OF ELEMENTS 1 2 3 5 6 8 9 10 11 12 13 14 15 16 17 18 4 7 (I) (II) (III) (IV) (V) (VI) (VII) (VIII) KEY 1 2 Atomic number H He 2,1 1 4 29 3 4 5 6 7 8 9 10 Li Be Electronegativity 1,9 Symbol B C N O F Ne 1,0 1,5 Cu 2,0 2,5 3,0 3,5 4,0 7 9 11 12 14 16 19 20 11 12 13 14 15 16 17 18 Na Mg Aℓ Si P S Cℓ Ar 0,9 1,2 Approximate relative atomic mass 1,5 1,8 2,1 2,5 3,0 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 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 0,8 1,0 1,3 1,5 1,6 1,6 1,5 1,8 1,8 1,8 1,9 1,6 1,6 1,8 2,0 2,4 2,8 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 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 0,8 1,0 1,2 1,4 1,8 1,9 2,2 2,2 2,2 1,9 1,7 1,7 1,8 1,9 2,1 2,5 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 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tℓ Pb Bi Po At Rn 0,7 133 0,9 137 139 1,6 179 181 184 186 190 192 195 197 201 1,8204 1,8 207 1,9 209 2,0 2,5 87 88 89 Fr Ra Ac 0,7 0,9 226 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

Physical Sciences/P2 4 NW/November 2024 Grade 11 Copyright reserved