Physical Sciences Grade 11 P2 Eastern Cape November 2022 QP

Downloaded from hlayiso.com NATIONAL SENIOR CERTIFICATE GRADE 11 NOVEMBER 2022 PHYSICAL SCIENCES P2 (CHEMISTRY) MARKS: 100 TIME: 2 hours This question paper consists of 16 pages, including 4 data sheets.

Downloaded from hlayiso.com 2 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) INSTRUCTIONS AND INFORMATION 1. Write your full NAME and SURNAME in the appropriate spaces on the ANSWER BOOK. 2. This question paper consists of SEVEN 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 sub-questions, 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. 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. You are advised to use the attached DATA SHEETS. 12. Write neatly and legibly. Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 3 QUESTION 1: MULTIPLE-CHOICE QUESTIONS Various options are provided as possible answers to the following questions. Choose the answer and write only the letter (A–D) next to the question numbers (1.1 to 1.7) in the ANSWER BOOK, for example 1.8 D. 1.1 Which ONE of the following is the NAME given to the reaction in which electrons are transferred from one substance to another substance? A Redox B Precipitation C Neutralisation D Decomposition (2) 1.2 The diagram below is used to demonstrate the differences between interatomic bonds (chemical bonds) and intermolecular forces. X H H Y H C H H C H H H Which ONE of the following statements is CORRECT? A X is stronger than Y B X is an interatomic bond C X is an intermolecular force D Y is an intermolecular force (2) 1.3 The minimum amount of energy needed for a chemical reaction to start is called … A activation energy. B catalyst. C heat of reaction. D bond energy. (2) Copyright reserved Please turn over

Downloaded from hlayiso.com 4 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) 1.4 Consider the potential energy graph for the hypothetical reaction: 2 P → P2 Potential energy (kJ·mol-1) Z 2P Y P2 X time The heat of the reaction (ΔH) is represented by … A Z – Y. B X – Y. C Y – X. D Y – Z. (2) 1.5 Consider the INCOMPLETE reaction below: X + HCℓ → Salt + H2O Which ONE of the following is CORRECT regarding compound X? Compound X is a(n) … A carbonate. B metal. C metal oxide. D acid. (2) Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 5 1.6 Consider the substances P, Q and R. P dissolves in Q but not in R. The MOST LIKELY bonds or intermolecular forces in substances P, Q and R are: P Q R A Ionic bonds Dipole-dipole forces London forces B London forces Dipole-dipole forces Ionic bonds C Dipole-dipole forces London forces Ionic bonds D Ionic bonds London forces Dipole-dipole forces (2) 1.7 According to the kinetic molecular theory, molecules of gases at the same temperature always have the same … A mass. B volume. C pressure. D average kinetic energy. (2) [14] Copyright reserved Please turn over

Downloaded from hlayiso.com 6 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) QUESTION 2 (Start on a new page.) Consider the following compounds. O2 ; H2O ; H3O+ 2.1 Define the term molecule. (2) 2.2 Draw the Lewis structures for: 2.2.1 O2 (2) 2.2.2 H2O (2) 2.3 The H3O+- ions forms when the oxygen atom in H2O donates its lone pair of electrons into the vacant orbital of H+. 2.3.1 Write down the NAME of the type of bond described by the underlined phrase. (1) 2.3.2 Draw the Lewis structure for the H3O+-ion. (2) 2.4 Which molecule is polar, H2O or O2? Explain your answer. (4) [13] Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 7 QUESTION 3 (Start on a new page.) The table below shows the relationship between the melting points of three molecules: Molecule Melting point (°C) CH4 -182,5 CF4 -150 CCℓ4 -23 3.1 Define the term melting point. (2) 3.2 Explain the trend in melting points of the molecules in the above table by referring to the intermolecular forces and energy involved. (4) 3.3 Which molecule in the table will have the highest vapour pressure at a given temperature? Explain the answer by referring to the data in the table. (2) 3.4 Water (H2O) is a smaller molecule than CCℓ4, but water has a higher melting point than CCℓ4. Explain this observation by referring to the type of intermolecular forces involved. (2) 3.5 Write down the name of intermolecular force that will exist in a mixture of H2O and CCℓ4. (2) [12] Copyright reserved Please turn over

Downloaded from hlayiso.com 8 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) QUESTION 4 (Start on a new page.) A group of learners investigate the relationship between pressure and the volume of an enclosed gas at room temperature. They recorded their results in the table below: Pressure (kPa) Volume (cm3) 100,33 7,34 102,2 7,21 103,93 7,09 X 6,97 4.1 For this investigation, write down the: 4.1.1 Name of the gas law that is being investigated (1) 4.1.2 Controlled variable (1) 4.1.3 Relationship between pressure and volume of the gas as described by the first 3 data sets in the table (2) 4.2 Calculate the value of X. (4) 4.3 Write down the TWO conditions under which real gases behave more like an ideal gas. (2) 4.4. Write down the NAME of a gas whose behaviour is close to that of an ideal gas, under the conditions mentioned in QUESTION 4.3 above. (1) [11] Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 9 QUESTION 5 (Start on a new page.) 5.1 An organic compound has the following composition by mass. Element Percentage (%) C 54,55 H 9,09 O 36,36 The molar mass of the compound is TWICE the empirical molar mass. 5.1.1 Define the term empirical formula. (2) 5.1.2 Determine, by calculation, the molecular formula of the compound. (5) 5.2 A teacher demonstrates to a group of learners the impact that the limiting reagent have on the amount of product formed during a chemical reaction. The teacher uses the following chemical equation: Zn (s) + 2 HCℓ (aq) → ZnCℓ2 (aq) + H2 (g) The teacher uses the following set-up for this investigation: Experiment 1 Experiment 2 7 g of Zn 3,27 g of Zn 1 mol of HCℓ 1 mol of HCℓ 5.2.1 Define the term limiting reagent. (2) 5.2.2 Determine, by calculation, the limiting reagent in experiment 1. (5) Copyright reserved Please turn over

Downloaded from hlayiso.com 10 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) 5.2.3 How will the amount of zinc chloride (ZnCℓ2) produced in experiment 2, compare to that of experiment 1? Write down only HIGHER THAN, LOWER THAN or EQUAL TO. Explain your answer. (4) 5.2.4 Experiment 2 was carried out at 40 °C. The molar volume of hydrogen gas at this temperature is 25,7 dm3·mol-1. Calculate the volume of hydrogen gas produced once the reaction reaches completion in experiment 2. (5) [23] Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 11 QUESTION 6 (Start on a new page.) 6.1 Consider the following ionisation reaction of HCℓ: HCℓ (g) + H2O (ℓ) ⇌ Cℓ- (aq) + H3O+ 6.1.1 Define an acid in terms of the Lowry-Brønsted model. (2) 6.1.2 Write down ONE conjugate acid-base pair. (2) 6.1.3 Write down the formula of the substance in the reaction that can act as an ampholyte in some reactions. (1) 6.2 A certain volume of a hydrochloric acid solution of concentration 0,5 mol.dm-3 is added to a sample of seashells of mass 8 g in a container. The hydrochloric acid solution (HCℓ) COMPLETELY reacts with the calcium carbonate (CaCO3) in the sample according to the balanced equation: CaCO3 (s) + 2 HCℓ (aq) → CaCℓ2 (aq) + 2 H2O (ℓ) + CO2 (g) ΔH < 0 The seashell contains 95% CaCO3. 6.2.1 Is the reaction ENDOTHERMIC or EXOTHERMIC? Give a reason for the answer. (2) 6.2.2 Calculate the volume, in cm3, of the hydrochloric acid (HCℓ) that was added to the sample inside the container. (7) [14] Copyright reserved Please turn over

Downloaded from hlayiso.com 12 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) QUESTION 7 (Start on a new page.) 7.1 Consider the balanced redox reaction: Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2Ag (s) 7.1.1 Define oxidation. (2) From the balanced equation above, write down the: 7.1.2 Reduction half reaction (2) 7.1.3 Formula of the reducing agent (1) 7.1.4 Explanation for the answer in QUESTION 7.1.3 by referring to the oxidation numbers (2) 7.2 The following INCOMPLETE chemical equation represents a redox reaction: Cr2O72-(aq) + Fe2+(aq) → Cr3+(aq) + Fe3+(aq) 7.2.1 Determine the oxidation number of Cr in Cr2O72-. (2) 7.2.2 Using information from the table of standard reduction potentials write down the BALANCED net ionic reaction. Clearly indicate the following: • Reduction half reaction • Oxidation half reaction • Balanced net ionic equation (4) [13] TOTAL: 100 Copyright reserved Please turn over

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 13 NATIONAL SENIOR CERTIFICATE NASIONALE SENIOR SERTIFIKAAT DATA FOR PHYSICAL SCIENCES GRADE 12 PAPER 2 (CHEMISTRY) GEGEWENS VIR FISIESE WETENSKAPPE GRAAD 12 VRAESTEL 2 (CHEMIE) TABLE 1: PHYSICAL CONSTANTS/TABEL 1: FISIESE KONSTANTES NAAM/NAME SIMBOOL/SYMBOL WAARDE/VALUE Standard pressure p 1,013 × 105 Pa Standaarddruk Molar gas volume at STP Vm 22,4 dm3∙mol-1 Molêre gasvolume teen STD Standard temperature Tθ 273 K Standaardtemperatuur Charge on electron e -1,6 × 10-19 C Lading op elektron Avogadro’s constant NA 6,02 × 1023 mol-1 Avogadro se konstante TABLE 2: FORMULAE/TABEL 2: FORMULES m n m n = M or/of c = V or/of c = MV pH= -log[H3O+] Kw = [H3O+][OH-] = 1x10-14 N ca Va na at /by 298K n= N or/of = A cb Vb n b V n= V m Eθcell = Eθcathode – Eθanode / Eθsel = Eθkatode – Eθanode Eθcell = Eθreduction – Eθoxidation / Eθsel = Eθreduksie – Eθoksidasie Eθcell = Eθoxidising agent – Eθreducing agent / Eθsel = Eθoksideermiddel – Eθreduseermiddel Copyright reserved Please turn over

14 Downloaded from hlayiso.com PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) TABLE 3: THE PERIODIC TABLE OF ELEMENTS/TABEL 3: DIE PERIODIEKE TABEL VAN ELEMENTE 1 2 3 4 5 67 8 9 10 11 12 13 14 15 16 17 18 (I) (II) Atoomgetal (III) (IV) (V) (VI) (VII) (VIII) KEY/ SLEUTEL Atomic number 1 2 H He 2,1 1 29 4 Elektronegatiwiteit Simbool 3 4 1,9 Cu 5 6 7 8 9 10 Electronegativity Symbol Li Be B C N O F Ne 1,0 1,5 63,5 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 Benaderde relatiewe atoommassa 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

Downloaded from hlayiso.com (EC/NOVEMBER 2022) PHYSICAL SCIENCES P2 15 TABLE 4A: STANDARD REDUCTION POTENTIALS TABEL 4A: STANDAARD REDUKSIEPOTENSIALE Half-reactions/Halfreaksies E θ (V) F2(g) + 2e− ⇌ 2F− + 2,87 Co 3+ +e − ⇌ Co2+ + 1,81 H2O2 + 2H+ +2e− ⇌ 2H2O +1,77 − MnO 4 + 8H+ + 5e− ⇌ Mn 2+ + 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− ⇌ Increasing reducing ability/Toenemende reduserende vermoë NO(g) + 2H2O + 0,96 Increasing oxidising ability/Toenemende oksiderende vermoë Hg 2+ + 2e − ⇌ Hg(ℓ) + 0,85 Ag+ + e− ⇌ Ag + 0,80 − NO 3 + 2H+ + e− ⇌ NO2(g) + H2O + 0,80 Fe3+ + e− ⇌ Fe2+ + 0,77 O2(g) + 2H + 2e + − ⇌ H2O2 + 0,68 I2 + 2e− ⇌ 2I− + 0,54 + Cu + e − ⇌ Cu + 0,52 SO2 + 4H + 4e + − ⇌ S + 2H2O + 0,45 2H2O + O2 + 4e− ⇌ 4OH− + 0,40 Cu2+ + 2e− ⇌ Cu + 0,34 2− SO 4 + 4H+ + 2e− ⇌ SO2(g) + 2H2O + 0,17 Cu 2+ +e − ⇌ Cu + + 0,16 Sn4+ + 2e− ⇌ Sn2+ + 0,15 S + 2H+ + 2e− ⇌ H2S(g) + 0,14 + 2H + 2e − ⇌ H2(g) 0,00 Fe3+ + 3e− ⇌ Fe − 0,06 Pb2+ + 2e− ⇌ Pb − 0,13 Sn2+ + 2e− ⇌ Sn − 0,14 Ni 2+ + 2e − ⇌ Ni − 0,27 Co2+ + 2e− ⇌ Co − 0,28 Cd2+ + 2e− ⇌ Cd − 0,40 Cr3+ + e− ⇌ Cr2+ − 0,41 Fe 2+ + 2e − ⇌ Fe − 0,44 Cr3+ + 3e− ⇌ Cr − 0,74 Zn2+ + 2e− ⇌ Zn − 0,76 2H2O + 2e − ⇌ H2(g) + 2OH − − 0,83 Cr2+ + 2e− ⇌ Cr − 0,91 Mn2+ + 2e− ⇌ Mn − 1,18 Aℓ3+ + 3e− ⇌ Aℓ − 1,66 Mg 2+ + 2e − ⇌ Mg − 2,36 Na+ + e− ⇌ Na − 2,71 Ca2+ + 2e− ⇌ Ca − 2,87 Sr2+ + 2e− ⇌ Sr − 2,89 Ba 2+ + 2e − ⇌ Ba − 2,90 Cs+ + e- ⇌ Cs - 2,92 K+ + e− ⇌ K − 2,93 Li+ + e− ⇌ Li − 3,05 Copyright reserved Please turn over

Downloaded from hlayiso.com 16 PHYSICAL SCIENCES P2 (EC/NOVEMBER 2022) TABLE 4B: STANDARD REDUCTION POTENTIALS TABEL 4B: STANDAARD REDUKSIEPOTENSIALE Half-reactions/Halfreaksies E θ (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 2+ Mg + 2e − ⇌ Mg − 2,36 Aℓ3+ + 3e− ⇌ Aℓ − 1,66 Mn2+ + 2e− ⇌ Mn − 1,18 ⇌ Increasing reducing ability/Toenemende reduserende vermoë Cr2+ + 2e− Cr − 0,91 2H2O + 2e− ⇌ H2(g) + 2OH− − 0,83 Increasing oxidising ability/Toenemende oksiderende vermoë Zn2+ + 2e− ⇌ Zn − 0,76 Cr3+ + 3e− ⇌ Cr − 0,74 2+ Fe + 2e − ⇌ Fe − 0,44 Cr3+ + e− ⇌ Cr2+ − 0,41 Cd2+ + 2e− ⇌ Cd − 0,40 Co2+ + 2e− ⇌ Co − 0,28 Ni2+ + 2e− ⇌ Ni − 0,27 Sn2+ + 2e− ⇌ Sn − 0,14 2+ Pb + 2e − ⇌ Pb − 0,13 Fe3+ + 3e− ⇌ Fe − 0,06 2H+ + 2e− ⇌ H2(g) 0,00 S + 2H+ + 2e− ⇌ H2S(g) + 0,14 Sn4+ + 2e− ⇌ Sn2+ + 0,15 2+ Cu + 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 Fe3+ + e− ⇌ Fe2+ + 0,77 − NO 3 + 2H+ + e− ⇌ NO2(g) + H2O + 0,80 Ag+ + e− ⇌ Ag + 0,80 2+ Hg + 2e − ⇌ Hg(ℓ) + 0,85 − NO 3 + 4H+ + 3e− ⇌ NO(g) + 2H2O + 0,96 Br2(ℓ) + 2e − ⇌ 2Br − + 1,07 Pt2+ + 2 e− ⇌ Pt + 1,20 MnO2 + 4H+ + 2e− ⇌ Mn2+ + 2H2O + 1,23 O2(g) + 4H + 4e + − ⇌ 2H2O + 1,23 2− Cr2O 7 + 14H+ + 6e− ⇌ 3+ 2Cr + 7H2O + 1,33 Cℓ2(g) + 2e− ⇌ 2Cℓ − + 1,36 − MnO 4 + 8H+ + 5e− ⇌ 2+ Mn + 4H2O + 1,51 H2O2 + 2H+ +2 e− ⇌ 2H2O +1,77 3+ Co + e − ⇌ Co 2+ + 1,81 F2(g) + 2e− ⇌ 2F− + 2,87 Copyright reserved Please turn over