Physical Sciences Grade 12 P2 North West June 2024 QP (Eng)

PROVINCIAL ASSESSMENT GRADE 12 PHYSICAL SCIENCES: CHEMISTRY (P2) JUNE 2024 MARKS: 150 TIME: 3 hours This question paper consists of 14 pages and 4 datasheets. Copyright reserved Please turn over

Physical Sciences/P2 2 NW/June 2024 Grade 12 INSTRUCTIONS AND INFORMATION 1. Write your name in the appropriate space on the ANSWER BOOK. 2. This question paper consists of EIGHT 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, 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 NW/June 2024 Grade 12 QUESTION 1: MULTIPLE CHOICE QUESTIONS Various options are provided as possible answers to the following questions. Each question has only ONE correct answer. Write the letter (A–D) next to the question numbers (1.1 to 1.10) in the ANSWER BOOK, for example 1.11 E. 1.1 Which ONE of the following compounds belongs to the same homologous series as an ester? A CH3COCH3 B CH3CH2CH2OH C CH3COOCH3 D CH3CH2CHO (2) 1.2 Molecules with the same molecular formulae, but different types of chains are called … A Positional isomers B Chain isomers C Structural isomers D Functional isomers (2) 1.3 Consider the reaction represented below. CH3CH2CHBrCH3 + H2O CH3CH2CHOHCH3 + HBr Which ONE of the following CORRECTLY gives the type of reaction that takes place and its reaction conditions? TYPE OF REACTION REACTION CONDITIONS A Addition Excess H2O + acid as catalyst B Addition Pt, Pd or Ni as catalyst C Substitution Dilute strong base + mild heat D Substitution Excess H2O + mild heat (2) 1.4 The activation energy for a certain reaction is 70 kJ.moℓ-1. Energy is released when this reaction takes place. Which ONE of the following is correct for the reverse reaction? Activation Energy (EA) Heat of Reaction (H) A EA < 70 kJ.moℓ-1 H > 0 B EA < 70 kJ.moℓ-1 H < 0 C EA > 70 kJ.moℓ-1 H < 0 D EA > 70 kJ.moℓ-1 H > 0 (2) Copyright reserved Please turn over

Physical Sciences/P2 4 NW/June 2024 Grade 12 1.5 The following reaction has reached equilibrium in a closed container at a temperature of 359 K: 4NH3(g) + 5O2(g) ⇋ 4NO(g) + 6H2O(g) + energy Which ONE of the following will increase the equilibrium concentration of NH3? A Add a catalyst. B Remove NO(g) from the container. C Increase the volume of the container. D The temperature is increased to 400 K. (2) 1.6 Which ONE of the following graphs shows the mass of a catalyst against time at the end of the chemical reaction? A B Mass (g) Mass (g) Time (s) Time (s) C D Mass (g) Mass (g) Time (s) Time (s) (2) 1.7 At a temperature of 150°C substances A(g) and B(s) are placed in a closed container. The concentration of A(g) is 0,0002 mol.dm-3 at equilibrium. Equal amounts of P(g) and Q(g) are formed. The Kc value = 0,123 The equilibrium concentrations of P and Q will be … A 1,57 x 10 -2mol.dm-3 B 2,46 x 10 -4mol.dm-3 C 1,23 x 10 -4mol.dm-3 D 4,92 x 10 -4mol.dm-3 (2) Copyright reserved Please turn over

Physical Sciences/P2 5 NW/June 2024 Grade 12 1.8 Which ONE of the following is a conjugate acid-base pair in the following reaction? CH3COOH + NH3 CH3COO- + NH4+ ACID CONJUGATE BASE A NH3 NH4+ B CH3COO- NH4+ C CH3COOH NH3 D CH3COOH CH3COO- (2) 1.9 A weak acid HA dissociates in aqueous solution as shown below. HA (aq) ⇋ H+(aq) + A-(aq) H = + 20 kJmoℓ-1 Which ONE of the following changes will result in an increase in the [H +] of the solution? A Addition of a little aqueous sodium hydroxide solution B Raising the temperature of the solution C Dissolving a little of the sodium salt,NaA, in the solution. D Adding a catalyst to the solution (2) 1.10 Which ONE of the following solutions has the HIGHEST pH value? A 0,1 mol·dm-3 Mg(OH)2 B 0,1 mol·dm-3 NH3 C 0,1 mol·dm-3 HCℓ D 0,1 mol·dm-3 H2SO4 (2) [20] Copyright reserved Please turn over

Physical Sciences/P2 6 NW/June 2024 Grade 12 QUESTION 2 (Start on a new page) Study the following organic compounds, represented by the letters A to I in the table below: A 2-methylpropane F B Butane G C C2H3Br H HC CH H H O D Butan-1-ol I H C C O C H H H E Butan-2-ol 2.1 Write down the letter(s) that represent(s) the following: 2.1.1 Two compounds that are CHAIN ISOMERS. (1) 2.1.2 A PRIMARY alcohol. (1) 2.1.3 A weak MONOPROTIC ACID (1) 2.2 Compound G is a hydrocarbon. 2.2.1 Define the term hydrocarbon. (2) 2.2.2 Is compound G SATURATED or UNSATURATED? Give a reason for your answer. (3) 2.2.3 Write down the IUPAC name of compound G. (2) Copyright reserved Please turn over

Physical Sciences/P2 7 NW/June 2024 Grade 12 2.3 Write down the NAME of the homologous series to which compound C belongs. (2) 2.4 Compound I is the product of an esterification reaction. Write down the: 2.4.1 IUPAC name for compound I (2) 2.4.2 STRUCTURAL formula of the alcohol from which compound I is synthesized (2) 2.4.3 IUPAC name of the carboxylic acid from which it is synthesized (2) 2.5 The table contains compounds which are functional isomers. 2.5.1 Define the term functional isomers. (2) 2.5.2 Write down the LETTERS that represent two compounds that are functional isomers. (2) [22] Copyright reserved Please turn over

Physical Sciences/P2 8 NW/June 2024 Grade 12 QUESTION 3 (Start on a new page.) A student performs an experiment to compare the boiling points of organic compounds belonging to different homologous series. Butan-1-ol, butanoic acid and butanal are used. He then recorded the results on the table given below. Name Boiling point (0 C) Compound A 76 Compound B 118 Compound C 164 3.1 Define the term vapour pressure (2) 3.2 For this experiment give the: 3.2.1 Independent variable (1) 3.2.2 Dependent variable (1) 3.3 Is the boiling point of butan-1-ol HIGHER or LOWER than the boiling point of propan-1-ol? Explain the answer by referring to the INTERMOLECULAR FORCES. (3) 3.4 Write down the STRUCTURAL FORMULA for the FUNCTIONAL group of: 3.4.1 Compound A (2) 3.4.2 Compound C (2) 3.5 Is the vapour pressure of butanal be LOWER or HIGHER than the vapour pressure of butan-1-ol? Explain your answer by referring to the type of INTERMOLECULAR FORCES present and ENERGY. (4) [15] Copyright reserved Please turn over

Physical Sciences/P2 9 NW/June 2024 Grade 12 QUESTION 4 (Start on a new page) Consider the following organic reactions I to IV involving organic compounds A to E. UV light I A + Br2 B + HBr B + concentrated alcoholic KOH → C + KBr + H2O II III 600 (0C) Catalyst IV A C4H10 + E 4.1 For the above reactions, write down the type of: 4.1.1 Reaction I (1) 4.1.2 Reaction III (1) 4.1.3 Reaction IV (1) 4.2 Write down the IUPAC name for compound D. (2) 4.3 Write the molecular formula for each of the following: 4.3.1 Compound A (2) 4.3.2 Compound E (2) 4.4 Draw the structural formula of compound B. (2) 4.5 Write down the balanced chemical equation for complete COMBUSTION of C4H10 using MOLECULAR FORMULAE. (3) 4.6 For Reaction II 4.6.1 Draw the STRUCTURAL FORMULA of compound C (2) 4.6.2 State TWO reaction conditions. (2) [18] Copyright reserved Please turn over

Physical Sciences/P2 10 NW/June 2024 Grade 12 QUESTION 5 (Start on a new page.) 5.1 A group of learners uses the reaction of hydrochloric acid with magnesium ribbon to investigate the factors that influence rate of reaction. The balanced equation for the reaction is given below: Mg(s) + 2HCℓ (ag) MgCℓ2(ag) + H2(g) The hydrochloric acid is in EXCESS, and the same mass of magnesium is used in ALL the experiments. REACTION CONDITIONS Experiment State of division Concentration of Temperature of 0,24g HCℓ(ag)(mol.dm-3) (0C) Magnesium Before After 1 2 35 57 Powder 2 2 30 48 Ribbon 3 2 20 33 Ribbon 4 1,5 30 45 Ribbon 5.1.1 Define the term rate of reaction. (2) 5.1.2 In which experiment is the reaction rate HIGHEST? Explain your answer. (3) 5.2 The reaction in Experiment 2 is compared to the reaction in Experiment 4. 5.2.1 Write down ONE control variable for this comparison. (1) 5.2.2 How does the amount of hydrogen gas produced in Experiment 2 compare to the amount produced in Experiment 4 if the same volume of acid is used in both experiments? Write down only HIGHER THAN, SMALLER THAN or EQUAL TO. Give a reason for your answer. (2) 5.3 Give a reason why it is not a fair test to compare the rate of reaction of Experiment 1 with that of Experiment 3. (1) Copyright reserved Please turn over

Physical Sciences/P2 11 NW/June 2024 Grade 12 5.4 Calculate the mass of hydrochloric acid that remains in the flask at the completion of the reaction in Experiment 1 if the initial volume of the hydrochloric acid is 80 cm3. (7) 5.5 The Maxwell-Boltzman distribution curves labelled P, Q and R for the reactions in experiments 1, 2 and 3 in random order are shown below. Kinetic energy 5.5.1 Write down the name of the label, Y, on the vertical axis. (1) 5.5.2 Which curve (Q, P or R) represents the results of Experiment 3? (1) 5.5.3 With the aid of the collision theory explain the effect of TEMPERATURE on reaction rate. (4) [22] Copyright reserved Please turn over

Physical Sciences/P2 12 NW/June 2024 Grade 12 QUESTION 6 (Start on a new page) Consider the following balanced chemical equation: CH4(g) + 2O2(g) ⇌ CO2(g) + 2H2O(ℓ) Δ H = - 216,7 kJ·moℓ-1 The graph below shows the potential energy against the course of this reaction. 6.1 Define the term activation energy. (2) 6.2 Is the reaction Endothermic or Exothermic? Give a reason for the answer. (3) 6.3 What do the following sections of the graph represents? 6.3.1 RP (1) 6.3.2 QP (1) 6.4 Determine BY CALCULATION the value of X. (3) 6.5 What effect will the addition of suitable catalyst to the reaction mixture have on the activation energy of the reaction? Choose from INCREASES, DECREASES or NO EFFECT. (1) [11] Copyright reserved Please turn over

Physical Sciences/P2 13 NW/June 2024 Grade 12 QUESTION 7 (Start on a new page.) Consider the reaction represented by the balance equation below. 4HCℓ(g) + O2(g) 2H2O(g) + 2Cℓ2(g) ∆H < 0 Initially 1,5 mole of HCℓ(g) and 2 mole of O 2(g) were mixed in a sealed 5 dm3 container which had 18g of H2O(g). The reaction reached equilibrium after 20 minutes at 600°C and 0.6 mole of Cℓ2(g) was present in the container. 7.1 Define the term chemical equilibrium. (2) 7.2 How does the rate of forward reaction compare to the rate of the reverse reaction after 10 minutes? Choose from HIGHER THAN, LOWER THAN or EQUAL TO. (1) 7.3 Calculate the value of Kc at 600°C (8) 7.4 State Le Chatelier’s principle (2) 7.5 The volume of the container is now decreased to 2,5 dm3 while the temperature is kept constant. How will each of the following be affected? Choose from INCREASES, DECREASES or REMAINS THE SAME. 7.5.1 The value of Kc (1) 7.5.2 The mass of Cℓ2(g) in the container. (1) 7.6 Explain your answer to QUESTION 7.5.2 by referring to Le Chatelier’s Principle (2) 7.7 The temperature of the container is now increased, and equilibrium is re- established 7.7.1 How does the new value of Kc at this temperature compare to the one obtained at 600°C? Choose from HIGHER THAN, LOWER THAN or EQUAL TO (1) 7.7.2 Explain the answer to QUESTION 7.7.1 by referring to Le Chatelier’s Principle (2) [20] Copyright reserved Please turn over

Physical Sciences/P2 14 NW/June 2024 Grade 12 QUESTION 8 (Start on a new page.) A group of learners use 35 cm3 standard solution of 0,1 mol.dm-3 sodium hydroxide solution to standardize an oxalic acid solution of volume 40 cm3. At the endpoint, 12 cm3 of the sodium hydroxide remains unreacted. 8.1 Define a standard solution (2) The net ionic equation is given below: C2H2O4 + 2 OH- ⇌ C2O42- + 2H2O 8.2 Identify the conjugate acid-base pairs (4) 8.3 Is oxalic acid a weak or a strong acid? Explain the answer (3) 8.4 H2CO3 undergoes ionisation in a TWO step process as shown below: I H2CO3 + H2O ⇌ HCO3- +H3O+ II HCO3- + H2O ⇌ X + H3O+ 8.4.1 Identify a substance in the above reactions that can act as an ampholyte. (2) 8.4.2 Write down the formula of the substance(s) that is represented by X in reaction II (2) 8.5 A sulphuric acid solution is prepared by dissolving 5,25 g of H 2SO4 in 250 cm3of water. Calculate the following: 8.5.1 The number of moles of sulphuric acid in the original standard solution. (4) 8.5.2 pH of the solution. (5) [22] TOTAL: 150 Copyright reserved

Physical Sciences/P2 1 NW/June 2024 Grade 12 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 NAME/NAAM SYMBOL/SIMBOOL VALUE/WAARDE Standard pressure Standaarddruk p 1,013 x 105 Pa Molar gas volume at STP Vm 22,4 dm3∙mol-1 Molêre gasvolume by STD Standard temperature Standaardtemperatuur T 273 K Charge on electron e -1,6 x 10-19 C Lading op electron Avogadro's constant NA 6,02 x 1023 mol-1 Avogadro-konstante TABLE 2: FORMULAE/TABEL 2: FORMULES m N n n M NA n m V c or/of c n V MV Vm c a v a na  pH = -log[H3O+] c b v b nb Kw = [H3O+][OH-] = 1 x 10-14 at/by 298 K Eθcell  Eθcathode  Eθanode / Eθsel  Ekatode θ  Eθanode or/of Eθcell  Ereduction θ  Eθoxidation / Eθsel  Ereduksie θ  Eθoksidasie or/of agent / Esel  Eoksideermi ddel  Ereduseermi ddel θ θ θ E θcell  E θoxidising agent  Ereducing θ 𝑄 𝑄 n=𝑒 n=𝑞 𝑒 q = I∆t Copyright reserved Please turn over

Physical Sciences/P2 2 NW/June 2024 Grade 12 Copyright reserved Please turn over

Physical Sciences/P2 3 NW/June 2024 Grade 12 TABLE 4A: STANDARD REDUCTION POTENTIALS TABEL 4A: STANDAARD-REDUKSIEPOTENSIALE Half-reactions/Halfreaksies Eθ (V) F2(g) + 2e ⇌ 2F + 2,87 Co3+ + e ⇌ Co2+ + 1,81 H2O2 + 2H+ +2e ⇌ 2H2O +1,77  MnO 4 + 8H+ + 5e ⇌ Mn + 4H2O 2+ + 1,51 Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36 2  3+ Cr2O 7 + 14H + 6e+ ⇌ 2Cr + 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 Increasing strength of reducing agents/Toenemende sterkte van reduseermiddels  Increasing strength of oxidising agents/Toenemende sterkte van oksideermiddels NO 3 + 4H+ + 3e ⇌ NO(g) + 2H2O + 0,96 Hg2+ + 2e ⇌ Hg(ℓ) + 0,85 Ag+ + e ⇌ Ag + 0,80  NO 3 + 2H+ + e ⇌ NO2(g) + H2O + 0,80 Fe3+ + e ⇌ Fe 2+ + 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 Cu2+ + 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  0,13 oksiderende vermoë ⇌ Pb 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 2H2O + 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 NW/June 2024 Grade 12 TABLE 4B: STANDARD REDUCTION POTENTIALS TABEL 4B: STANDAARD-REDUKSIEPOTENSIALE 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 Increasing strength of oxidising agents/Toenemende sterkte van oksideermiddels Increasing strength of reducing agents/Toenemende sterkte van reduseermiddels Mn2+ + 2e ⇌ Mn  1,18 Cr2+ + 2e ⇌ Cr  0,91 2H2O + 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 Cd2+ + 2e ⇌ Cd  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 ⇌ H2S(g) + 0,14 Sn4+ + 2e ⇌ Sn2+ + 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 Fe3+ + e ⇌ Fe2+ + 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 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 ⇌ 2Cr3+ + 7H2O + 1,33 Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36  2+ MnO 4 + 8H+ + 5e ⇌ Mn + 4H2O + 1,51 +  ⇌ 2H2O +1,77 H2O2 + 2H +2 e Co3+ + e ⇌ Co2+ + 1,81 F2(g) + 2e ⇌ 2F + 2,87 Copyright reserved