Gr10 Physics P2 Exam Nov 2024 PDF

NATIONAL SENIOR SERTIFICATE GRADE 10 NOVEMBER 2024 PHYSICAL SCIENCES P2 FINAL EXAMINATION MARKS: 100 DURATION: 2 hours This question paper consists of 10 pages and 2 da...

NATIONAL SENIOR SERTIFICATE GRADE 10 NOVEMBER 2024 PHYSICAL SCIENCES P2 FINAL EXAMINATION MARKS: 100 DURATION: 2 hours This question paper consists of 10 pages and 2 data sheets.  2 INSTRUCTIONS AND INFORMATION 1. This question paper consists of EIGHT questions. Answer ALL the questions in the ANSWER BOOK. 2. H question on a NEW page in the ANSWER BOOK. 3. the answers correctly according to the numbering system used in this. , paper. 4. Leave ONE line between two sub-questions, for example between QUESTION 2.1 and QUESTION 2.2. 5. You may use a non-programmable calculator. 6. You may use appropriate mathematical instruments. 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.  3 QUESTION 1: MULTIPLE-CHOICE QUESTIONS Four 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 number (1.1-1.5) in the ANSWER BOOK, for example 1.6 D. 1.1 the following is not a property of a metal? A B Ductile and malleable C Thermal conductor D Insulator of electricity (2) 1.2 An investigation is conducted to study the effect of temperature on the conductivity of a substance. The results are represented in the graph below. f ti I 'C ­ c 0 0 Which ONE of the following is the substance being investigated? A Copper B Aluminium C Silicon D Zinc (2)  4 1.3 Which one of the following is an example of a chemical change? A arating oil and water mixture using a decanter. B -. densation of water vapour. C gnesium burning in air. D Dissolving sugar in water. (2) 1.4 Consider the balanced chemical equation below: 4At(s) + 3O2(g) -» 2At0(s) Which one of the following is the correct number of oxygen atoms required to form 4 moles of aluminium oxide (At2Oa)? A 6x6,02x10° 8 12x6,02x103 C 3x6,02x10° D 36x6,02x10° (2) 1.5 Consider the unbalanced chemical equation below: NH + O2 NO + H2O Which ONE of the sets of coefficients will balance the equation? A 2, 2, 2, 3 B 2,3,2,3 C 5 , 4 , 5, 6 D 4, 5, 4, 6 (2)  5 QUESTION 2 (Start on a new page.) Four different substances, w, X, Y and z are represented in the table below. Substance w Substance X KEY O -warooen 0o 0o @ -mo 0o Substance Y Substance Z - N i t ro g e n 1 e........ -Oxygen I ,.......... gt 0o 2.1 Is Substance X an ELEMENT or a COMPOUND? Give a reason for the answer. (2) 2.2 Write down the LETTER of the substance that represents a mixture. (1) 2.3 Write down the COMMON NAME of Substance Y. (1) 2.4 Draw the Lewis structure of Substance Y. (2) 2.5 Identify the type of chemical bond between atoms in Substance W. (1) 2.6 Hydrogen gas and Nitrogen gas reacts to produce Substance Y. 2.6.1 Write down a BALANCED chemical equation for the reaction that (3) takes place. 2.6.2 Is this a synthesis or decomposition reaction? Give a reason for the answer. (2) 2.6.3 Use the balanced chemical equation from Question 2.6.1 to prove the law of conservation of mass in this reaction. (3) (15)  6 QUESTION 3 (Start on a new page.) 3.1 The cooling curve of ETHANOIC ACID is represented in the graph below. The ot drawn to scale. The Cooling Curve of Ethanoic Acid B 118 - --- - -.. - - - - - - - - - - - - - - - - , - - - - - - - - - - , 16 - - - - - - - - - - - - - --:----- - - - - - - - - - --- ---:-.. ' ' C ' ' ' ' 0 10 20 80 90 95 Time (min) 3.1 Define the term melting point in words. (2) 3.2 What is the melting point of ethanoic acid? (1) 3.3 Are the forces between particles stronger in ETHANOIC ACID or in WATER? (2) Give a reason for the answer. 3.4 Write down the phase of ethanoic acid at 5 minutes. (1) 3.5 Write down the name given to the phase change occurring between 10 and 20 minutes. (1) 3.6 Explain why the change referred to in QUESTION 3.5 is a Physical Change. (2) 3.7 At which points, A, B or C a r e the following statements applicable? 3.7.1 The forces between particles are the strongest. (1) 3.7.2 The spaces between the particles are the largest (1) 3.7.3 The kinetic energies of the particles remain constant. (1)  7 QUESTION 4 (Start on a new page.) Some information for the substances IRON and the SULPHIDE ION are given in the table below. Number of Number of Number of Name ymbol protons electrons neutrons IRON Fe 4.1.1 26 4.1.2 SULPHIDE ION 4.1.3 16 4.1.4 16 4.1 Complete the table by providing the answers to questions 4.1.1 to 4.1.4. Do not redraw the table. Write the numbers (4.1.1-4.1.4) down and the correct answer next to it. (4) 4.2 Draw the aufbau diagram and write down the electronic configuration (sp-notation) for the sulphide ion. (3) 4.3 How many valence electrons does the sulphide ion have? (1) 4.4 Iron (Fe) has three common isotopes as indicated below Isotope Percentaae Abundance Fe - 54 5,8 % Fe - 5 6 91,7% Fe-57 REMAINDER 4.4.1 Define the term isotope in words. (2) 4.4.2 Determine the relative atomic mass of Iron (Fe). (3)  8 QUESTION 5 (Start on a new page.) 5.1 The table below shows the first and second ionisation energies of elements in PERIOD 2 of the periodic table. IRST IONISATION ENERGY SECOND IONISATION ENERGY J.mol') (kJ.mol) Li r-- 520 7 297 Be 899 1 757 B 801 2 427 C 1086 2 352 N 1402 2 854 0 1214 3 391 F 1681 3 381 Ne 2 080 3 964 5. 1. 1 Explain why there is a general increase in the first ionisation energy on going from left to right across the period. (2) 5.1.2 It is observed that the second ionisation energy of Li {Lithium) is considerably higher than Be (Beryllium). Explain this observation. (2) 5.1.3 Write down the NAME of the group whose elements have the highest first ionisation energy in the period. (1) 5.2 Write down the CHEMICAL FORMULA for: 5.2.1 Sodium oxide () 5.2.2 Calcium phosphate (1) 5.2.3 Copper (II) carbonate (1) 5.3 Write down the CHEMICAL NAME for: 5.3.1 MgBr2 (1) 5.3.2 (NH4)»SO4 (1) (10) QUESTION 6 (Start on a new page) Sulphur dioxide (SO2) reacts with oxygen (O2) to form sulphur trioxide (SOs), as shown in the balance uation below. 2$O2(g) + O2(g) - 2SO»(g) In one such reaction 2450 cm? sulphur trioxide (SO3), is formed at STP. 6.1 State Avogadro's law in words. (2) 6.2 Calculate the: 6.2.1 Number of moles of so, that formed. (4) 6.2.2 Mass of so, that reacted. (4) 6.2.3 Number of oxygen (O2) molecules that reacted (4) QUESTION 7 (Start on a new page) 7.1 The analysis of a compound made up of the elements sodium (Na), sulphur (S) and oxygen (0) provides the following percentage composition, by mass. Element Percenta osition Na s 40,51 Ox en O 30.38 7.1.1 Define the term empirical formula in words. (2) 7.1.2 Determine the empirical formula of this compound (5) 7.2 Determine the percentage composition of water (HO) in hydrated copper sulphate (CuSO+·5HO). (4)  10 QUESTION 8 (Start on a new page) Calcium c a r b on at e (CaCOa) reacts completely with excess phosphoric acid (HPOL) of concentration.?' moldm3 The reaction presented by the following balanced equation: aracOs(s) + 2H3PO4(aq) -» Ca(P0)2(a0) + 3C02(g) + 3HO(t The graph below (not drawn to scale), shows the mass of the calcium carbonate (CaCO3) as the reaction progresses $ 25 6 20 8 u r & s5 > WW Lua[i Time (min) 0 1 2 3 4 8.1 Determine the number of moles of Ca3(PO±) FORMED AFTER 1 M I N U T E. (5) The reaction is thereafter allowed to reach completion. 8.2 Determine the number of moles of calcium carbonate (CaCO) used. (2) 8.3 Calculate the volume of phosphoric acid that reacts with the calcium carbonate after 4 MINUTES. (4) 8.4 Calculate the percentage yield of carbon dioxide (CO2), if 4 dm? of CO was formed at STP. (4) TOTAL: 100  11 DATA FOR PHYSICAL SCIENCES GRADE 10 CHEMISTRY TABLE 1: PHYSICAL CONSTANTS NAME SYMBOL VALUE Standard pressure p" 1 , 0 1 3 x 10° Pa Molar gas volume at STP 22,4 dm?·mol' Va Standard temperature ro 273 K Avogadro's constant N» 6,02 x 10° mol' TABLE 2: FORMULAE m N f=­ fl M N, n m V C= or C­ fl = V MV v,  TABLE 3: THE PERIODIC TABLE OF ELEMENTS 1 2 3 4 5 8 9 10 11 12 13 14 15 16 17 18 (I) (II) (Ill) (IV) (V) (VI) (VII) (VIII) omic num ber 1 KEYISLEUTEL 2 if Atopmgetal av H He 1 4 29 3 4 Electronegativity_, Symbol 5 6 7 8 9 10 o Cu c ei Li.. Lo Be E/ektronegatiwiteit f 63,5 Simbool o eN B u av C c c N Lo c 0 o er F Ne 7 9 11 12 14 16 19 20 11 12 T 13 14 15 16 17 18 0 c Na.. c Mg Approximate relative atomic mass A€.. 00 Si et av p u av s z ce Ar Benaderde relatiewe atoommassa 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 00 o 0 Luo NiI c K i Ca i Sc T Ti "' +i V < cr Mn Fe 3 co ,. z cu z zn z Ga Ge 3 A s Se 3 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 00 o ¢V «t ,._ Luo c Rb i Sr i y T Zr Nb Mo Tc Ru Rh Pd 3Ag Cd er In z Sn 3 Sb Te v 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 co > o» o Cs o Ba La el Hf Ta w Re Os Ir Pt Au Hg Te Pb BiI $Po < At Rn 133 137 139 179 181 184 186 190 192 195 197 201 204 207 209 87 88 89 p 0 c Fr c Ra Ac 58 59 60 61 62 63 64 65 66 67 68 69 70 71 226 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