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NSW HSC 2005 : CHEMISTRY

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2005 H I G H E R S C H O O L C E R T I F I C AT E E X A M I N AT I O N Chemistry Total marks 100 General Instructions Reading time 5 minutes Working time 3 hours Write using black or blue pen Draw diagrams using pencil Board-approved calculators may be used A data sheet and a Periodic Table are provided at the back of this paper Write your Centre Number and Student Number at the top of pages 13, 15, 17, and 21 Section I Pages 2 24 75 marks This section has two parts, Part A and Part B Part A 15 marks Attempt Questions 1 15 Allow about 30 minutes for this part Part B 60 marks Attempt Questions 16 27 Allow about 1 hour and 45 minutes for this part Section II Pages 25 36 25 marks Attempt ONE question from Questions 28 32 Allow about 45 minutes for this section 115 Section I 75 marks Part A 15 marks Attempt Questions 1 15 Allow about 30 minutes for this part Use the multiple-choice answer sheet. Select the alternative A, B, C or D that best answers the question. Fill in the response oval completely. Sample: 2+4= (A) 2 A (B) 6 (C) 8 B C (D) 9 D If you think you have made a mistake, put a cross through the incorrect answer and fill in the new answer. A B C D If you change your mind and have crossed out what you consider to be the correct answer, then indicate the correct answer by writing the word correct and drawing an arrow as follows. correct A B C 2 D 1 Which of the following conditions would produce a radioactive isotope? (A) Too many atoms in the sample provided (B) Too many protons and neutrons in the atom (C) Too many electrons in the outer shell of the atom (D) Too many electrons for the number of neutrons in the atom 2 Which of the following makes cellulose a potential raw material for the petrochemical industry? (A) It is available in many parts of the world. (B) It is light in weight and easy to transport. (C) It is an organic polymer based on carbon. (D) It is a polymer that undergoes combustion. 3 The heat of combustion of butan-1-ol is 2676 kJ mol 1. What is the value of the heat of combustion in kJ g 1? (A) 30.41 (B) 36.10 (C) 44.60 (D) 47.79 3 4 Terylene (polyester) is a condensation polymer. Part of the structure of the polymer is shown. O C C H C O H C H O O O O H C C C O H C H O H H What are the two monomers that form this polymer? Monomer 1 Monomer 2 H H H (B) HO HO H H C C (C) H C C H (A) H OH O HO C C H OH O H OH O H (D) O C H O HO C C H HO OH 4 H C C H O H OH 5 An electrochemical cell is set up as shown in the diagram. V salt bridge Al(s) Cu(s) Al3+(aq) Cu2+(aq) Beaker 1 Beaker 2 What are two observations for this electrochemical cell? Observation 1 Observation 2 (A) In Beaker 2 the solution became a darker blue (B) In Beaker 2 the blue solution faded A reddish precipitate formed on the copper electrode (C) A grey precipitate formed on the aluminium electrode In Beaker 2 the solution became a darker blue (D) 6 A reading was shown on the voltmeter Electrons moved through the voltmeter A reddish precipitate formed on the copper electrode Which of the following is a common use for ethyl pentanoate? (A) Flavouring (B) Fuel (C) Indicator (D) Solvent 5 7 A series of observations was made about a first-hand investigation. A cup of carbonated soft drink was poured from a newly-opened, chilled bottle. A lot of bubbles were observed in the cup. The cup was then left on the kitchen bench for several hours. After this time, it was observed that there were no bubbles visible in the cup. Why were there no bubbles visible in the cup after several hours? (A) The bubbles of carbon dioxide had dissolved into the soft drink. (B) The carbon dioxide had been neutralised by the water in the soft drink. (C) Carbon dioxide is less soluble at higher temperatures and lower pressures. (D) Carbon dioxide is more soluble at higher temperatures and lower pressures. 8 What would be the pH of a 0.1 mol L 1 solution of sulfuric acid? (A) Less than 1.0 (B) Exactly 1.0 (C) Between 1.0 and 7.0 (D) Greater than 7.0 9 Which of the following pairs would form a buffer solution? (A) HCl(aq) / Cl (aq) (B) H2PO4 (aq) / PO43 (aq) (C) H2SO4(aq) / HSO4 (aq) (D) CH3COOH(aq) / CH3COO (aq) 6 10 A titration was conducted by adding NaOH from a teflon-coated burette to HCl in a conical flask. The pH in the flask was recorded during the titration and Curve A was produced. Curve A 14 pH 7 0 0 10 20 30 40 Volume of NaOH added (mL) The table shows appropriate indicators used to identify the equivalence point in titrations. For NaOH and HCl the appropriate indicator is bromothymol blue. Indicator Acidic colour Range of colour change Basic colour Methyl orange red 3.1 4.4 yellow Methyl red red 4.4 6.2 yellow yellow 6.0 7.6 blue Cresolphthalein colourless 8.1 9.7 red Alizarin yellow yellow 10.1 12.0 red Bromothymol blue A second titration was conducted by adding NaOH to a different acid. The pH in the flask was recorded during the titration and Curve B was produced. Curve B 14 pH 7 0 0 10 20 30 40 Volume of NaOH added (mL) What is the appropriate indicator for Curve B using the table? (A) Methyl orange (B) Methyl red (C) Cresolphthalein (D) Alizarin yellow 7 11 Which of the following substances is best analysed by atomic absorption spectroscopy (AAS)? (A) Calcium (B) Iodine (C) Nitrogen (D) Silicon 12 A student performed a sampling technique as part of a first-hand investigation on water quality and repeated the sampling technique several times. What aspect of the experiment was improved by repeating the procedure? (A) Accuracy (B) Reliability (C) Safety (D) Validity 13 What is the name of the following compound? F C C H H F Cl (A) 1,2-difluoro-1-chloroethane (B) 1,2-difluoro-2-chloroethane (C) 1-chloro-1,2-difluoroethane (D) 2-chloro-1,2-difluoroethane 8 H 14 Water quality analyses were performed at different sites on a river shown on the map. Map Town River source River Limestone quarry 50 km The table shows the results of the tests performed at the different sites. Results of tests performed Site Dissolved oxygen (ppm) Biochemical oxygen demand (ppm) pH 1 3 145 5.2 2 10 2 6.9 3 7 12 7.4 Where was each set of tests performed? River source Limestone quarry Town (A) Site 2 Site 1 Site 3 (B) Site 1 Site 2 Site 3 (C) Site 1 Site 3 Site 2 (D) Site 2 Site 3 Site 1 9 15 The Winkler method is used to determine the amount of dissolved oxygen in a sample. In this procedure, oxygen reacts with Mn2+ under alkaline conditions to produce a precipitate of MnO(OH)2. 2Mn2+(aq) + O2(aq) + 4OH (aq) 2MnO(OH)2(s) The precipitate is then dissolved in acid and reacted with iodide, forming iodine and Mn2+. MnO(OH)2(s) + 2 (aq) + 4H+(aq) I2(aq) + Mn2+(aq) + 3H2O(aq) Finally, the amount of iodine produced is determined by reaction with thiosulfate. I2(aq) + 2S2O32 (aq) 2 (aq) + S4O62 (aq) When a sample of water was analysed using the Winkler method, a total of 0.60 mol of thiosulfate was used in the reaction. How many moles of oxygen were present in the original sample? (A) 0.15 (B) 0.30 (C) 0.60 (D) 1.20 10 BLANK PAGE 11 BLANK PAGE 12 Board of Studies NSW 2005 2 005 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Part B 60 marks Attempt Questions 16 27 Allow about 1 hour and 45 minutes for this part Student Number Answer the questions in the spaces provided. Show all relevant working in questions involving calculations. Marks Question 16 (5 marks) During your practical work you performed a first-hand investigation to distinguish between an alkene and the corresponding alkane. (a) Name the alkene used in your investigation. 1 ............................................................................................................................... (b) Identify a potential hazard in your investigation, and outline how you addressed this hazard. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Outline the procedure you used for your first-hand investigation. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 116 13 2 Marks Question 17 (3 marks) The heat of combustion of ethanol is 1367 kJ mol 1. In a first-hand investigation to determine the heat of combustion of ethanol, the experimental value determined differed from the theoretical value. (a) Identify a reason for this difference. 1 ............................................................................................................................... ............................................................................................................................... (b) Calculate the theoretical mass of ethanol required to heat 200 mL of water from 21.0 C to 45.0 C. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 18 (4 marks) Assess the impact of the recent development of a named biopolymer on society and the environment. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 14 Board of Studies NSW 2005 4 2 005 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 19 (4 marks) You have studied one of the cells shown below. Cell X Cell Y Choose ONE of the cells and answer parts (a) and (b). (a) State ONE environmental impact associated with the cell you have chosen. 1 ............................................................................................................................... ............................................................................................................................... (b) Describe the chemistry of the cell you have chosen. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 117 15 3 Marks Question 20 (7 marks) The flow chart shows a series of steps involved in the production of ethyl butanoate. glucose mixture containing ethanol pure ethanol ethyl butanoate Describe the chemistry and procedure involved in each of these steps, using diagrams where appropriate. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 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Analyse how knowledge of the composition and properties of acids has led to changes in the definition of acids. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 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......................................................................................................................................... ......................................................................................................................................... 118 17 5 Marks Question 22 (7 marks) A student carried out a first-hand investigation to identify the relationship between the mass of a metal used in a reaction, and the volume of gas produced. The first-hand investigation was carried out at 25 C, and 100 kPa. In each experiment, 200 mL of hydrochloric acid was added to some zinc, and the volume of gas produced was recorded. The diagram shows the equipment used, and the table contains the student s results. Mass of zinc (g) 0.12 45 0.33 125 0.56 115 0.83 315 0.96 365 1.22 380 1.64 380 1.93 (a) Volume of gas collected at 25 C and 100 kPa (mL) 380 Freely sliding piston 200 mL HCl(aq) Zinc Graph the results from these experiments. Question 22 continues on page 19 18 3 Marks Question 22 (continued) (b) Predict the volume of gas that would be produced in this experiment if 3.00 g of zinc had been used. Justify your answer. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Calculate the theoretical volume of gas produced at 25 C and 100 kPa by the reaction of 0.56 g of zinc with the 200 mL of hydrochloric acid. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 23 (2 marks) (a) 1 What causes incomplete combustion? ............................................................................................................................... ............................................................................................................................... (b) Write a balanced equation for the incomplete combustion of methane. ............................................................................................................................... 19 1 Marks Question 24 (5 marks) An antacid tablet is known to contain calcium carbonate (CaCO3). To determine the mass of calcium carbonate in the tablet, the following procedure was used. The tablet was crushed and then placed in a beaker. A pipette was used to add 25.0 mL of 0.600 mol L 1 hydrochloric acid to the crushed tablet in the beaker. Once the reaction between the calcium carbonate and hydrochloric acid had stopped, phenolphthalein indicator was added to the reaction mixture. A teflon-coated burette was then used to add 0.100 mol L 1 sodium hydroxide to the beaker to neutralise the excess hydrochloric acid. The phenolphthalein changed from colourless to pink after 14.2 mL of the sodium hydroxide solution had been added. (a) Write a balanced chemical equation for the reaction that occurred between the calcium carbonate in the tablet and the hydrochloric acid. 1 ............................................................................................................................... (b) How many moles of hydrochloric acid were added to the tablet? 1 ............................................................................................................................... ............................................................................................................................... (c) Calculate the mass of calcium carbonate in the original antacid tablet. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 20 Board of Studies NSW 2005 3 2 005 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 25 (6 marks) A student collected a 500 mL sample of water from a local creek for analysis. It was filtered and the filtrate evaporated to dryness. The following data were collected. Mass of filter paper 0.16 g Mass of filter paper and solid 0.19 g Mass of evaporating basin Mass of basin and solid remaining (a) 45.33 g 45.59 g Calculate the percentage of total dissolved solids in the creek sample. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) It is suspected that lead has contaminated the creek. Describe a chemical test that could be carried out on the water sample to determine the presence of lead. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) The concentrations of ions in substances used by society need to be monitored. Justify this statement with reference to ONE ion you have studied. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 119 21 2 Question 26 (7 marks) The map shows the catchment for a town water supply. Undisturbed pine forest Logged native forest Lake Undisturbed native forest Vegetable patch Farm Water supply pipe MAP NOT TO SCALE Town Question 26 continues on page 23 22 Dam Marks Question 26 (continued) Describe TWO possible sources of contamination in this catchment, and assess methods that could be used for purifying the water before it reaches the town. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... End of Question 26 23 7 Marks Question 27 (5 marks) The graph shows the variation in concentrations of reactants and product with time for the Haber process. hydrogen Molar concentration nitrogen ammonia T1 (a) Time T2 State why the concentrations of reactants and product do not change between T1 and T2. 1 ............................................................................................................................... ............................................................................................................................... (b) At time T2 the volume of the reaction vessel was reduced. (i) Sketch on the graph how the concentrations of reactants and product would change after the volume was reduced. 2 (ii) Explain the changes shown on your graph. 2 ................................................................................................................... ................................................................................................................... ................................................................................................................... ................................................................................................................... ................................................................................................................... ................................................................................................................... 24 Board of Studies NSW 2005 2 005 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Section II 25 marks Attempt ONE question from Questions 28 32 Allow about 45 minutes for this section Answer the question in a writing booklet. Extra writing booklets are available. Show all relevant working in questions involving calculations. Pages Question 28 Question 29 Shipwrecks, Corrosion and Conservation ............................ 28 29 Question 30 The Biochemistry of Movement .......................................... 30 32 Question 31 The Chemistry of Art ........................................................... 33 34 Question 32 120 Industrial Chemistry ............................................................. 26 27 Forensic Chemistry .............................................................. 35 36 25 Marks Question 28 Industrial Chemistry (25 marks) (a) Sulfuric acid is an important industrial chemical. One of the intermediate products in the synthesis of sulfuric acid is H2S2O7. (i) 1 (ii) (b) What is the name of H2S2O7? With reference to the properties of sulfuric acid, describe safety precautions necessary for its transport. 3 Nitrogen dioxide forms an equilibrium mixture with dinitrogen tetraoxide as shown. 2NO2(g) N2O4(g) At 100 C, K for this reaction is 2.08. At 25 C, a 1.00 L vessel initially contained 0.132 mol of NO2(g). Once equilibrium had been established, there was 0.0400 mol of N2O4(g) in the vessel. (i) 2 (ii) (c) Explain the effects of the addition of a catalyst and an increase in pressure on the yield of N2O4 in this reaction when carried out at 25 C. Calculate the equilibrium constant for this reaction at 25 C, and account for any difference from the K value at 100 C. 4 Advances in chemistry have impacted on the development of technologies. Discuss this statement by analysing changes that have occurred in industrial methods for the production of sodium hydroxide. Question 28 continues on page 27 26 7 Marks Question 28 (continued) (d) The diagram summarises the Solvay process. carbon dioxide sodium bicarbonate carbon dioxide X brine Carbonating tower ammonia ammonium chloride calcium chloride ammonia limestone Heating kiln (i) Identify compound X. 1 (ii) During the Solvay process, ammonia is recovered. 2 Outline the chemistry involved in the recovery of ammonia, and suggest a reason why this recovery is desirable. (iii) Identify possible environmental issues that may arise from the Solvay process, and evaluate methods of dealing with those environmental issues. End of Question 28 27 5 Marks Question 29 Shipwrecks, Corrosion and Conservation (25 marks) (a) (i) Reactive metals such as aluminium and zinc form a strongly adhering oxide coating as a result of the reaction with oxygen. 1 What name is given to these metals? (ii) The hulls of modern ships contain steels that have lower levels of carbon and sulfur than was used in the past. 3 Compare the properties and uses of TWO types of steel that you have studied. (b) (i) Outline ONE factor that influences the rate of corrosion of iron in deep-water wrecks. 2 (ii) A student set up a laboratory experiment in which a beaker contained a strip of magnesium, an iron nail, and a solution of iron(II) sulfate and magnesium sulfate. This was left for several days. 4 Magnesium sulfate/ iron(II) sulfate solution Magnesium Iron nail Describe what would happen in this experiment. Include relevant chemical equations in your answer. Question 29 continues on page 29 28 Marks Question 29 (continued) (c) Advances in chemistry have impacted on the development of technologies. 7 Discuss this statement by analysing current methods of corrosion protection for ships. (d) An iron cannon was recovered from a wreck on the Great Barrier Reef. Reproduced with the permission of the Museum of New Zealand Te Papa Tonarewa The process used to restore the cannon was as follows: Step 1: The cannon was placed in dilute sodium hydroxide for several weeks. During this period, the solution was replaced by fresh dilute sodium hydroxide solution at regular intervals. Step 2: Coral that had grown on the cannon was carefully chipped away. Step 3: Electrolysis was performed on the cannon. Step 4: The restored cannon was then coated in wax. (i) Why was the restored cannon coated in wax? 1 (ii) Explain the purpose of Step 1 in the restoration of the iron cannon. 2 (iii) Describe and justify the procedure for Step 3. Include relevant chemical equations in your answer. 5 End of Question 29 29 Marks Question 30 The Biochemistry of Movement (25 marks) (b) (i) Draw the structure of glycerol. 1 (ii) (a) Explain the viscosity of glycerol and its solubility in water. 3 The diagram below summarises some of the steps involved in respiration. glucose and other sugars Glycolysis pyruvic acid acetyl-CoA C6 C4 TCA Cycle CO2, 2H+ CO2, 2H+ C5 O2 Oxidative phosphorylation H2O (i) Compare the energy output from glycolysis with the total energy output from respiration. 2 (ii) Explain the role of oxidation and reduction in respiration. 4 Question 30 continues on page 31 30 Marks Question 30 (continued) (c) A diagram illustrating the structure of a protein is shown. CH2 OH OC O H CH2C NH H OCH2 + H3N CH 3 CHCH2CH3 C O CH CH 3 CH3 HN + (CH2)4NH3 O OCCH 2 CH2 S S CH2 COO Describe how chemical features affect the structure and shape of proteins, and assess the importance of shape in the current model of enzyme function. Question 30 continues on page 32 31 7 Marks Question 30 (continued) (d) An athletics coach persuaded his runners to drink one of two sports drinks immediately before a race to boost performance. The composition of the two drinks is shown in the table. The coach believes that the sports drinks will give the runners extra energy during both a sprint race and a marathon. Name of sports drink Carbohydrate content (%) Carbohydrate composition Sodium (mg per 500 mL) Athletaid 6 sucrose glucose fructose 225 Energade 8 fructose maltodextrin* 130 *Maltodextrin is a polymer composed of many glucose molecules bonded together. (i) Define the term carbohydrate. 1 (ii) Describe the chemical process involved when humans store carbohydrates for later use. 2 (iii) Use data in the table to assess the hypothesis made by the coach. 5 End of Question 30 32 Marks Question 31 The Chemistry of Art (25 marks) (a) A solution of iron(II) sulfate is mixed with a solution of potassium permanganate under acidic conditions, resulting in a colour change. (i) 1 (ii) (b) What is the observed colour change? Account for the colour change in terms of oxidation states. Include relevant half-equations in your answer. 3 The table provides examples of the colours shown by transition metal complexes. Metal ion Ligand Colour of complex Cu2+ H2O light blue Cu2+ NH3 dark blue Cr3+ H2O green Cr2+ H2O violet (i) 2 (ii) (c) Account for the differences in colours shown by these transition metal complexes. Assess the importance of minerals as pigments to TWO ancient cultures. 4 Describe the methodology and use of laser microspectral analysis, and assess the impact of advances in the understanding of emission spectra on the development of technologies. 7 Question 31 continues on page 34 33 Marks Question 31 (continued) (d) (i) Define the Pauli exclusion principle. 1 (ii) Distinguish between first ionisation energy and electronegativity. 2 (iii) The graph shows the first ionisation energies for the elements helium to neon. 5 2500 2000 First ionisation 1500 energy (kJ mol 1) 1000 500 0 He Li Be B C N O F Ne Analyse the relationship between first ionisation energy and electron configuration, using data from the graph. End of Question 31 34 Marks Question 32 Forensic Chemistry (25 marks) (a) The diagram shows the emission spectra of three elements and an unknown mixture. Na Pb As Unknown mixture Reproduced with the permission of Dr Alan J, Jircitano (i) 1 (ii) (b) Name TWO elements present in the unknown mixture. Describe how emission spectra assist in the identification of elements in a mixture. 3 The diagram illustrates the structure of DNA. X Y Z (i) Identify the components labelled X, Y and Z. 1 (ii) Explain how the analysis of DNA allows for identification of relationships between people. 2 (iii) Discuss the ethics of maintaining data banks of DNA. 3 Question 32 continues on page 36 35 Marks Question 32 (continued) (c) (d) Describe the structure and composition of proteins, and assess the potential of electrophoresis as a method for their analysis. 7 (i) What type of carbohydrate is sucrose? 1 (ii) Describe a chemical test that can be used to distinguish glucose from starch. 2 (iii) A scientist wanted to develop a method of separation for a mixture of six carbohydrates using high performance liquid chromatography. The diagram shows the chromatograms obtained for the mixture using two different solvents as the mobile phase. 5 Awaiting Copyright Clearance Describe high performance liquid chromatography, and assess the effectiveness of the different solvents used by the scientist for separating the mixture of carbohydrates. End of paper 36 Board of Studies NSW 2005 2005 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry DATA SHEET Avogadro constant, NA .................................................................. 6.022 1023 mol 1 Volume of 1 mole ideal gas: at 100 kPa and at 0 C (273.15 K) ...................... 22.71 L at 25 C (298.15 K) .................... 24.79 L Ionisation constant for water at 25 C (298.15 K), Kw ................. 1.0 10 14 Specific heat capacity of water ..................................................... 4.18 103 J kg 1 K 1 Some useful formulae H = m C T pH = log10 [H+ ] Some standard potentials K+ + e 2+ 2+ Ba Ca K(s) 2.94 V + 2e Ba(s) 2.91 V + 2e Ca(s) 2.87 V Na(s) 2.71 V Mg(s) 2.36 V Al(s) 1.68 V + Na + e Mg 2+ 3+ Al + 2e + 3e Mn2+ + 2e Mn(s) H2O + e 1 H2(g) + OH 2 2+ + 2e 2+ 2+ 2+ + 2e 2+ + 2e Zn Fe Ni Sn Pb Zn(s) 0.76 V + 2e Fe(s) 0.44 V + 2e Ni(s) 0.24 V Sn(s) 0.14 V Pb(s) 0.13 V 2 Cu 2+ 1 H2(g) 2 + + 4H + 2e + 2e 1 O2(g) + 2 + H2O + 2e Cu + e +e + Ag + e 1 Br2(l) + e 2 1 Br2(aq) + e 2 1 O2(g) + 2H+ + 2e 2 1 Cl2(g) + e 2 1 Cr2O72 + 7H+ + 3e 2 1 Cl2(aq) + e 2 MnO4 + 8H+ + 5e 1 F2(g) + e 2 120a 0.16 V Cu(s) 0.00 V SO2(aq) + 2H2O 1 I2(s) + e 2 1 I (aq) + e 2 2 3+ Fe 0.83 V H+ + e SO4 1.18 V 0.34 V 0.40 V Cu(s) 0.52 V 2OH I 0.54 V I 0.62 V Fe2+ 0.77 V Ag(s) 0.80 V Br 1.08 V Br 1.10 V H2O 1.23 V 1.36 V Cl 7 Cr3 + + H2O 2 Cl Mn F 1.36 V 1.40 V 2+ + 4H2O 1.51 V 2.89 V Aylward and Findlay, SI Chemical Data (5th Edition) is the principal source of data for this examination paper. Some data may have been modified for examination purposes. 37 38 Yttrium 57 71 Strontium 56 Ba 137.3 Barium 88 Ra [226.0] Radium Rubidium 55 Cs 132.9 Caesium 87 Fr [223.0] Francium Rutherfordium 104 Rf [261.1] Hafnium 72 Hf 178.5 Zirconium 90 Th 232.0 Thorium Actinides 89 Ac [227.0] Actinium Protactinium 91 Pa 231.0 Praseodymium 59 Pr 140.9 Dubnium 105 Db [262.1] Tantalum 73 Ta 180.9 Niobium 41 Nb 92.91 Vanadium Uranium 92 U 238.0 Neodymium 60 Nd 144.2 Seaborgium 106 Sg [266.1] Tungsten 74 W 183.8 Molybdenum 42 Mo 95.94 Chromium Neptunium 93 Np [237.0] Promethium 61 Pm [144.9] Bohrium 107 Bh [264.1] Rhenium 75 Re 186.2 Technetium 43 Tc [97.91] Manganese Platinum 78 Pt 195.1 Palladium 46 Pd 106.4 Nickel Plutonium 94 Pu [244.1] Samarium Americium 95 Am [243.1] Europium 63 Eu 152.0 Meitnerium Hassium 62 Sm 150.4 109 Mt [268] 108 Hs [277] 111 Rg [272] Gold 79 Au 197.0 Silver 47 Ag 107.9 Copper Curium 96 Cm [247.1] Gadolinium 64 Gd 157.3 Berkelium 97 Bk [247.1] Terbium 65 Tb 158.9 Darmstadtium Roentgenium 110 Ds [271] Iridium 77 Ir 192.2 Rhodium 45 Rh 102.9 Cobalt Osmium 76 Os 190.2 Ruthenium 44 Ru 101.1 Iron 28 Ni 58.69 Californium 98 Cf [251.1] Dysprosium 66 Dy 162.5 Mercury 80 Hg 200.6 Cadmium 48 Cd 112.4 Zinc Einsteinium 99 Es [252.1] Holmium 67 Ho 164.9 Thallium 81 Tl 204.4 Indium 49 In 114.8 Gallium 31 Ga 69.72 Fermium 100 Fm [257.1] Erbium 68 Er 167.3 Lead 82 Pb 207.2 Tin 50 Sn 118.7 Germanium 32 Ge 72.64 Silicon 14 Si 28.09 Carbon 6 C 12.01 9 F 19.00 Sulfur Phosphorus Mendelevium 101 Md [258.1] Thulium 69 Tm 168.9 Bismuth 83 Bi 209.0 Antimony 51 Sb 121.8 Arsenic Nobelium 102 No [259.1] Ytterbium 70 Yb 173.0 Polonium 84 Po [209.0] Tellurium 52 Te 127.6 Selenium 34 Se 78.96 16 S 32.07 15 P 30.97 33 As 74.92 Oxygen Nitrogen Lawrencium 103 Lr [262.1] Lutetium 71 Lu 175.0 Astatine 85 At [210.0] Iodine 53 I 126.9 Bromine 35 Br 79.90 Chlorine 17 Cl 35.45 Fluorine 8 O 16.00 7 N 14.01 Where the atomic weight is not known, the relative atomic mass of the most common radioactive isotope is shown in brackets. The atomic weights of Np and Tc are given for the isotopes 237Np and 99Tc. Cerium Lanthanum Lanthanides 57 58 La Ce 138.9 140.1 Actinides 89 103 Lanthanides 39 Y 88.91 38 Sr 87.62 40 Zr 91.22 Titanium Scandium Calcium 27 Co 58.93 30 Zn 65.41 37 Rb 85.47 26 Fe 55.85 29 Cu 63.55 Potassium 25 Mn 54.94 Aluminium 24 Cr 52.00 20 Ca 40.08 19 K 39.10 23 V 50.94 Magnesium Sodium 22 Ti 47.87 13 Al 26.98 Boron 12 Mg 24.31 Name of element 11 Na 22.99 Atomic Weight Gold Beryllium Symbol of element Lithium 21 Sc 44.96 5 B 10.81 79 Au 197.0 3 Li 6.941 Atomic Number KEY 4 Be 9.012 PERIODIC TABLE OF THE ELEMENTS Hydrogen 1 H 1.008 Radon 86 Rn [222.0] Xenon 54 Xe 131.3 Krypton 36 Kr 83.80 Argon 18 Ar 39.95 Neon 10 Ne 20.18 Helium 2 He 4.003

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