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NSW HSC 2006 : CHEMISTRY

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2006 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 9, 11, 15, 17, 21 and 25 Section I Pages 2 27 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 28 Allow about 1 hour and 45 minutes for this part Section II Pages 29 40 25 marks Attempt ONE question from Questions 29 33 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 is the main industrial source of ethylene? (A) Ethanol (B) Glucose (C) Petroleum (D) Polyethylene 2 Catalysts are required for the production of both ethanol from ethylene and ethylene from ethanol. ethylene + water Catalyst A Catalyst B What are the identities of Catalyst A and Catalyst B ? Catalyst A (A) dilute H+ conc H+ (B) dilute H+ dilute H+ (C) conc H+ conc H+ (D) 3 Catalyst B conc H+ dilute H+ Which set contains only stable nuclei? (A) 2 1H 12 6C 238 92 U (B) 16 8O 39 19 K 12 6C (C) 65 30 Zn 18 8 8O 24 12 Mg (D) 14 6C 16 8O 1 1H 3 ethanol 4 A student used the apparatus shown to determine the molar heat of combustion of ethanol. Thermometer Can containing 300 g water Burner containing ethanol The following results were obtained. Initial mass of burner 133.20 g Final mass of burner 132.05 g Initial temperature of water 25.0 C Final temperature of water 45.5 C What is the molar heat of combustion calculated from this data? (A) 22.4 kJ mol 1 (B) 25.7 kJ mol 1 (C) 1030 kJ mol 1 (D) 1180 kJ mol 1 5 How many isomers are there for C3H6Cl2? (A) 3 (B) 4 (C) 5 (D) 6 4 6 Glucose (C6H12O6) is a monomer that can form naturally occurring polymers. The approximate atomic weights for the elements which make up glucose are shown in the table. Element Approximate atomic weight Carbon 12 Hydrogen 1 Oxygen 16 Using data from the table, what would be the approximate molecular weight of a polymer made from 5 glucose monomers? (A) 810 (B) 828 (C) 882 (D) 900 7 Which class of compounds typically has a sweet smell? (A) Esters (B) Alkenes (C) Haloalkanes (D) Alkanoic acids 8 Acid X is 0.1 mol L 1 hydrochloric acid. Acid Y is 1.0 mol L 1 acetic acid (ethanoic acid). How does acid X compare with acid Y ? (A) X is weaker and more dilute than Y. (B) X is stronger and more dilute than Y. (C) X is weaker and more concentrated than Y. (D) X is stronger and more concentrated than Y. 5 9 Which statement best describes the equivalence point in a titration between a strong acid and a strong base? (A) The point at which the first sign of a colour change occurs (B) The point at which equal moles of acid and base have been added together (C) The point at which equal moles of H+ ions and OH ions have been added together (D) The point at which the rate of the forward reaction equals the rate of the reverse reaction 10 Phosphorus pentoxide reacts with water to form phosphoric acid according to the following equation. P2O5(s) + 3H2O(l ) 2H3PO4(aq) Phosphoric acid reacts with sodium hydroxide according to the following equation. H3PO4(aq) + 3NaOH(aq) Na3PO4(aq) + 3H2O(l ) A student reacted 1.42 g of phosphorus pentoxide with excess water. What volume of 0.30 mol L 1 sodium hydroxide would be required to neutralise all the phosphoric acid produced? (A) 0.067 L (B) 0.10 L (C) 0.20 L (D) 5.0 L 11 In 1884, Svante Arrhenius proposed a definition for acids. His definition was soon accepted as superior to that put forward by earlier chemists. Why was Arrhenius definition seen as a major improvement? (A) It explained why some acids do not contain oxygen. (B) It showed how the solvent can affect the strength of an acid. (C) It showed the relationship between pH and the concentration of H+ ions. (D) It could be used to explain why some acids are strong and others are weak. 6 12 Which statement explains why catalysts are often used in chemical reactions? (A) Catalysts increase the rate of reactions. (B) Catalysts increase the yield of products of reactions. (C) Catalysts increase the purity of products of reactions. (D) Catalysts increase the activation energies of reactions. 13 Why are microscopic membrane filters useful for water purification? (A) They can kill bacteria. (B) They adjust the pH of water to 7. (C) They are composed of biodegradable polymers. (D) They can remove very small particles from water. 14 A scientist used atomic absorption spectroscopy (AAS) to analyse the concentration of iron in a sample of water. The scientist analysed the sample five times and obtained the absorbances shown in the table. Analysis Absorbance 1 0.390 2 0.392 3 0.249 4 0.387 5 0.394 The scientist needed an average absorbance to determine the concentration of iron from a calibration curve. Which value should the scientist use? (A) 0.362 (B) 0.3624 (C) 0.39075 (D) 0.391 7 Which graph shows how pressure and temperature affect the yield of ammonia produced by the Haber process? % yield of ammonia (A) 80 70 60 50 40 30 20 10 0 350 C 400 C 450 C 500 C 550 C 100 200 300 400 Pressure (atmosphere) % yield of ammonia (B) 80 70 60 50 40 30 20 10 0 550 C 500 C 450 C 400 C 350 C 100 200 300 400 Pressure (atmosphere) % yield of ammonia (C) 80 70 60 50 40 30 20 10 0 550 C 500 C 450 C 400 C 350 C 100 200 300 400 Pressure (atmosphere) (D) % yield of ammonia 15 80 70 60 50 40 30 20 10 0 350 C 400 C 450 C 500 C 550 C 100 200 300 400 Pressure (atmosphere) 8 Board of Studies NSW 2006 2 006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Part B 60 marks Attempt Questions 16 28 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 (3 marks) Describe how technology has enabled the transuranic elements to be produced. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 116 9 3 Marks Question 17 (4 marks) (a) Calculate the pH of a 0.2 mol L 1 solution of hydrochloric acid. 1 ............................................................................................................................... ............................................................................................................................... (b) Calculate the pH after 20 mL of 0.01 mol L 1 sodium hydroxide is added to 50 mL of 0.2 mol L 1 hydrochloric acid. Include a balanced chemical equation in your answer. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 10 Board of Studies NSW 2006 3 2006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 18 (4 marks) A student studying the mass change that occurs during fermentation added glucose, water and yeast to a flask and stoppered the flask with some cotton wool. The student measured the mass of the flask daily for seven days. The table shows the data collected. Day 1 381.05 2 376.96 3 373.42 4 370.44 5 370.42 6 370.40 7 (a) Mass (g) 370.39 Calculate the moles of CO2 released between days 1 and 7. 1 ............................................................................................................................... ............................................................................................................................... (b) Calculate the mass of glucose that underwent fermentation between days 1 and 7. Include a balanced chemical equation in your answer. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 117 11 3 Marks Question 19 (7 marks) A student was asked to perform a first-hand investigation to measure the difference in potential of various combinations of metals in an electrolyte solution. The student was provided with three metals: aluminium, zinc and silver; and three electrolyte solutions: aluminium nitrate, zinc nitrate and silver nitrate. (a) Identify which combination of the metals supplied should give the highest potential difference. 1 ............................................................................................................................... (b) Sketch and label a diagram of an experimental setup that the student could use with the combination of metals identified in part (a). 2 (c) Write a balanced chemical equation for the overall reaction for the metals identified in part (a), and calculate the expected potential difference. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 19 continues on page 13 12 Marks Question 19 (continued) (d) The measured potential difference obtained varied from the theoretical value. Outline steps the student could have taken to minimise this variation. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 19 13 2 BLANK PAGE 14 Board of Studies NSW 2006 2006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 20 (7 marks) Analyse why ethylene is such an important starting material for the chemical industry. In your answer, include relevant chemical equations, and a description of new materials and fuels that can be prepared from ethylene. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 118 XXX 15 7 Marks Question 21 (3 marks) You performed a first-hand investigation to identify the pH of a range of salt solutions. (a) Identify an acidic salt you used. 1 ............................................................................................................................... (b) Explain the acidic nature of the salt you selected. Include a balanced chemical equation in your answer. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 16 Board of Studies NSW 2006 2 2006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 22 (4 marks) The atmosphere contains acidic oxides of sulfur which have been increasing in concentration since the Industrial Revolution. Discuss the evidence for this statement, and include relevant balanced chemical equations. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 118a 17 4 Marks Question 23 (6 marks) Correct swimming pool maintenance requires regular monitoring of the pH level of the water. (a) Select the best indicator from the graph to check that the pH of swimming pool water lies within the correct range of 7.0 7.6. Justify your choice. Methyl orange Bromothymol blue Phenolphthalein red yellow yellow blue pink colourless 1234567 8 9 10 11 12 13 pH ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 23 continues on page 19 18 3 Marks Question 23 (continued) (b) Another part of swimming pool maintenance is adjusting chlorine levels in the pool. Liquid chlorine is a solution of sodium hypochlorite (NaOCl) which can be used to do this. Upon addition of sodium hypochlorite to the pool, the following equilibrium reaction occurs: OCl (aq) + H2O(l) (i) HOCl(aq) + OH (aq) State a reason for the regular chlorination of swimming pool water. 1 ................................................................................................................... ................................................................................................................... (ii) Explain how the addition of sodium hypochlorite will affect the pH of the water in the pool. ................................................................................................................... ................................................................................................................... ................................................................................................................... ................................................................................................................... End of Question 23 19 2 BLANK PAGE 20 Board of Studies NSW 2006 2 006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 24 (5 marks) Early in the twentieth century, Fritz Haber developed a method for preparing ammonia. (a) Write a balanced chemical equation for the preparation of ammonia using the Haber process. 1 ............................................................................................................................... (b) Evaluate the significance of Haber s discovery at that time in world history. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 119 21 4 Marks Question 25 (5 marks) Atomic absorption spectroscopy was used to analyse a set of standard solutions of copper. The results are presented in the table. Concentration of copper (ppm) 0 0 5 0.20 10 0.39 15 0.52 20 0.64 25 (a) Absorbance 0.77 2 Draw an appropriate graph of the data. 1.00 Absorbance 0.80 0.60 0.40 0.20 0 0 5 10 15 20 25 Concentration of copper (ppm) Question 25 continues on page 23 22 30 35 Marks Question 25 (continued) (b) An analysis of two samples containing copper was then performed. The results are given in the table. Sample Absorbance 1 0.44 2 0.90 Use your graph to estimate the concentration of copper present in the samples, and assess the validity of each of your estimates. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 25 23 3 BLANK PAGE 24 Board of Studies NSW 2006 2006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 26 (4 marks) The flow diagram shows a series of tests that can be used to identify carbonate, chloride and sulfate ions present in a sample. Sample Step 1 Add excess HNO (aq) 3 Bubbles observed Step 2 Add excess Ba2+(aq) White precipitate forms Step 3 Filter off precipitate Add Ag+(aq) to the filtrate White precipitate forms (a) Identify the gas observed during Step 1. 1 ............................................................................................................................... (b) Explain why the analysis must be performed in the sequence given. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 119a 25 3 Marks Question 27 (4 marks) One of the most common methods for determining the concentration of metal ions in water samples involves titration with a reagent called EDTA. In alkaline solution EDTA is present as an anion with a 4 charge. In this form it reacts with metal ions such as calcium and magnesium in a 1 : 1 ratio: Ca2+ + EDTA4 Ca(EDTA)2 When the reaction between the metal ions and EDTA4 is complete, an indicator also present in the solution changes colour. A student used the following procedure to determine the concentration of calcium in a sample of water: 50.0 mL of water sample was pipetted into a conical flask 5.0 mL of ammonia/ammonium ion buffer and two drops of indicator were added Sample was titrated with 0.0200 mol L 1 EDTA4 until indicator changed colour The above procedure was repeated a further three times The average volume of EDTA4 used in the four titrations was 24.0 mL (a) What is the average number of moles of EDTA4 added to reach the end point? 1 ............................................................................................................................... ............................................................................................................................... (b) The student used the answer to part (a) to calculate the concentration of Ca2+ in the water sample in mg L 1. 2 What concentration was obtained? ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) The concentration of Ca2+ in the water sample was also determined by atomic absorption spectroscopy, and found to be 16% lower than the value obtained by titration with EDTA4 . Suggest a reason why the concentration of Ca2+ determined by EDTA titration was higher. ............................................................................................................................... ............................................................................................................................... 26 1 Marks Question 28 (4 marks) The diagram shows recent atmospheric ozone concentrations above Antarctica. Dobson Units 100 200 300 400 500 Explain how this information was obtained, and outline the changes that have occurred in atmospheric ozone concentrations above Antarctica during the past twenty years. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 27 4 BLANK PAGE 28 Board of Studies NSW 2006 2 006 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Section II 25 marks Attempt ONE question from Questions 29 33 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 29 Question 30 Shipwrecks, Corrosion and Conservation ............................ 32 33 Question 31 The Biochemistry of Movement .......................................... 34 36 Question 32 The Chemistry of Art ........................................................... 37 38 Question 33 120 Industrial Chemistry ............................................................ 30 31 Forensic Chemistry .............................................................. 39 40 29 Marks Question 29 Industrial Chemistry (25 marks) (a) During your practical work you performed a first-hand investigation to identify the products of electrolysis of sodium chloride. (i) 3 (ii) (b) Outline a risk assessment for this investigation, and show how this would influence the experimental procedure. Provide a conclusion based on one set of observations from your first-hand investigation. 2 The diagram represents how one class of molecules assembles in water to form a structure called a micelle. Na+ Na+ Na+ CH3 (CH2)13 Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ SO3 Na+ Na+ (i) 1 (ii) Account for the formation of a micelle. 2 (iii) (c) Identify the class of molecules shown. Explain what happens when oil is added to water containing these molecules. 3 In this option you studied one natural product that was not a fossil fuel. Describe the issues associated with shrinking world supplies of this natural product, and evaluate progress being made to solve the problems identified. Question 29 continues on page 31 30 7 Marks Question 29 (continued) (d) The diagram summarises the steps in the Contact process. Oxygen from air X Step 1 Oxygen from air Sulfur dioxide Step 2 Sulfur trioxide Step 3 Sulfuric acid (i) Identify the starting material, X, for the first step in the Contact process. 1 (ii) Outline the chemistry involved in the conversion of sulfur trioxide to sulfuric acid. 2 (iii) Justify the conditions you would use to maximise the rate and yield of the second step in the Contact process. Include a balanced chemical equation in your answer. 4 End of Question 29 31 Marks Question 30 Shipwrecks, Corrosion and Conservation (25 marks) (a) During your practical work you performed a first-hand investigation to identify the factors that affect the rate of an electrolysis reaction. (i) 3 (ii) (b) Outline a risk assessment for this investigation, and show how this would influence the experimental procedure. Provide a conclusion based on one set of observations from your first-hand investigation. 2 The diagram shows the wreck of an iron ship sitting on the bottom of the ocean at a great depth. Ocean water Sulfate-reducing bacteria microenvironment Ocean floor Acidic microenvironment (i) Identify the gas dissolved in water that causes corrosion. 1 (ii) Outline the effect of temperature and pressure on the solubility of gases in water. 2 (iii) Microenvironments are localised areas where conditions are different from those in the surrounding areas. 3 Explain the effect of each microenvironment on the rate of corrosion of the iron ship. Include at least one balanced chemical equation in your answer. Question 30 continues on page 33 32 Marks Question 30 (continued) (c) The diagram shows artefacts recovered from a shipwreck. Wooden chest Encrusted copper coins 7 Lead cannon balls Describe how these artefacts may have been affected by prolonged exposure to the marine environment, and analyse the role of chemistry in procedures used for restoration of such objects. (d) The diagram shows that iron is an important construction material for an oil rig. Iron tower Iron pylon Ocean surface (i) Identify the name for alloys composed of iron and carbon. 1 (ii) Outline the process of rusting. 2 (iii) Describe TWO methods for preventing corrosion of iron, and assess their suitability for use in different parts of the oil rig. 4 End of Question 30 33 Marks Question 31 The Biochemistry of Movement (25 marks) (a) During your practical work you performed a first-hand investigation to observe the effect of changes in pH and temperature on the reaction of an enzyme. (i) 3 (ii) (b) Outline a risk assessment for this investigation, and show how this would influence the experimental procedure. Provide a conclusion based on one set of observations from your first-hand investigation. 2 (i) Identify the part of the cell where glycolysis occurs. 1 (ii) The diagram shows ATP which is used in many metabolic processes. 2 NH2 N O O P O O O P O O O P H O CH2 C C N C C N C H N O O H H OH H OH H Account for the widespread use of ATP in metabolism. (iii) Enzymes usually show a high degree of substrate specificity in the reactions they catalyse. Explain how this specificity is achieved. Question 31 continues on page 35 34 3 Marks Question 31 (continued) (c) Increased understanding of how the body produces energy has led to a number of weight loss diets. Several of these promote a diet low in carbohydrates. The diagram summarises how two of the food groups used by the body are metabolised to produce energy. Food Fats Carbohydrates Acetyl CoA TCA cycle Oxidative phosphorylation Describe how carbohydrates and fats are metabolised to produce energy, and explain how a diet low in carbohydrates might lead to weight loss. Question 31 continues on page 36 35 7 Marks Question 31 (continued) (d) The diagram represents the structure of a relaxed skeletal muscle cell. Muscle cell Myofibril Myosin Actin (i) Identify the class of molecules to which myosin and actin belong. 1 (ii) Contrast the appearance and function of type 1 and type 2 skeletal muscle cells. 2 (iii) Describe how muscle contractions occur, and explain how a contraction would change the appearance of the muscle cell in the diagram above. 4 End of Question 31 36 Marks Question 32 The Chemistry of Art (25 marks) (a) During your practical work you performed a first-hand investigation to gather information about the oxidising strength of KMnO4. (i) 3 (ii) Provide a conclusion based on one set of observations from your first-hand investigation. 2 (i) Identify a pigment commonly used in an ancient culture, such as early Egyptian or Roman. 1 (ii) (b) Outline a risk assessment for this investigation, and show how this would influence the experimental procedure. The diagram shows the absorption spectrum of a pigment used in a painting found inside an ancient Egyptian tomb. 2 Absorbance 1.0 0.0 Violet Blue Green Orange 400 500 600 Red 700 800 Wavelength, nm Use the spectrum to identify the colour of this pigment. Justify your choice. (iii) (c) Explain why many minerals containing transition metal ions have been used as pigments. 3 Evaluate the contributions of Bohr, Pauli and Hund in developing our current understanding of the arrangement of electrons around the nuclei of atoms. 7 Question 32 continues on page 38 37 Marks Question 32 (continued) (d) (i) Name the block in the Periodic Table occupied by the transition metals. 1 (ii) Account for the observation that some transition metal complex ions can act as strong oxidising agents. 2 (iii) The formulae of a number of complex ions are shown. 4 [Cu(H2O)6]2+ [Fe(CN)6]4 [Co(NH3)4Cl2]+ [Ni(H2O)6]2+ [Fe(H2O)4Cl2]+ Identify a feature of all ligands that enables them to form bonds to metal ions, and explain the bonding in one of the above complex ions. Include a Lewis diagram in your answer. End of Question 32 38 Marks Question 33 Forensic Chemistry (25 marks) (a) During your practical work you performed a first-hand investigation using flame tests and/or spectroscope analysis to identify and describe the emission spectra of elements including sodium and mercury. (i) 3 (ii) (b) Outline a risk assessment for this investigation, and show how this would influence the experimental procedure. Provide a conclusion based on one set of observations from your first-hand investigation. 2 Carbohydrates are a general class of compounds that includes monosaccharides such as glucose, and polysaccharides such as glycogen and cellulose. (i) 1 (ii) Compare the composition of glycogen and cellulose, and where they occur in nature. 2 (iii) (c) What is the general formula of carbohydrates? Explain the differences in structure between glycogen and cellulose. 3 The diagram shows a crime scene where there has been a fire. No identification was found on the body. A small amount of residue was extracted from the tin for analysis. Describe TWO modern forensic chemistry techniques that could be used to examine evidence from this crime scene, and analyse why these techniques are suitable for forensic investigations. Question 33 continues on page 40 39 7 Marks Question 33 (continued) (d) The structure of the amino acid glycine is shown. H H N C C H A O H OH (i) Identify the functional group A. 1 (ii) Use structural formulae to write a balanced chemical equation to show the formation of a dipeptide containing two glycine molecules. 2 (iii) The amino acid sequences of two proteins are shown. 4 Protein A Cysteine Tyrosine Isoleucine Glutamine Asparagine Cysteine Proline Leucine Glycine Protein B Cysteine Tyrosine Phenylalanine Glutamine Asparagine Cysteine Proline Arginine Glycine Describe a chemical test for proteins, and explain how enzymes could be used to distinguish between Proteins A and B. End of paper 40 Board of Studies NSW 2006 2006 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 Ba 2+ Ca 2+ 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+ 2+ 2+ + 2e Sn 2+ + 2e Pb 2+ + 2e Zn Fe Ni + 2e Zn(s) 0.76 V + 2e Fe(s) 0.44 V Ni(s) 0.24 V Sn(s) 0.14 V Pb(s) 0.13 V 2 2+ Cu 1 H2(g) 2 + + 2e H2O + 2e Cu + e 1 I2(s) + e 2 1 I (aq) + e 2 2 3+ +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 + 4H + 2e 1 O2(g) + 2 + 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 1.08 V Br 1.10 V H2O 1.23 V 1.36 V Br 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. 41 42 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 28 Ni 58.69 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 29 Cu 63.55 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 27 Co 58.93 Name of element Osmium 76 Os 190.2 Ruthenium 44 Ru 101.1 Iron 26 Fe 55.85 Atomic Weight Symbol of element Californium 98 Cf [251.1] Dysprosium 66 Dy 162.5 Mercury 80 Hg 200.6 Cadmium 48 Cd 112.4 Zinc 30 Zn 65.41 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 Aluminium 13 Al 26.98 Boron 5 B 10.81 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 37 Rb 85.47 25 Mn 54.94 Potassium 24 Cr 52.00 20 Ca 40.08 19 K 39.10 23 V 50.94 Magnesium Sodium 22 Ti 47.87 12 Mg 24.31 11 Na 22.99 21 Sc 44.96 Beryllium Lithium Gold 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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