# UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level

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1 UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level * * CEMISTRY 5070/41 Paper 4 Alternative to Practical October/November hour Candidates answer on the Question Paper. No Additional Materials are required. READ TESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use a soft pencil for any diagrams, graphs or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. Electronic calculators may be used. Write your answers in the spaces provided in the Question Paper. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question. This document consists of 15 printed pages and 1 blank page. DC (SJF/CGW) 58060/4 [Turn over

2 2 1 A student adds a known mass of magnesium ribbon to 100 cm 3 of dilute hydrochloric acid (an excess) in the apparatus shown below. ydrogen gas is evolved. The time taken to collect 48 cm 3 of gas at room temperature and pressure is measured. magnesium ribbon A dilute hydrochloric acid B (a) (i) Name apparatus A....[1] (ii) Name apparatus B....[1] (b) (i) Calculate the number of moles of hydrogen in the 48 cm 3 of gas. [1 mole of any gas occupies cm 3 at room temperature and pressure.]... moles [1] (ii) the equation below to deduce the mass of magnesium used in the experiment to produce 48 cm 3 of hydrogen at room temperature and pressure. [A r : Mg, 24] Mg + 2Cl MgCl (c) Give a test for hydrogen gas....g [1]...[1] 5070/41/O/N/13

3 3 (d) What is the effect on the time taken to collect the same volume of gas if, (i) large lumps of the same mass of magnesium are used instead of magnesium ribbon,...[1] (ii) the reaction is carried out at a higher temperature?...[1] [Total: 7] 5070/41/O/N/13 [Turn over

4 4 2 (a) A student investigates the electrolysis of aqueous copper(ii) sulfate using graphite electrodes and the apparatus shown below. + electrodes aqueous copper(ii) sulfate S R (i) What is observed at electrode R?...[1] (ii) Construct the equation for the reaction taking place at electrode R....[1] (iii) When graphite electrodes are used a colour change is seen in the solution. What is this colour change? Explain why it happens [2] (iv) When graphite electrodes are used, a gas is evolved at one of the electrodes. Name the gas and give a test for the gas. name... test... [2] (v) If the graphite electrodes are replaced with copper electrodes, no colour change is seen on electrolysis of the solution. Explain why [1] 5070/41/O/N/13

5 5 (b) The student does more experiments using the apparatus in (a) with graphite electrodes but, in each case, using a different electrolyte. Complete the table below. electrolyte product at the anode (+ electrode) observations at the anode (+ electrode) product at the cathode ( electrode) observations at the cathode ( electrode) (i) dilute sulfuric acid bubbles of colourless gas (ii) concentrated aqueous potassium iodide bubbles of colourless gas (iii) molten lead bromide silvery grey liquid [9] [Total: 16] 5070/41/O/N/13 [Turn over

6 6 In questions 3 to 7 inclusive place a tick ( ) in the box against the correct answer. 3 A compound contains 0.48 g of carbon, 0.08 g of hydrogen and 0.64 g of oxygen. [A r :, 1; C, 12; O, 16] What is the empirical formula of the compound? (a) CO (b) CO 2 (c) C 2 O (d) C 2 O 2 [Total: 1] 4 A student does a chromatography experiment to identify the components of Z, a sample of ink containing a mixture of coloured dyes. The chromatogram below contains a sample of Z as well as individual dyes, which are labelled 1, 2, 3 and 4. solvent front solvent flow X X X X X Z starting line Z contains (a) dyes 1 and 2. (b) dyes 1 and 3. (c) dyes 2 and 4. (d) dye 1 plus a dye which cannot be identified from the experiment. [Total: 1] 5070/41/O/N/13

7 7 5 Which two of the following compounds are isomers? C C C C C C C C C C A B C C C C C C C C C C D (a) A and B (b) B and C (c) C and D (d) A and C [Total: 1] 6 Which of the following mixtures produces an ester? (a) propanoic acid, potassium dichromate(vi), sulfuric acid (b) ethanol, potassium dichromate(vi), sulfuric acid (c) ethanol, propanoic acid, sulfuric acid (d) ethanol, propanol, sulfuric acid [Total: 1] 5070/41/O/N/13 [Turn over

8 8 7 A student sets up four test-tubes as shown in the diagram. E F G magnesium iron iron zinc aqueous copper(ii) sulfate aqueous magnesium sulfate aqueous copper(ii) sulfate aqueous magnesium sulfate In which of the test-tubes would a displacement reaction take place? (a) E only (b) E and F (c) E and G (d) F, G and [Total: 1] 5070/41/O/N/13

9 9 8 A student does an experiment to determine the numerical value of x in the compound KIO x. A sample of KIO x is placed in a previously weighed container and reweighed. mass of container + KIO x = 7.25 g mass of empty container = 6.44 g (a) Calculate the mass of KIO x used in the experiment....g [1] The student transfers the sample of KIO x to a beaker, adds about 100 cm 3 of distilled water and stirs the mixture until all the solid has dissolved. The contents of the beaker are then transferred to a 250 cm 3 volumetric flask. The solution is made up to 250 cm 3 with distilled water. This is solution J. A 25.0 cm 3 portion of J is transferred to a conical flask. A few grams of potassium iodide and 10 cm 3 of dilute hydrochloric acid are added to the conical flask. All the iodine in KIO x is converted into iodine molecules, I 2. A few drops of a suitable indicator are added. 1 mole of KIO x reacts with KI and produces 3 moles of iodine molecules, I 2. (b) What apparatus should be used to transfer 25.0 cm 3 of J to the conical flask?...[1] 5070/41/O/N/13 [Turn over

10 10 (c) mol/dm 3 aqueous sodium thiosulfate, Na 2 S 2 O 3, is put into a burette and run into the conical flask. Three titrations are done. The diagrams below show parts of the burette with the liquid levels at the beginning and end of each titration. first titration second titration third titration the diagrams to complete the results table. titration number final burette reading /cm 3 initial burette reading /cm 3 volume of mol/dm 3 sodium thiosulfate /cm 3 best titration results ( ) Summary Tick ( ) the best titration results. Using these results, the average volume of mol/dm 3 sodium thiosulfate, Na 2 S 2 O 3, is...cm 3. [4] (d) Calculate the number of moles in the average volume of mol/dm 3 sodium thiosulfate, Na 2 S 2 O moles [1] 5070/41/O/N/13

11 11 (e) 2 moles of Na 2 S 2 O 3 react with 1 mole of I 2. Calculate the number of moles of iodine, I 2, present in 25.0 cm 3 of the solution titrated.... moles [1] (f) 1 mole of KIO x produces 3 moles of I 2. Using your answer to (e) calculate the number of moles of KIO x in 25.0 cm 3 of solution J.... moles [1] (g) Using your answer to (f) calculate the number of moles of KIO x in 250 cm 3 of solution J.... moles [1] (h) Using your answers to (a) and (g) calculate the relative formula mass of KIO x. (i) Using your answer to (h) calculate the value of x in the formula KIO x. [A r : O, 16; K, 39; I, 127]...[1]...[1] [Total: 12] 5070/41/O/N/13 [Turn over

12 12 BLANK PAGE 5070/41/O/N/13

13 13 9 X is a metal carbonate which is insoluble in water. X reacts with dilute hydrochloric acid to form solution K and a gas. (a) (i) Name the gas and give a test for the gas. name... test... [2] (ii) Write the ionic equation for the reaction between a carbonate and an acid....[1] The following table shows the tests a student does on solution K. Complete the table by adding the conclusion for test (b), the observations for tests (c)(i), (c)(ii) and (d) and the test and observation for (e). test observations conclusion (b) K is divided into two parts for tests (c) and (d). K is a colourless solution. (c) (i) To the first part, aqueous sodium hydroxide is added. (ii) An excess of aqueous sodium hydroxide is added to the mixture from (c)(i). (d) To the second part, aqueous ammonia is added. K contains Ca 2+ ions. K contains Ca 2+ ions. (e) K contains Cl ions. [7] [Total: 10] 5070/41/O/N/13 [Turn over

14 14 10 When excess zinc powder is added to aqueous copper(ii) sulfate the temperature rises. (a) (i) What type of reaction does the temperature rise suggest?... [1] (ii) In addition to the temperature rise, suggest two observations that can be made as the reaction takes place [2] A student does an experiment to determine the heat produced in the reaction. Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s) The student adds 25.0 cm 3 of 1.0 mol / dm 3 aqueous copper(ii) sulfate to a glass beaker. The temperature of the solution is 20 C. Excess zinc powder is added to this solution and the temperature rises rapidly. After 1.0 minute the temperature of the solution is noted. Further temperature readings, taken at 1.0 minute intervals as the solution cools down, are shown in the table below. time /min temperature / C /41/O/N/13

15 15 (b) Plot the results on the grid. Draw a straight line through the points. Extend the line until it intersects the y-axis temperature / C time / min [3] 5070/41/O/N/13 [Turn over

16 (c) (i) (ii) 16 your graph to determine the temperature at 0 minutes. This gives the maximum temperature reached by the solution.... C [1] The initial temperature of the aqueous copper(ii) sulfate was 20 C. Using your answer to (c)(i) calculate the maximum temperature rise.... C [1] (iii) Calculate the number of moles of copper(ii) sulfate in 25.0 cm 3 of 1.0 mol / dm 3 aqueous copper(ii) sulfate.... moles [1] (d) Using your answers to (c)(ii) and (c)(iii) determine the heat produced in kj / mol. heat produced = maximum temperature rise 1000 moles of copper(ii) sulfate...kj / mol [1] [Total: 10] Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. 5070/41/O/N/13

17 UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level * * CEMISTRY 5070/42 Paper 4 Alternative to Practical October/November hour Candidates answer on the Question Paper. No Additional Materials are required. READ TESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use a soft pencil for any diagrams, graphs or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. Electronic calculators may be used. Write your answers in the spaces provided in the Question Paper. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question. This document consists of 14 printed pages and 2 blank pages. DC (CW/SW) 58061/4 [Turn over

18 2 1 Approximately 4 g of sodium hydroxide is added to 100 cm 3 of water. A thermometer is used to measure the temperature of the liquid both before and after the addition of sodium hydroxide. The diagrams below show parts of the thermometer stem giving the two temperatures T 1 (before) T 2 (after) (a) Complete the table and calculate the change in temperature. temperature T 2 after sodium hydroxide is added / C temperature T 1 before sodium hydroxide is added / C change in temperature / C [2] (b) (i) What type of process does this temperature change suggest has taken place?... [1] 5070/42/O/N/13

19 (ii) 3 Complete the energy profile diagram for sodium hydroxide dissolving in water. On your diagram label the products, the enthalpy change, Δ. NaO(s) + 2 O(l) energy progress of reaction [2] (c) (i) If aqueous litmus is added to aqueous sodium hydroxide, what colour is the resulting solution?... [1] (ii) ow can the p of aqueous sodium hydroxide be determined?...[1] (iii) Suggest a value for the p of aqueous sodium hydroxide.... [1] [Total: 8] 5070/42/O/N/13 [Turn over

20 4 2 The fertiliser ammonium nitrate is a source of nitrogen. It has the formula N 4 NO 3. It can be made by adding an acid to aqueous ammonia. (a) Name and give the formula of this acid. name... formula... [1] (b) Describe briefly how crystals of ammonium nitrate can be made from aqueous ammonium nitrate [3] (c) (i) Calculate the mass of nitrogen contained in 1000 g of ammonium nitrate. [A r :,1; N,14; O,16]...g [2] (ii) What volume would the mass of nitrogen calculated in (i) occupy in the gaseous state at room temperature and pressure? [One mole of a gas occupies 24 dm 3 at room temperature and pressure.]... dm 3 [1] (d) Name and give the formula of another ammonium salt which may be used as a fertiliser. name... formula... [1] (e) Give both the formula and a test for the ammonium ion. formula... test... observation...[3] [Total: 11] 5070/42/O/N/13

21 5 In questions 3 to 6 inclusive, place a tick ( ) in the box against the correct answer. 3 Which method can be used to obtain pure water from aqueous sodium chloride? (a) chromatography (b) distillation (c) evaporation (d) titration [Total: 1] 4 Which is the best apparatus for transferring 25.0 cm 3 of a liquid from one flask to another during a titration experiment? (a) beaker (b) burette (c) measuring cylinder (d) pipette [Total: 1] 5 A student does an experiment to decompose hydrogen peroxide. 2 2 O 2 (aq) 2 2 O(l) + O 2 (g) e repeats this experiment using solid manganese(iv) oxide as a catalyst. Which observation regarding the use of manganese(iv) oxide is correct? (a) The rate of decomposition of hydrogen peroxide increases. (b) The manganese(iv) oxide reacts with hydrogen peroxide. (c) The total volume of oxygen produced in the reaction increases. (d) The mass of manganese(iv) oxide decreases. [Total: 1] 5070/42/O/N/13 [Turn over

22 6 6 The presence of an alkene is confirmed by its reaction with aqueous bromine. 1 mole of alkene reacts with 1 mole of bromine, Br 2. In an experiment 8.4 g of an alkene reacts completely with 32 g of bromine. [A r :,1; C,12; Br, 80] The alkene is (a) C 2 4. (b) C 3 6. (c) C 4 8. (d) C [Total: 1] 5070/42/O/N/13

23 7 7 A student determines the percentage of iron in iron wire by titration with mol / dm 3 potassium manganate(vii), KMnO 4. (a) A piece of iron wire is added to a previously weighed container which is then reweighed. mass of container + iron wire = 8.59 g mass of container = 6.94 g Calculate the mass of iron wire used in the experiment.... g [1] (b) The iron wire is placed in a conical flask as shown in the diagram below. Dilute sulfuric acid is added to react completely with all the iron in the wire. The iron in the wire is oxidised to Fe 2+ ions. The valve allows the gas to escape but does not allow air into the flask. valve iron wire dilute sulfuric acid heat (i) Suggest why it is necessary to prevent air entering the apparatus....[1] (ii) Name and give a test for the gas produced during the reaction. name... test...[2] 5070/42/O/N/13 [Turn over

24 8 (c) When all the iron has reacted, the contents of the conical flask are transferred to a volumetric flask. The solution is made up to 250 cm 3 with distilled water. This is solution P cm 3 of P is transferred to a conical flask. A burette is filled with mol / dm 3 potassium manganate(vii) which is added to the conical flask. What is the colour of P (i) before the addition of aqueous potassium manganate(vii),... (ii) at the end-point?... [2] 5070/42/O/N/13

25 9 (d) The student does three titrations. The diagrams below show parts of the burette with the liquid levels at the beginning and end of each titration. 1st titration 2nd titration 3rd titration the diagrams to complete the results table. titration number final burette reading / cm 3 initial burette reading / cm 3 volume of mol / dm 3 potassium manganate(vii) added / cm 3 best titration results ( ) Summary: Tick ( ) the best titration results. Using these results, the average volume of mol / dm 3 potassium manganate(vii) is... cm 3. [4] 5070/42/O/N/13 [Turn over

26 10 (e) Calculate the number of moles of potassium manganate(vii) in the average volume of mol / dm 3 KMnO 4. (f) Five moles of Fe 2+ ions react with one mole of KMnO 4. Calculate the number of moles of Fe 2+ ions in 25.0 cm 3 of P.... moles [1] (g) Calculate the number of moles of Fe 2+ ions in 250 cm 3 of P.... moles [1] (h) Calculate the mass of iron in 250 cm 3 of P. [A r : Fe, 56]... moles [1]... g [1] (i) Using your answers to (a) and (h), calculate the percentage by mass of iron in the sample of iron wire....% [1] [Total: 15] 5070/42/O/N/13

27 11 8 V is a compound which contains two ions. Complete the table by adding the observations for tests (a), (b) and (c) and the test and observation for test (d). test observations conclusions (a) V is dissolved in water and the resulting solution divided into three parts for tests (a), (b) and (c). V is probably not a compound of a transition metal. (b) (i) (ii) To the first part, aqueous sodium hydroxide is added until a change is seen. An excess of aqueous sodium hydroxide is added to the mixture from (i). V may contain Al 3+ or Zn 2+ ions. (c) (i) (ii) To the second part, aqueous ammonia is added until a change is seen. An excess of aqueous ammonia is added to the mixture from (i). The presence of Al 3+ ions is confirmed. (d) V contains SO 4 2 ions. Conclusion: the formula of V is... [Total: 8] 5070/42/O/N/13 [Turn over

28 12 9 A constant current is passed through aqueous copper(ii) sulfate using inert electrodes as shown in the diagram below. Copper is deposited at one of the electrodes. + electrodes aqueous copper(ii) sulfate D E (a) Name a suitable material for the inert electrodes.... [1] (b) At which electrode is copper deposited?... [1] (c) What is seen at the other electrode?...[1] (d) (i) The electrode at which copper is deposited is removed at 10 minute intervals, washed, dried and weighed. The results are shown in the table below. Complete the table by calculating the total increase in mass after each 10 minute interval. time / min mass of cathode / g total increase in mass / g [1] 5070/42/O/N/13

29 13 (ii) 3.5 Plot these results on the grid below. Draw two intersecting straight lines through the points total increase in mass / g time / min [3] (iii) ow long does it take for 1.60 g of copper to be deposited?... min [1] (iv) ow long does it take for all the copper to be deposited?... min [1] 5070/42/O/N/13 [Turn over

30 14 (e) What is the colour of the electrolyte (i) at the start of the experiment,... [1] (ii) at the end of the experiment?... [1] (f) The experiment is repeated using aqueous copper(ii) sulfate of the same concentration as before but this time using copper electrodes. The same current is passed for the same length of time. Draw a line on your graph, labelled S, to show the result you would expect for this second experiment. [1] (g) State and explain the colour of the electrolyte at the end of the experiment [2] [Total: 14] 5070/42/O/N/13

31 15 BLANK PAGE 5070/42/O/N/13

32 16 BLANK PAGE Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. 5070/42/O/N/13

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