GCSE (9 1) Combined Science (Chemistry) A (Gateway Science) J250/09 Paper 9, C1 C3 and CS7 (PAGs C1 C5)
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1 Oxford Cambridge and RSA GCSE (9 1) Combined Science (Chemistry) A (Gateway Science) Paper 9, C1 C3 and CS7 (PAGs C1 C5) (Higher Tier) Year 11 Test Time allowed: 1 hour 10 minutes H You must have: a ruler (cm/mm) the Data Sheet for GCSE Combined Science A (Chemistry) You may use: a scientific or graphical calculator a pencil First name Last name Centre number Candidate number INSTRUCTIONS Use black ink. You may use an HB pencil for graphs and diagrams. Complete the boxes above with your name, centre number and candidate number. Answer all the questions. Write your answer to each question in the space provided. Additional paper may be used if required but you must clearly show your candidate number, centre number and question number(s). INFORMATION The total mark for this paper is 60. The marks for each question are shown in brackets [ ]. Quality of extended responses will be assessed in questions marked with an asterisk (*). This document consists of 16 pages. Any blank pages are indicated. DC (SC/SG) /2 OCR is an exempt Charity Turn over
2 2 SECTION A Answer all the questions. You should spend a maximum of 20 minutes on this section. 1 Which equation shows a physical change? A CaCO 3 (s) CaO(s) + CO 2 (g) B C(s) + O 2 (g) CO 2 (g) C MgO(s) + H 2 SO 4 (aq) MgSO 4 (aq) + H 2 O(l) D H 2 O(s) H 2 O(l) 2 What is the typical bond length in a molecule, in metres? A 10 6 B 10 8 C D A calcium ion has the formula Ca 2+. A phosphate ion has the formula PO 4 3. What is the formula of calcium phosphate? A CaPO 4 B Ca(PO 4 ) 3 C Ca 2 (PO 4 ) 3 D Ca 3 (PO 4 ) 2
3 3 4 The accurate relative atomic mass of silicon is What is this number to four significant figures? A B C D The mean mass of an atom of an element is g. The Avogadro constant is atoms/mol. What is the element? A B C D Carbon Fluorine Nitrogen Oxygen 6 What is the mass of 2 moles of aluminium nitrate, Al (NO 3 ) 3? A B C D 234 g 426 g 594 g 702 g Turn over
4 7 Calcium Iodide, CaI 2, is a solid at room temperature and pressure. Which type of forces or bonds are broken when calcium iodide changes state? 4 A B C D Covalent Intermolecular Ionic Metallic 8 The table shows bond energy. Bond Bond energy in kj/mol H H 436 O=O 498 O H 464 Hydrogen reacts with oxygen to make steam. 2H H + O=O 2 H O H What is the energy change, in kj/mol? A 442 B 486 C +442 D +486
5 9 Hydrochloric acid is a strong acid. 5 Some hydrochloric acid has a ph of 2. The acid is diluted by a factor of Estimate the ph of the diluted acid. A 3 B 4 C 5 D 6 10 An electric current is passed through an aqueous solution of copper sulfate, CuSO 4, using inert electrodes. Cathode ( ) Anode (+) A copper oxygen B copper sulfur C oxygen copper D sulfur copper Which row of the table shows the correct products at each electrode? Turn over
6 6 SECTION B Answer all the questions. 11 This question is about properties of carbon. (a) Ethylene glycol is a carbon compound used in antifreeze. The displayed formula of a molecule of ethylene glycol is shown below. H H H O C C O H H H Each line represents a covalent bond. (i) Calculate the relative molecular mass of ethylene glycol.... (ii) What is the empirical formula for ethylene glycol?... (b) Carbon atoms form four covalent bonds. (i) Explain what is meant by a covalent bond in terms of electrons.... [2] (ii) Why can a carbon atom form four covalent bonds?... (iii) An organic compound in the same family as ethylene glycol has the molecular formula C 3 H 8 O 2. Draw a displayed formula for this molecule.
7 (c) Diamond and graphite are crystalline forms of carbon. The table shows properties of diamond, graphite and aluminium. Substance Melting point / C 7 Electrical conductivity Diamond 3550 Poor Graphite 3652 Very good Aluminium 2467 Very good Explain the properties of the substances in the table. Use the data from the table and your knowledge of structure and bonding.... [6] Turn over
8 8 12 This question is about atoms and ions of elements in the periodic table. (a) Elements contain different isotopes. Define the term isotopes.... (b) Complete the table for an atom and an ion of two different elements. Element symbol Mass number Protons Neutrons Electrons Charge [3] (c) Sodium oxide is an ionic compound with the formula Na 2 O. Sodium oxide can be made by reacting sodium with oxygen. (i) In the reaction, electrons are transferred between sodium and oxygen atoms. Describe this transfer of electrons.... [2] (ii) Construct a dot and cross diagram for Na 2 O. Show outer electrons only and the charges on each ion. [2]
9 (iii) Construct a balanced equation for the reaction. 9 Add state symbols.... (...) +... (...)... (...) [3] (d) Magnesium reacts with nitrogen to form magnesium nitride, which is an ionic compound. Predict the charge on the nitride ion and suggest the formula of magnesium nitride. Use the periodic table to help you. Charge:... Formula:... [2] Turn over
10 10 13 A student wants to make magnesium chloride, MgCl 2. The student adds magnesium carbonate to hydrochloric acid, HCl. (a) The equation is shown below. MgCO 3 (s) + 2HCl (aq) MgCl 2 (aq) + CO 2 (g) + H 2 O(l) (i) Describe a test that would identify the gas that has formed.... [2] (ii) Calculate the masses of MgCO 3 and HCl that react to form mol of MgCl 2. Mass of MgCO 3 =... g Mass of HCl =... g [4]
11 11 (b) The student wanted to make sure that all of the HCl had reacted. The student added an excess of magnesium carbonate so that HCl is the limiting reagent. The student then purified the reaction mixture in two stages to make a dry sample of magnesium chloride. Explain how the student would obtain pure magnesium chloride from the reaction mixture in two stages. Include a labelled diagram for the first stage.... [5] Turn over
12 12 14 A student does some experiments with acids, alkalis and salts. (a) Experiment 1 The student measures the temperature of 30 cm 3 of 2.0 mol/dm 3 hydrochloric acid, HCl. The student adds 30 cm 3 of 2.0 mol/dm 3 sodium hydroxide, NaOH. The student measures an increase in temperature of 12 C. The equation for the reaction is shown below. HCl (aq) + NaOH(aq) NaCl (aq) + H 2 O(l) (i) Explain whether the reaction is exothermic or endothermic.... [2] (ii) Draw and label the reaction profile for the reaction. On your diagram: Include the formulae of the reactants and products Label the activation energy A Label the energy change E. Energy Progress of reaction [3]
13 (iii) 13 Calculate the mass of NaOH in 30 cm 3 of 2.0 mol/dm 3 NaOH. Answer =... g [3] (iv) The student repeats the experiment but mixes 60 cm 3 volumes of 2.0 mol/dm 3 hydrochloric acid and 60 cm 3 of 2.0 mol/dm 3 sodium hydroxide. The temperature increase is the same as in the first experiment. Suggest reasons for these observations.... [2] Turn over
14 (b) Experiment 2 14 The student add the solution of sodium chloride obtained from Experiment 1 to a beaker. The student set up the circuit below using inert electrodes. d.c. supply + Cathode Anode Sodium chloride solution The student observes gas bubbles at each electrode. She is confident that only one gas formed at the cathode She also concludes that two different gases could have formed at the anode. Predict the gases at the electrodes and explain the student s conclusions.... [4] END OF QUESTION PAPER
15 15 BLANK PAGE
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