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AQA AS Level CHEMISTRY 7404-1 Paper 1 Inorganic and Physical Chemistry Question Paper June 2021

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AQA AS Level CHEMISTRY 7404/1 Paper 1 Inorganic and Physical Chemistry Question Paper June 2021 / AQA AS Level CHEMISTRY 7404-1 Paper 1 Inorganic and Physical Chemistry Question Paper June 2021 / AQA ... AS Level CHEMISTRY Paper 1 Inorganic and Physical Chemistry Question Paper June 2021 *JUN217404101* IB/M/Jun21/E7 7404/1 For Examiner’s Use Question Mark 1 2 3 4 5 6 7 8 9 10 Section B TOTAL Time allowed: 1 hour 30 minutes Materials For this paper you must have: •the Periodic Table/Data Sheet, provided as an insert (enclosed) •a ruler with millimetre measurements •a scientific calculator, which you are expected to use where appropriate. Instructions •Use black ink or black ball-point pen. •Fill in the boxes at the top of this page. •Answer all questions. •You must answer the questions in the spaces provided. Do not write outside the box around each page or on blank pages. •If you need extra space for your answer(s), use the lined pages at the end of this book. Write the question number against your answer(s). •All working must be shown. •Do all rough work in this book. Cross through any work you do not want to be marked. Information •The marks for questions are shown in brackets. •The maximum mark for this paper is 80. Advice You are advised to spend about 65 minutes on Section A and 25 minutes on Section B. Please write clearly in block capitals. Centre number Candidate number Surname Forename(s) Candidate signature I declare this is my own work. AS CHEMISTRY Paper 1 Inorganic and Physical Chemistry 2 *02* IB/M/Jun21/7404/1 Do not write outside the box Section A Answer all questions in this section. 0 1 This question is about atomic structure. 0 1 . 1 Figure 1 is a model proposed by Rutherford to show the structure of an atom. Figure 1 State two features of the current model that are not shown in the Rutherford model. [2 marks] Feature 1 of the current model Feature 2 of the current model 3 *03* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 0 1 . 2 A sample of tin is analysed in a time of flight mass spectrometer. The sample is ionised by electron impact to form 1+ ions. Table 1 shows data about the four peaks in this spectrum. Table 1 m/z Percentage abundance 112 22.41 114 11.78 117 34.97 120 To be determined Give the symbol, including mass number, of the ion that reaches the detector first. Calculate the relative atomic mass of tin in this sample. Give your answer to 1 decimal place. [4 marks] Symbol of ion Relative atomic mass 6 4 *04* IB/M/Jun21/7404/1 Do not write outside the box 0 2 This question is about magnesium and its compounds. 0 2 . 1 State one observation when magnesium reacts with steam. Give an equation, including state symbols, for this reaction. [2 marks] Observation Equation 0 2 . 2 Describe the bonding in magnesium. [2 marks] 0 2 . 3 Explain, in terms of structure and bonding, why magnesium chloride has a high melting point. [3 marks] 0 2 . 4 Give one medical use for magnesium hydroxide. [1 mark] 8 5 *05* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 0 3 This question is about redox reactions. 0 3 . 1 State, in terms of electrons, the meaning of the term oxidising agent. [1 mark] 0 3 . 2 Cr2O72– can oxidise SO32– in acidic conditions to form Cr3+ and SO42– Deduce a half-equation for the oxidation of SO32– to SO42– Deduce a half-equation for the reduction of Cr2O72– to Cr3+ Deduce the overall equation for the oxidation of SO32– by Cr2O72– [3 marks] Half-equation for the oxidation of SO32– to SO42– Half-equation for the reduction of Cr2O72– to Cr3+ Overall equation Turn over for the next question 4 6 *06* IB/M/Jun21/7404/1 Do not write outside the box 0 4 This question is about the identification of ions in unknown solutions. A student completes a number of test-tube reactions on solutions A, B and C. Table 2 shows the student’s observations. Table 2 Test 1 Test 2 Test 3 Add H2SO4(aq) Warm with NaOH(aq) Add acidified AgNO3(aq) A white precipitate no visible change no visible change B effervescence a gas is formed that turns damp red litmus blue effervescence C no visible change no visible change off-white precipitate 0 4 . 1 Suggest the identity of the positive ion in solution A. Give the simplest ionic equation for the formation of the white precipitate in Test 1 for solution A. [2 marks] Identity of positive ion in A Ionic equation 0 4 . 2 Different gases are formed when solution B reacts in Test 1 and in Test 2. Suggest the identity of each gas. Give the simplest ionic equation for the formation of the gas in Test 2. [2 marks] Gas formed in Test 1 Gas formed in Test 2 Ionic equation for the formation of the gas in Test 2 7 *07* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 0 4 . 3 The student thinks that solution C contains either chloride ions or bromide ions. Describe a further test, or tests, to show whether solution C contains chloride or bromide ions. [3 marks] Turn over for the next question 7 8 *08* IB/M/Jun21/7404/1 Do not write outside the box 0 5 This question is about chlorine. 0 5 . 1 Chlorine has a low boiling point because the forces between the molecules are weak. Explain how these forces arise between molecules of chlorine. [3 marks] 0 5 . 2 Give an equation for the reaction of chlorine with water. Give a reason why chlorine is added to drinking water. [2 marks] Equation Reason 0 5 . 3 Chlorine reacts with cold, aqueous sodium hydroxide in the manufacture of bleach. Give an equation for this reaction. [1 mark] 6 9 *09* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 0 6 Calcium sulfide reacts with calcium sulfate as shown. CaS + 3 CaSO4 → 4 CaO + 4 SO2 2.50 g of calcium sulfide are heated with 9.85 g of calcium sulfate until there is no further reaction. Show that calcium sulfate is the limiting reagent in this reaction. Calculate the mass, in g, of sulfur dioxide formed. Mr (CaS) = 72.2 Mr (CaSO4) = 136.2 [5 marks] Mass of sulfur dioxide g Turn over for the next question 5 10 *10* IB/M/Jun21/7404/1 Do not write outside the box 0 7 This question is about combustion. 0 7 . 1 State the meaning of the term standard enthalpy of combustion. [2 marks] 0 7 . 2 A student does an experiment to determine the enthalpy of combustion of propan-1-ol (CH3CH2CH2OH, Mr = 60.0). Combustion of 0.497 g of propan-1-ol increases the temperature of 150 g of water from 21.2 °C to 35.1 °C Calculate a value, in kJ mol–1, for the enthalpy of combustion of propan-1-ol in this experiment. The specific heat capacity of water is 4.18 J K–1 g–1 [3 marks] Enthalpy of combustion kJ mol‒1 11 *11* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 0 7 . 3 The enthalpy of combustion determined experimentally is less exothermic than that calculated using enthalpies of formation. Give one possible reason for this, other than heat loss. [1 mark] Turn over for the next question 6 12 *12* IB/M/Jun21/7404/1 Do not write outside the box 0 8 A student is provided with a 5.60 g sample of ethanoic acid (CH3COOH) contaminated with sodium ethanoate (CH3COONa). The student dissolves the sample in deionised water and makes the volume up to 200 cm3 The student removes 25.0 cm3 samples of the solution and titrates them with 0.350 mol dm–3 sodium hydroxide solution. Table 3 shows the results of these titrations. Table 3 Rough 1 2 3 Final volume / cm3 20.85 41.10 20.50 40.80 Initial volume / cm3 0.00 20.85 0.00 20.50 Titre / cm3 20.85 20.25 20.50 20.30 0 8 . 1 Use the results in Table 3 to calculate the mean titre value. Use the mean titre to calculate the percentage by mass of sodium ethanoate in the original sample. [6 marks] Mean titre value cm3 13 *13* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box Percentage by mass 0 8 . 2 The student rinses the burette with deionised water before filling with sodium hydroxide solution. State and explain the effect, if any, that this rinsing will have on the value of the titre. [2 marks] Turn over for the next question 8 14 *14* IB/M/Jun21/7404/1 Do not write outside the box 0 9 Hydrogen can be prepared on an industrial scale using the reversible reaction between methane and steam. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) ΔH = +206 kJ mol−1 The reaction is done at a temperature of 800 °C and a low pressure of 300 kPa in the presence of a nickel catalyst. Explain, in terms of equilibrium yield and cost, why these conditions are used. [6 marks] 15 *15* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 6 16 *16* IB/M/Jun21/7404/1 Do not write outside the box 1 0 Sulfur dioxide reacts with oxygen to form sulfur trioxide. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) ΔH = –196 kJ mol−1 1 0 . 1 Give an expression for the equilibrium constant (Kc) for this reaction. [1 mark] Kc 1 0 . 2 A mixture of sulfur dioxide and oxygen is allowed to reach equilibrium in a container of volume 1800 cm3 at temperature T. At equilibrium, the mixture contains 0.176 mol of sulfur dioxide and 0.461 mol of sulfur trioxide. At temperature T the equilibrium constant, Kc = 15.0 mol–1 dm3 Calculate the amount, in moles, of oxygen at equilibrium. [3 marks] Amount of oxygen mol 17 *17* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 1 0 . 3 At a different temperature, a mixture contains 0.025 mol of sulfur dioxide 0.049 mol of oxygen 0.034 mol of sulfur trioxide. The total pressure of the mixture in a 3500 cm3 reaction vessel is 255 kPa Use the data to calculate the temperature, in °C, of the mixture. The ideal gas constant, R = 8.31 J K−1 mol−1 [5 marks] Temperature °C Turn over for Section B 9 18 *18* IB/M/Jun21/7404/1 Do not write outside the box Section B Answer all questions in this section. Only one answer per question is allowed. For each answer completely fill in the circle alongside the appropriate answer. CORRECT METHOD WRONG METHODS If you want to change your answer you must cross out your original answer as shown. If you wish to return to an answer previously crossed out, ring the answer you now wish to select as shown. You may do your working in the blank space around each question but this will not be marked. Do not use additional sheets for this working. 1 1 In a time of flight mass spectrometer, molecule X is ionised using electrospray ionisation. What is the equation for this ionisation? [1 mark] A X(l) + e– → X+(g) + 2 e– B X(g) + e– → X+(g) + 2 e– C X(l) + H+ → XH+(g) D X(g) + H+ → XH+(g) 1 2 What is the electron configuration of V2+ in the ground state? [1 mark] A 1s2 2s2 2p6 3s2 3p6 3d3 B 1s2 2s2 2p6 3s2 3p6 3d1 4s2 C 1s2 2s2 2p6 3s2 3p6 3d3 4s2 D 1s2 2s2 2p6 3s2 3p6 3d5 4s2 19 *19* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 1 3 Which molecule is not able to form a co-ordinate bond with another species? [1 mark] A BH3 B CH4 C NH3 D H2O 1 4 Which species has a square planar shape? [1 mark] A NH4+ B SF4 C XeF4 D PCl4+ 1 5 Which bond has the most unsymmetrical electron distribution? [1 mark] A H–O B H–S C H–N D H–P Turn over for the next question 20 *20* IB/M/Jun21/7404/1 Do not write outside the box 1 6 Which compound contains a chlorine atom with an oxidation state of +4? [1 mark] A KClO4 B CCl4 C ClO2 D ClO2F 1 7 Which element is classified as a d block element? [1 mark] A Antimony B Molybdenum C Strontium D Uranium 1 8 Which element in Period 3 has the highest melting point? [1 mark] A Aluminium B Silicon C Sodium D Sulfur 21 *21* Turn over ► IB/M/Jun21/7404/1 Do not write outside the box 1 9 Which pair of solutions, when mixed, reacts to form a dark brown solution? [1 mark] A NaF(aq) + Cl2(aq) B NaCl(aq) + Br2(aq) C NaBr(aq) + Cl2(aq) D NaI(aq) + Br2(aq) 2 0 Some solid sodium halides are reacted with concentrated sulfuric acid. Which solid sodium halide does not produce a sulfur-containing gas as one of the products? [1 mark] A NaCl B NaBr C NaI D NaAt Turn over for the next question 22 *22* IB/M/Jun21/7404/1 Do not write outside the box 2 1 Which atom has one more proton and two more neutrons than P1531 ? [1 mark] A P1633 B P1634 C S1633 D S1634 2 2 What is a use for barium sulfate? [1 mark] A In agriculture to act as a fertiliser B In agriculture to neutralise acidic soil C In medicine to produce an X-ray image D In medicine as an antacid to treat indigestion 2 3 Which ion has the largest radius? [1 mark] A F– B Mg2+ C Na+ D O2– 23 *23* IB/M/Jun21/7404/1 Do not write outside the box 2 4 Which element has a first ionisation energy lower than that of sulfur? [1 mark] A Chlorine B Oxygen C Phosphorus D Selenium 2 5 The first seven successive ionisation energies for element Z are shown. What is element Z? [1 mark] A Carbon B Nitrogen C Silicon D Phosphorus END OF QUESTIONS 15 24 *24* IB/M/Jun21/7404/1 Do not write outside the box There are no questions printed on this page DO NOT WRITE ON THIS PAGE ANSWER IN THE SPACES PROVIDED 25 *25* IB/M/Jun21/7404/1 Do not write outside the box Question number Additional page, if required. Write the question numbers in the left-hand margin. 26 *26* IB/M/Jun21/7404/1 Do not write outside the box Question number Additional page, if required. Write the question numbers in the left-hand margin. 27 *27* IB/M/Jun21/7404/1 Do not write outside the box Question number Additional page, if required. Write the question numbers in the left-hand margin. 28 *28* IB/M/Jun21/7404/1 Do not write outside the box There are no questions printed on this page DO NOT WRITE ON THIS PAGE ANSWER IN THE SPACES PROVIDED Copyright information For confidentiality purposes, all acknowledgements of third-party copyright material are published in a separate booklet. This booklet is published after each live examination series and is available for free download from www.aqa.org.uk. Permission to reproduce all copyright material has been applied for. In some cases, efforts to contact copyright-holders may have been unsuccessful and AQA will be happy to rectify any omissions of acknowledgements. If you have any queries please contact the Copyright Team. Copyright © 2021 AQA and its licensors. All rights reserved. *216A7404/1* [Show More]

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