9701_w21_qp_42
A paper of Chemistry, 9701
Questions:
10
Year:
2021
Paper:
4
Variant:
2
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1
Radium is a Group2 element. The predicted lattice energy, , of radium sulfide, RaS, is –2612 kJ mol–1. Define . Some data relating to radium and sulfur are listed. Select relevant data from this list for use in your answers to parts to . process value / kJ mol–1 enthalpy change for Ra→ Ra2++ 2e– +1619 first ionisation energy of sulfur +1000 second ionisation energy of sulfur +2260 first electron affinity of sulfur –200 second electron affinity of sulfur +532 enthalpy change for S8+ 2e– → S2–+555 lattice energy of RaS–2612 Write an equation for the process corresponding to the second electron affinity of sulfur. Include state symbols. Sulfur exists as S8 molecules in the solid state. Use the data in this question to calculate the enthalpy change for the reaction S8→8S.  enthalpy change = kJ mol–1 Calculate the standard enthalpy change of formation, , of radiumsulfide.  standard enthalpy change, = kJ mol–1 State the two major factors that affect the numerical magnitude of a lattice energy. For each factor you have identified in , state whether it tends to make the lattice energy of radiumsulfide more or less exothermic than that of sodiumchloride. Explain your answer. The lattice energies of sodiumchloride, NaCl, and radiumsulfide, RaS, are –771 kJ mol–1 and –2612 kJ mol–1, respectively. Identify the dominant factor in determining the relative numerical magnitudes of the lattice energies of radiumsulfide and sodiumchloride. Explain your answer.
1. Atomic structure  →  1.4. Ionisation energy
5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)
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Ethoxyethane, C2H5OC2H5, can dissolve both in water and in octan-1-ol. The expression and numerical value for the partition coefficient of ethoxyethane between water and octan-1-ol are given. Water and octan-1-ol are immiscible. Kpc = concentration of C2H5OC2H5 in octan-1-ol = 6.760 at 20 °C concentration of C2H5OC2H5 in water In an experiment, octan-1-ol at 20 °C is added to a solution of ethoxyethane in water at 20 °C. The mixture is analysed immediately and a value of Kpc is calculated. The calculation is performed correctly; the value calculated is 5.625. Explain why the value calculated is less than 6.760. A second experiment is performed and the value of Kpc is found to be 6.760. The concentration of ethoxyethane in the octan-1-ol layer is 7.62 g dm–3. Calculate the concentration, in g dm–3, of ethoxyethane in the aqueous layer.  g dm–3 100 cm3 of the octan-1-ol layer is taken and shaken with 100 cm3 of water. Calculate the maximum amount, in mol, of ethoxyethane that can be extracted into the water.  mol An aqueous solution of lead(nitrate is mixed with an aqueous solution of sodiumiodide. A yellow precipitate of lead(iodide is formed and is filtered out, leaving solutionX. The concentration of Pb2+ in solutionX is 5.68 × 10–3 mol dm–3. The concentration of I– in solutionX is 4.20 × 10–4 mol dm–3. Use these data to calculate a value for the solubility product, Ksp, of lead(iodide. State the units of Ksp.  Ksp =  units =  Potassiumiodide is very soluble in water. Describe and explain what is seen if a few drops of saturated potassiumiodide solution are added to a portion of solutionX.
7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases
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Pure water is a very poor conductor of electricity. However, when hydrogenchloride gas is dissolved in water, ions are formed and a current flows during electrolysis. HCl + aq → H++ Cl –The overall change after electrolysis is that hydrogenchloride gas is converted into hydrogen and chlorine. 2HCl → H2+ Cl 2When a current of 3.10 A is passed through the solution for Y minutes, 351 cm3 of chlorine are produced at the anode, measured under room conditions. Calculate the number of chlorine molecules produced during the electrolysis.  number of chlorine molecules = Calculate the total number of electrons transferred to produce this number of chlorine molecules.  total number of electrons = Calculate the quantity of charge, in coulombs, of the total number of electrons calculated in .  quantity of charge = C Calculate the time, Y, in minutes, for which the current flows.  Y = minutes The standard entropies, S o, of three species are given in the table. species S o / J K–1 mol–1 HCl +187 H2+131 Cl 2+223 Calculate ∆S o for the reaction 2HCl → H2+ Cl 2. ∆S o = J K–1 mol–1 ∆H o for the reaction 2HCl → H2+ Cl 2is +185 kJ mol–1. Calculate ∆G o for this reaction at 298 K. ∆G o = kJ mol–1 Predict the effect of increasing temperature on the spontaneity of this reaction. Explain your answer.
11. Group 17  →  11.4. The reactions of chlorine
9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3
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Separate samples of 0.01 mol of magnesiumnitrate and 0.01 mol of strontiumnitrate are heated until completely decomposed to the metal oxide, nitrogendioxide and oxygen. State which of these two Group2 nitrates requires the higher temperature before it begins to decompose. Explain your answer. After decomposition is complete the 0.01 mol sample of magnesium oxide is taken and increasing amounts of water are added to it, with stirring, until no solid remains. This procedure is repeated with the 0.01 mol sample of strontiumoxide. Identify the sample to which most water must be added to cause all the solid to dissolve. Explain your answer by reference to the solubilities of the products formed when water is added to the oxides. You should refer to relevant energy terms in your answer. The nitrogen dioxide given off by the decomposition of 0.0100 mol of strontium nitrate is dissolved in water. The oxidising agent H2O2is then added to give 150.0 cm3 of a solution in which nitricacid, HNO3, is the only nitrogen-containing product. Calculate the concentration, in mol dm–3, of HNO3 in the 150.0 cm3 of solution.  concentration = mol dm–3 The HNO3 present in 25.0 cm3 of this solution is neutralised using 0.125 mol dm–3 NaOH. Calculate the minimum volume, in cm3, of NaOHneeded. Give your answer to three significant figures.  volume = cm3
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
2. Atoms, molecules and stoichiometry  →  2.4. Reacting masses and volumes (of solutions and gases)
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Transition elements form complexes. Molybdenum, Mo, forms an octahedral complex consisting of one Mo atom surrounded by carbon monoxide, CO, molecules. CO is a monodentate ligand. Iron forms an octahedral complex consisting of one Fe3+ and a number of cyanide, CN–, ions. CN– is a monodentate ligand. Define the term monodentate ligand. Complete the table by stating the formulae and charges of the complexes described. formula charge molybdenum complex iron(complex  Draw a three-dimensional diagram to show the shape of this iron(complex. Label one 180° bond angle on your diagram. Fe  An excess of aqueous ammonia is added to dilute copper(sulfate solution. A dark blue complex, [Cu(NH3)4(H2O)2]2+, is formed. Write an ionic equation for this reaction. Explain the origin of colour in copper(complexes. An excess of concentrated hydrochloric acid is added to the dark blue solution of [Cu(NH3)4(H2O)2]2+. A new complex, Z, is formed. The colour of the solution changes. Write an equation for the formation of Z from the solution of [Cu(NH3)4(H2O)2]2+. Include the formula and charge of Z. Name the type of reaction when Z forms from [Cu(NH3)4(H2O)2]2+. State the geometry of Z. State the colour of a solution of Z. Explain why the colour of a solution of [Cu(NH3)4(H2O)2]2+ is different from the colour of a solution of Z. You should refer to the energies of the orbitals involved in your answer. 
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
11. Group 17  →  11.3. Some reactions of the halide ions
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An excess of aqueous ammonia is added to a solution containing the complex ion [Co(H2O)6]2+. [Co(H2O)6]2+ + 6NH3 [Co(NH3)6]2+ + 6H2O Complete the sentence to describe the colour change that will be seen during this reaction. The colour changes from to ���������������������������������������������� . Write an expression for the stability constant, Kstab, of [Co(NH3)6]2+. Kstab =  The numerical value of Kstab of [Co(NH3)6]2+ is 7.7×104. What deduction about the properties of [Co(NH3)6]2+ and [Co(H2O)6]2+ can be made from this Kstab value? Oxygen can oxidise [Co(NH3)6]2+ to [Co(NH3)6]3+ under standard conditions in alkaline solutions. [Co(NH3)6]3+ + e– [Co(NH3)6]2+ E o = +0.10 V Use this information and the Data Booklet to calculate the value for this oxidation of [Co(NH3)6]2+.  = V  Write an ionic equation for this oxidation of [Co(NH3)6]2+. Predict, by selecting suitable data from the Data Booklet, whether oxygen can oxidise Co2+in acidic solution, in the absence of ammonia. Explain your answer. 
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
17. Carbonyl compounds  →  17.1. Aldehydes and ketones
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The structure of benzene-1,3-dicarboxylic acid is shown. HO OH O O benzene-1,3-dicarboxylic acid State the empirical formula of benzene-1,3-dicarboxylic acid. Benzene-1,3-dicarboxylic acid is an isomer of benzene-1,4-dicarboxylic acid. These two isomers can be distinguished by carbon-13 (13C) NMR spectroscopy. State the number of peaks in the carbon-13 (13C) NMR spectrum of each compound. benzene-1,3-dicarboxylic acid benzene-1,4-dicarboxylic acid  Benzene-1,3-dicarboxylic acid can be made by the two-step synthesis shown below. HO OH O O benzene-1,3-dicarboxylic acid HO O compound P step 2 step 1 compound Q C9H8O3 Name compound P. Explain why the major product of this two-step synthesis is benzene-1,3-dicarboxylicacid and not benzene-1,4-dicarboxylic acid. The reagents used for step 1 are CH3COCl and Al Cl 3. These reagents give rise to CH3C=O + ions which react with compoundP. Name the mechanism of this reaction. Draw the mechanism of the reaction of CH3C=O + ions with compound P. Include all relevant curly arrows and charges, the structure of the intermediate and the structure of compoundQ. HO O CH3C=O + intermediate compound Q  Suggest a reagent and conditions to convert compoundQ into benzene‑1,3‑dicarboxylic acid, in step2. 
21. Organic synthesis  →  21.1. Organic synthesis
18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids
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Alanine, H2NCH(CH3)CO2H, and glutamic acid, H2NCH(CH2CH2CO2H)CO2H, are two naturally occurring amino acids. H2NCH(CH3)CO2H exists as two optical isomers. Draw three-dimensional structures of these two optical isomers.  The proton (1H) NMR spectrum of either alanine in D2O or glutamic acid in D2O is shown. / ppm State whether this is the spectrum of alanine in D2O or the spectrum of glutamicacid in D2O. Explain your answer by reference to the number of peaks and splitting patterns. The mass spectrum of glutamicacid, H2NCH(CH2CH2CO2H)CO2H, is obtained. State the m/e value of the molecular ion peak in this spectrum. The spectrum has peaks with m/e values of 88 and 131. Draw the structures of the ions responsible for these peaks. m/e structure of ion  At pH 11 alanine exists as H2NCH(CH3)CO2 – ions and glutamic acid exists as H2NCH(CH2CH2CO2 –)CO2 – ions. A mixture of alanine and glutamicacid at pH 11 is subjected to electrophoresis. State how the mixture can be maintained at pH11 during electrophoresis. Draw a fully labelled diagram for the apparatus that would be used to carry out this electrophoresis. Your diagram should include the position of the mixture of alanine and glutamic acid at the start of the electrophoresis experiment. Identify the electrode that each amino acid travels towards during electrophoresis at pH11. alanine glutamic acid  In a particular electrophoresis experiment at pH 11, the glutamic acid travels 3.4 cm. Alanine travels a shorter distance. Explain the factors that account for the difference in the distances travelled. 
22. Analytical techniques  →  22.2. Mass spectrometry
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Butylamine, CH3CH2CH2CH2NH2, can be synthesised from different organic compounds by using suitable reagents. Each reaction involves one step. Complete the table to describe three different syntheses. ●One of the three syntheses should involve a nucleophilic substitution reaction. ●The starting organic compound for each synthesis should contain a different functional group. ●A different reagent should be used for each synthesis. starting organic compound reagent and conditions  Compare and explain the relative basicities of ammonia, butylamine and phenylamine. > > most basic least basic
21. Organic synthesis  →  21.1. Organic synthesis
17. Carbonyl compounds  →  17.1. Aldehydes and ketones
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