9701_s21_qp_42
A paper of Chemistry, 9701
Questions:
8
Year:
2021
Paper:
4
Variant:
2
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An aqueous solution of chromium(contains the green [Cr(H2O)6]3+ complex ion. Complete the electronic configuration of an isolated, gaseous Cr3+ ion. 1s2 ��������������������������������������������������������������������������������������������������������������������������������� Define the term complex ion. [Cr(H2O)6]3+shows some similar chemical properties to [Co(H2O)6]2+. Samples of [Cr(H2O)6]3+ are reacted separately with either NaOH, H2O2, or excess NH3. Use this information and the Data Booklet to suggest the formula of the chromium species formed. State the type of reaction taking place in each case. reagent added to [Cr(H2O)6]3+formula of chromium species formed type of reaction NaOHH2O2an excess of NH3 [Cr(H2O)6]2+ and [Cr2(O2CCH3)4(H2O)2] are both complexes of chromium(and have different colours. Explain why the colours of these complexes are different. The structure of [Cr2(O2CCH3)4(H2O)2] is shown. Ethanoate ions act as ligands in this complex. The ethanoate ligand, CH3CO2 –, is shown as O O. Cr O O O H2O O O O O OH2 O Cr Water and ethanoate ions behave as different types of ligand in this complex. Suggest an explanation for this statement. Deduce the coordination number of Cr and the geometry around each Cr atom in this structure. coordination number geometry around Cr atom ���������������������������������������������������������������������������������������������������  State the type of bond between the two atoms in the Cr–Cr bond. The [Cr2(O2CCH3)4(H2O)2] complex reacts with aqueous acid to form Cr2+ions. Cr2+ions react with O2under acidic conditions. Cr3+ions are formed. Use the Data Booklet to answer the following questions. Construct an ionic equation for the reaction of Cr2+with O2under acidic conditions. Calculate for the reaction in .  = V 
11. Group 17  →  11.3. Some reactions of the halide ions
11. Group 17  →  11.4. The reactions of chlorine
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State and explain the trend observed in the thermal stability of the Group2 nitrates. Lead(nitrate, Pb(NO3)2, decomposes on heating in a similar manner to the Group2 nitrates. Write an equation for the decomposition of lead(nitrate. Suggest how the ease of decomposition of Pb(NO3)2 would compare to that of Ba(NO3)2. Explain your answer. You may find it useful to refer to the Data Booklet. Bariumethanedioate, BaC2O4, decomposes on heating to produce bariumoxide and a mixture of two different gases. Construct an equation for the decomposition of barium ethanedioate. An impure sample of BaC2O4, of mass 0.500 g, is added to 50.0 cm3 of 0.0200 mol dm–3 acidified MnO4 –, an excess. A redox reaction takes place and all the BaC2O4 reacts. The resulting solution, containing unreacted acidified MnO4 –, is titrated with 0.0500 mol dm–3 Fe2+. The end-point is reached when 30.40 cm3 of 0.0500 mol dm–3 Fe2+has been added. C2O4 2– 2CO2 + 2e– MnO4 – + 8H+ + 5e– Mn2+ + 4H2O Fe2+ Fe3+ + e– Calculate the percentage by mass of BaC2O4 in the 0.500 g impure sample. Show your working. [Mr: BaC2O4, 225.3]  percentage by mass of BaC2O4 = Bariumhydroxide, Ba(OH)2, is completely dissociated in aqueous solution. Calculate the pH of 0.120 mol dm–3 Ba(OH)2at 298 K.  pH = 
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
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Define the term standard electrode potential. Three redox systems, A, B and C, are shown. The ligand 1,2-diaminoethane, H2NCH2CH2NH2, is represented by en. A [Ru(H2O)6]3+ + e– [Ru(H2O)6]2+ B [Ru(NH3)6]3+ + e– [Ru(NH3)6]2+ C [Ru3]3+ + e– [Ru3]2+ Two electrochemical cells are set up to compare the standard electrode potentials, E o, of three half-cells. The diagrams show the relative potential of each electrode. [Ru(NH3)6]3+ [Ru(NH3)6]2+ salt bridge V [Ru3]3+ [Ru3]2+ + – Pt Pt [Ru(H2O)6]3+ [Ru(H2O)6]2+ salt bridge V [Ru3]3+ [Ru3]2+ + – Pt Pt Use this information to complete the table by adding the labels A, B and C to deduce the order of E o for the three half-cells. E o redox system most negative least negative  The complex [Ru3]3+ shows stereoisomerism. The ligand en is bidentate. Draw three-dimensional diagrams to show the two isomers of [Ru3]3+. Represent the ligand en by using N N . Name the type of stereoisomerism. isomer 1 Ru isomer 2 Ru type of stereoisomerism  An electrochemical cell consists of a Br2/Br – half-cell and a Ag+/Ag half-cell, under standard conditions. Use the Data Booklet to calculate the . Deduce the direction of electron flow in the wire through the voltmeter between these two half-cells. = V direction of electron flow from to ����������������������������������������� Water is added to the Ag+/Ag half-cell in . Suggest the effect of this addition on the Ecell. Place a tick ( ) in the appropriate box. less positive no change more positive Explain your answer. Silver bromide, AgBr, dissolves in an aqueous solution of S2O3 2– ions to form the complex ion [Ag(S2O3)2]3–. The S2O3 2– ions act as monodentate ligands. equilibrium 1 AgBr+ 2S2O3 2–[Ag(S2O3)2]3–+ Br –Define the term ligand. Write an expression for the equilibrium constant, Kc, for equilibrium1. Kc =  Some additional data are given about the dissolution of AgBr in S2O3 2–. equilibrium constant numerical value solubility product, Ksp, of AgBr 5.4 × 10–13 stability constant, Kstab, of [Ag(S2O3)2]3– 2.9 × 1013 Use your answer to and these data to calculate Kc for equilibrium1. Include the units for Kc.  Kc = units The numerical values for the stability constants, Kstab, of two other silver(complexes are given. silver(complex numerical value of Kstab [Ag(CN)2]– 5.3 × 1018 [Ag(NH3)2]+ 1.6 × 107 An aqueous solution containing Ag+ is added to a solution containing equal concentrations of CN–, NH3and S2O3 2–. The mixture is left to reach equilibrium. Deduce the relative concentrations of [Ag(CN)2]–, [Ag(NH3)2]+ and [Ag(S2O3)2]3– present in the resulting mixture. Explain your answer. > > highest concentration lowest concentration 
11. Group 17  →  11.3. Some reactions of the halide ions
14. Hydrocarbons  →  14.2. Alkenes
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
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Define the term lattice energy. Use the following data to calculate a value for the enthalpy change of solution of copper(chloride, CuCl 2. You might find it helpful to construct an energy cycle. enthalpy change of hydration of Cl – = –378 kJ mol–1 enthalpy change of hydration of Cu2+ = –2099 kJ mol–1 lattice energy of CuCl 2= –2824 kJ mol–1  enthalpy change of solution of CuCl 2= kJ mol–1 The enthalpy change of hydration of Ca2+ is –1579 kJ mol–1. Use the Data Booklet to suggest why there is a big difference in the values of ∆Hhyd for Ca2+ and Cu2+. Identify the substances formed at the anode and at the cathode during the electrolysis of saturated CaCl 2. at the anode at the cathode  Calcium can be produced by the electrolysis of molten calciumchloride, CaCl 2. Calculate the mass, in g, of Ca formed when a current of 0.75 A passes through CaCl 2for 60minutes. [Ar: Ca, 40.1]  mass of Ca = g Explain what is meant by the term entropy of a system. Place one tick ( ) in each row of the table to show the sign of each entropy change, ∆S. process ∆S is negative ∆S is zero ∆S is positive NaCl dissolving in water water solidifying to ice  The evaporation of one mole of water has a standard Gibbs free energy change, ∆G o, of +8.6 kJ at 25 °C. Sketch a graph on the axes to show how ∆G o changes for this process between 25 °C and 150 °C at 101 kPa. positive negative 100 125 150 G o temperature / C  The reaction between A and B is feasible at low temperatures but is not feasible at high temperatures. A + B C + D Deduce the signs of ∆H and ∆S for this reaction and explain why the feasibility changes with temperature. sign of ∆H = sign of ∆S = 
5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)
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Describe and explain the relative basicities of phenylamine, ethylamine and 4-nitrophenylamine. > > most basic least basic The dye R can be synthesised from 4-nitrophenylamine in two steps. O2N O2N OH N N NH2 4-nitrophenylamine step 1 step 2 Q R Deduce and draw the structure of the organic salt Q in the box. Suggest reagents and conditions for step 1 and 2 in . step 1 step 2  Compound G can be synthesised from methylbenzene in three steps. E step 1 F G step 2 step 3 CH3 CO2H NO2 Br Give the systematic name of compound G. Deduce the identities of E and F and draw their structures in the boxes. Suggest reagents and conditions for each of steps 1 to 3 in . step 1 step 2 step 3  
21. Organic synthesis  →  21.1. Organic synthesis
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There are four possible structural isomers of C8H10 that contain a benzene ring. Draw the skeletal formulae of the four structural isomers in the appropriate boxes. The number of peaks observed in the carbon‑13 (13C) NMR spectrum of each compound is given. isomer 1 three peaks in 13C NMR isomer 2 four peaks in 13C NMR isomer 3 five peaks in 13C NMR isomer 4 six peaks in 13C NMR  A three-step synthesis of X (C10H10O) from benzene is suggested as shown. Cl (CH2)3CO2H Al Cl 3 Al Cl 3 step 1 step 2 step 3 W X (C10H10O) O Cl Step1 is the alkylation of benzene by electrophilic substitution. Use R–Cl to represent Cl (CH2)3CO2H. Write an equation for the formation of an electrophile from R–Cl and Al Cl 3. Deduce and draw the structures of W and X in the boxes. Suggest the reagents and conditions for step2. Complete the mechanism for the reaction of benzene with the electrophile formed in . Include all relevant charges and curly arrows showing the movement of electron pairs. Draw the structure of the intermediate. R intermediate  
14. Hydrocarbons  →  14.2. Alkenes
21. Organic synthesis  →  21.1. Organic synthesis
14. Hydrocarbons  →  14.1. Alkanes
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In aqueous solution, chlorinedioxide, Cl O2, reacts with hydroxide ions as shown. 2Cl O2 + 2OH– → Cl O3 – + Cl O2 – + H2O A series of experiments is carried out using different concentrations of Cl O2 and OH–. The table shows the results obtained. experiment [Cl O2] / mol dm–3 [OH–] / mol dm–3 initial rate / mol dm–3 min–1 0.020 0.030 7.20 × 10–4 0.020 0.120 2.88 × 10–3 0.050 0.030 4.50 × 10–3 Explain the term order of reaction. Use the data in the table to determine the order of reaction with respect to each reactant, Cl O2 and OH–. Explain your reasoning. Use your answer to to construct the rate equation for this reaction. rate = Use your rate equation and the data from experiment1 to calculate the rate constant, k, for this reaction. Include the units of k.  k = units The decomposition of benzenediazonium ions, C6H5N2 +, using a large excess of water, is a first‑order reaction. The graph shows the results obtained. 0.025 0.020 0.015 0.010 0.005 time / s [C6H5N2 +] / mol dm–3 Draw the structure of the organic product formed in this reaction.  Use the graph to determine the rate of reaction at 100 s. Show your working.  rate = mol dm–3 s–1 Sketch a concentration–time graph for a zero-order reaction. Use your graph to suggest how successive half-lives for a zero-order reaction vary as the concentration of a reactant decreases. Indicate this by placing a tick ( ) in the appropriate box in the table. concentration time successive half-lives decrease no change in successive half-lives successive half-lives increase  
8. Reaction kinetics  →  8.1. Rate of reaction
11. Group 17  →  11.4. The reactions of chlorine
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State and explain the relative rate of hydrolysis of acyl chlorides, alkyl chlorides and arylchlorides. > > fastest slowest The drug remifentanil is shown. O O remifentanil O O O N N Remifentanil is completely hydrolysed under acidic conditions. Three different organic compounds are formed. Draw the structures for these organic compounds in the boxes.  CompoundY, C5H10O2, reacts with Na2CO3to evolve bubbles of gas. The proton (1H) NMR spectrum of compoundY in D2O is shown. / ppm Use this information to suggest a structure for Y.  Use the Data Booklet, the proton (1H) NMR spectrum and your answer to to complete the table. chemical shift (δ) environment of proton splitting pattern number of 1H atoms responsible for the peak 0.95 1.90 2.20  
11. Group 17  →  11.3. Some reactions of the halide ions
15. Halogen compounds  →  15.1. Halogenoalkanes
14. Hydrocarbons  →  14.1. Alkanes
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