9701_w20_qp_42
A paper of Chemistry, 9701
Questions:
7
Year:
2020
Paper:
4
Variant:
2
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1
The rate of the reaction H2+ I22HIis studied. A small amount of H2is mixed with a large excess of I2at a temperature of 400 K and the reaction is monitored. The graph obtained is shown. relative concentration of H2time / seconds Suggest why a large excess of I2is used in this experiment. The reaction is first order with respect to H2. Use data from the graph to confirm this statement. Three separate experiments were carried out at 400 K with different starting concentrations of H2and I2. The results are shown in the table. experiment [H2] / mol dm–3 [I2] / mol dm–3 rate of reaction / mol dm–3 s–1 1.0 × 10–2 1.0 × 10–2 2.0 × 10–17 1.0 × 10–1 1.0 × 10–1 2.0 × 10–15 5.0 × 10–1 5.0 × 10–1 5.0 × 10–14 Use the data, and the order of reaction with respect to H2given in , to deduce the order of reaction with respect to I2. Explain your answer, giving data in support of your explanation. Use information from and your answer to to write the rate equation for the forward reaction. rate = Use your rate equation and data from experiment1 to calculate the value of the rate constant, k, for the forward reaction at 400 K. Include units for k.  k = units =  At 400 K the rate constant for the forward reaction is approximately 1000times greater than the rate constant for the backward reaction. The overall orders of the forward and backward reactions are the same. forward reaction H2+ I2→ 2HIbackward reaction 2HI→ H2+ I2Use this information to explain what will happen if equal concentrations of HI, H2and I2are mixed at 400 K. You should comment on: ● the relative initial rates of the forward and backward reactions ● the position of the equilibrium reached. At 700 K the rate constant for the forward reaction is approximately 50times greater than the rate constant for the backward reaction. Use this information and the information in to deduce the signs of the ∆H values of the forward and backward reactions. Explain your answer. 
8. Reaction kinetics  →  8.1. Rate of reaction
8. Reaction kinetics  →  8.2. Effect of temperature on reaction rates and the concept of activation energy
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Write an expression for the Ka of the weak acid HA in terms of the concentrations of the species involved. Ka =  The hydroxylammonium ion, HONH3 +, is a weak acid. A 1.00 × 10–3 mol dm–3 solution of hydroxylammonium ions has a pH of 4.41. Calculate the Ka of HONH3 +.  Ka = Calculate the pKa of HONH3 +.  pKa = The solubility product of manganese(hydroxide, Mn(OH)2, in water is 1.1×10–11 mol3 dm–9 at 298 K. Calculate the solubility of Mn(OH)2 in water at 298 K.  solubility = mol dm–3 
7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases
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The energy cycle shown can be used, along with suitable data, to calculate the enthalpy change of hydration of Ca2+. Each arrow indicates a transformation, W, X, Y and Z. Each transformation consists of one or more steps. Ca2++ 2Cl –Ca+ Cl 2CaCl 2CaCl 2W X Y Z The following data and data from the Data Booklet should be used. electron affinity of Cl = –349 kJ mol–1 enthalpy change of atomisation of Ca= +193 kJ mol–1 enthalpy change of formation of CaCl 2= –795 kJ mol–1 enthalpy change of solution of CaCl 2= –83 kJ mol–1 enthalpy change of hydration of Cl –= –364 kJ mol–1 Calculate the value of the enthalpy change corresponding to transformation W. Show your working.  enthalpy change W = kJ mol–1 Use your answer to and other data to calculate the value of the enthalpy change corresponding to transformation Z.  enthalpy change Z = kJ mol–1 Use your answer to to calculate the enthalpy change of hydration of Ca2+.  enthalpy change of hydration of Ca2+= kJ mol–1 Write an expression, in terms of W, X, Y and/or Z, to show how the enthalpy changes of two of the transformations can be used to calculate the lattice energy of CaCl 2. lattice energy of CaCl 2= State whether the lattice energy of CaCl 2is more or less exothermic than the lattice energy of MgF2. Explain your answer. The sulfates of the Group2 elements vary in solubility down Group2. Give the names of two solutions that could be mixed to form bariumsulfate. State and explain how the solubilities of the sulfates of the Group2 elements vary down Group2. 
5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)
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Identify the substances liberated at the anode and at the cathode during the electrolysis of saturated KCl . at the anode at the cathode  When dilute sulfuricacid is electrolysed, oxygen is liberated at the anode. Dilute sulfuricacid is electrolysed for 15.0minutes using a current of 0.750 A. Calculate the volume of oxygen that is liberated under room conditions.  volume of oxygen = cm3 The halogens chlorine, bromine and iodine differ in their strengths as oxidising agents. These strengths are indicated by the E o values for these halogens. Give the E o values for chlorine, bromine and iodine acting as oxidising agents. Deduce which of chlorine, bromine and iodine will react with a solution of Sn2+under standard conditions. Explain your answer. Include a relevant equation in your explanation. An excess of chlorine is added to a solution of acidified Mn2+under standard conditions. Give the formula of the product of this reaction that contains manganese. An electrochemical cell can be made by connecting an Fe3+ / Fe2+ half-cell to an S2O8 2– / SO4 2– half-cell under standard conditions. Calculate the standard cell potential of this electrochemical cell.  = V State the material that should be used as the electrode in each half-cell. in the Fe3+ / Fe2+ half-cell in the S2O8 2– / SO4 2– half-cell  Describe one change to each half‑cell that would increase the value of the cell potential. The temperature should remain at 298 K. Fe3+ / Fe2+ half-cell S2O8 2– / SO4 2– half-cell  
11. Group 17  →  11.4. The reactions of chlorine
11. Group 17  →  11.2. The chemical properties of the halogen elements and the hydrogen halides
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Define the term transition element. Complete the electronic configuration of an isolated gaseous Fe3+ ion. 1s2 Name two transition elements whose isolated gaseous atoms have the same number of electrons in the 3d subshell as an isolated gaseous Fe3+ ion. Cobalt(sulfate is added to water to form a pink solution containing complex ion P. An excess of concentrated hydrochloricacid is added to this solution to form a blue solution containing complex ion Q. Complete the diagram to show the three-dimensional structure of Q. State the charge on this complex ion. Co charge  Name the type of reaction in which P forms Q. Explain why solutions that contain transition element ions are often coloured. Explain why the colours of P and Q are different. A solution of the bidentate ligand 1,2‑diaminoethane, H2NCH2CH2NH2, is added to an aqueous solution of cobalt(sulfate. Oxygen is then bubbled into the mixture forming a complex ion with the formula [Co(H2NCH2CH2NH2)3]3+. This complex ion exists as a mixture of two isomers. The geometry of both of these isomeric complexes is octahedral. In this reaction, cobalt undergoes two types of reaction. One type of reaction is the same as that described in . Name the other type of reaction that cobalt undergoes. Draw the three-dimensional structures of the two isomeric complexes in the boxes. You may use N N to represent a molecule of H2NCH2CH2NH2. Co Co  Name the type of stereoisomerism shown by these two isomeric complexes. State the co-ordination number of cobalt in these two isomeric complexes. The stability constants, Kstab, of three complexes of mercury(are given in the table. complex Kstab [Hg(CN)4]2– 2.5 × 1041 [HgCl 4]2– 1.7 × 1016 [HgI4]2– 2.0 × 1030 Write an expression for the Kstab of [Hg(CN)4]2–. Kstab =  An aqueous solution containing Hg2+ is added to a solution containing equal concentrations of CN–, Cl –and I–. The mixture is left to reach equilibrium. Predict which of the complexes [Hg(CN)4]2–, [HgCl 4]2– and [HgI4]2– is present in the resulting mixture in the highest concentration and which is present in the lowest concentration. Explain your answer. 
3. Chemical bonding  →  3.4. Covalent bonding and coordinate (dative covalent) bonding
11. Group 17  →  11.3. Some reactions of the halide ions
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
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Ethanoic acid, CH3CO2H and trichloroethanoic acid, CCl 3CO2H, are both carboxylic acids. Ethanoicacid can be used to make ethanamide, CH3CONH2. Place these three compounds in order of acidity, starting with the least acidic. Explain your answer. least acidic most acidic  Methanoicacid, HCO2H, and ethanedioicacid, HO2CCO2H, are two other carboxylic acids. State which, if any, of ethanoicacid, methanoicacid and ethanedioicacid will react with Fehling’s reagent. State which, if any, of ethanoicacid, methanoicacid and ethanedioicacid will react with warm acidified manganate(ions. Ethanamide can be made from ethanoicacid in a two-step synthesis. step 1 step 2 ethanoic acid A ethanamide CompoundA contains chlorine. Give the structural formula and name of A. structural formula name  Suggest suitable reagents for steps 1 and 2. step 1 step 2  CompoundA can also be used to make the amide CH3CONHC2H5. The proton NMR spectrum of the amide CH3CONHC2H5 in the solvent CDCl 3 is shown. δ / ppm Explain why CDCl 3 is used as a solvent instead of CHCl 3. Complete the diagram with the chemical shifts, δ, of the protons labelled in the CH3CONHC2H5 molecule. C O C H2 C H3 C H3 N H = = = =  State and explain how the proton NMR spectrum of the amide CH3CONHC2H5 differs when dissolved in D2O rather than CDCl 3. The mass spectrum of the amide CH3CONHC2H5 includes a fragment ion with m/e value of 58. Give the molecular formula of this fragment ion.  fragment ion with m/e value of 58 is The amide undergoes the following reaction to produce diethylamine. reagent B CH3CONHC2H5 C2H5NHC2H5 diethylamine Identify reagentB. State the number of different absorptions in the carbon‑13 NMR spectrum of diethylamine. 
17. Carbonyl compounds  →  17.1. Aldehydes and ketones
18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids
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Describe the structure of a benzene molecule, C6H6. Your answer should include: ● the shape of the molecule ● the relative lengths of the C–C bonds ● bond angles ● the hybridisation of the carbon atoms ● the overlap between orbitals that produces each type of bond present. Benzene can be used as a starting material to produce phenylamine by a two-step synthesis. benzene nitrobenzene phenylamine NO2 NH2 step 1 step 2 Step1 is the reaction of benzene with NO2 + ions. Complete the mechanism and draw the intermediate of step1. Include all relevant charges and curly arrows to show the movement of electron pairs. intermediate nitrobenzene + H+ +NO2  State the name of the mechanism in . Identify the reagents needed to produce NO2 + ions. Write an equation to explain how these reagents produce NO2 + ions. Give reagents and conditions for the production of phenylamine from nitrobenzene in step2. Phenylamine reacts with Br2. Write an equation for this reaction. You may use structural or displayed formulae. Name the organic product of this reaction. Describe two observations that can be seen when phenylamine reacts with Br2. observation 1 observation 2  Describe the relative basicities of ammonia, ethylamine and phenylamine, starting with the least basic. Explain your answer in terms of their structures. least basic most basic  1,3‑diaminopropane, H2NCH2CH2CH2NH2, can be used to make polyamides. Identify one compound that would react with 1,3‑diaminopropane to form a polyamide. Draw a section of the polymer chain formed from 1,3‑diaminopropane and the compound you chose in . Your answer should: ● include four monomer residues (two of each type of monomer) ● show the amide link fully displayed ● clearly identify one repeat unit of this polymer.  
14. Hydrocarbons  →  14.2. Alkenes
21. Organic synthesis  →  21.1. Organic synthesis
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