科目：化学 Chemistry (9701)
年份：2022 夏季
试卷：Paper 41
总页数：20
章节：19 Lattice energy, 20 Electrochemistry, 21 Further aspects of equilibria, 22 Reaction kinetics, 23 Entropy and Gibbs free energy, 24 Transition elements, 25 Benzene and its compounds, 26 Carboxylic acids and their derivatives, 27 Organic nitrogen compounds, 28 Polymerisation, 30 Analytical chemistry
Answer all the questions in the spaces provided.
1. (a) The solubility of the Group 2 sulfates decreases down the group.
Explain this trend.
[3]
(b) Describe what is observed when magnesium and barium are reacted separately with an excess of dilute sulfuric acid.
magnesium .....
barium ..... [1]
(c) The solubility product, $K_{\text{sp}}$, of $\text{BaSO}_4$ is $1.08 \times 10^{-10} \text{mol}^2\text{dm}^{-6}$ at 298 K.
Calculate the solubility of $\text{BaSO}_4$ in g per $100\text{cm}^3$ of solution.
solubility of $\text{BaSO}__4 = \dots\dots\dots\dots\g per 100\text{cm}^3$of solution [2](d) (i) The equation for the formation of a gaseous sulfate ion is shown.
$$S(s) + 2O_2(g) + 2e^- \rightarrow SO_4^{2-}(g) \quad \Delta H = \Delta H^\circ_f\text{ of }SO_4^{2-}(g)$$
Calculate the standard enthalpy change of formation, $\Delta H^\circ_f$, of $SO_4^{2-}(g)$. It may be helpful to draw a labelled energy cycle. Use relevant data from Table 1.1 in your calculations.
Table 1.1
| energy change | value/kJ mol$^{-1}$ |
| :--- | :--- |
| lattice energy of barium sulfate, BaSO$_4$(s) | –2469 |
| standard enthalpy change of formation of barium sulfate | –1473 |
| standard enthalpy change of atomisation of barium | +180 |
| first ionisation energy of barium | +503 |
| second ionisation energy of barium | +965 |
| standard enthalpy change of atomisations of sulfur | +279 |
| standard(ii) Suggest how the lattice energy of BaSO$_4$(s) differs from the lattice energy of Cs$_2$SO$_4$(s). Explain your answer.
[2]
(e) The reaction of solid hydrated barium hydroxide, Ba(OH)$_2$·8H$_2$O, with ammonium salts is endothermic.
(i) Calculate the minimum temperature at which the reaction of Ba(OH)$_2$·8 H$_2$O with NH$_4$NO$_3$ becomes feasible. Show all your working.
$$\text{Ba(OH)}_2 \cdot 8\text{H}_2\text{O}(s) + 2\text{NH}_4\text{NO}_3(s) \rightarrow 2\text{NH}_3(g) + \text{Ba(NO}_3)_2(s) + 10\text{H}_2\text{O(l)} \quad \Delta H^\circ_r = +132\text{kJ mol}^{-1}$$
$$\Delta S^\circ_r = +616\text{J K}^{-1}\text{mol}^{-1}$$
temperature = ... °C [2]
(ii) Barium hydroxide reacts readily with ammonium chloride on mixing at room temperature.
$$\text{Ba(OH)}_{2} \cdot 8\text{H}_2 (a) Define transition element.
[1]
(b) Sketch the shape of a 3d$_{z^2}$ orbital.
[1]
(c) Manganese(IV) oxide, MnO$_2$, acts as a heterogeneous catalyst in the decomposition of hydrogen peroxide, H$_2$O$_2$.
(i) Explain what is meant by a heterogeneous catalyst.
[1]
(ii) Describe the mode of action of a heterogeneous catalyst in a reaction.
[3]
(d) Manganese(VII) oxide, Mn$_2$O$_7$, can be made by treatment of KMnO$_4$ with concentrated sulfuric acid (reaction 1).
Mn$_2$O$_7$ readily decomposes at room temperature to form manganese(IV) oxide and a colourless diatomic gas (reaction 2).
Construct equations for both the reactions described.
reaction 1 ..... [2]
reaction 2 ..... [2](e) Aqueous manganese(II) ions show similar chemical properties to aqueous copper(II) ions when reacted separately with NaOH(aq) and with concentrated HCl.
(i) Write the ionic equation, and state the type of reaction, for the reaction of $[\text{Mn(H}_2\text{O})_6]^{2+}$ with NaOH(aq).
ionic equation ..... [2]
type of reaction ..... [2]
(ii) Write the ionic equation, and statethe type of reaction, for the reaction of $[{\text{Mn(H}_2\text{ O}})_6]^{2+}$ with concentrated HCl.
ionic equation ..... [2]
typeofreaction..... [2]
(iii) Table 2.1 lists relevant electrode potentials for some electrode reactions.
<table><thead><tr><th>electrode reaction</th><th>$E^\circ/\text{V}$</th></tr></thead><tbody><tr><td>$\text{Mn}^{2+} + 2\text{e}^- \rightleftharpoons \text{Mn}$</td><td>-1.18</td></3 (a) The rate of reaction between 2-chloro-2-methylpropane, $(\text{CH}_3)_3\text{CCl}l$, and methanol is investigated. When a large excess of methanol is used, the overall reaction is first order.
$$(\text{CH}_3)_3\text{CCI} + \text{CH}_3\text{OH} \rightarrow (\text{CH}_3)_3\text{COCH}_3 + \text{HCl}$$
Fig. 3.1 shows the results obtained.
**Fig. 3.1**
(i) Use the graph to determine the rate of reaction at 40 s. Show all your working.
$$\text{rate} = \dots\dots\dots\dots\mathrm{mol}\,\mathrm{dm}^{-3}\,\mathrm{s}^{-1}$$ [1]
(ii) Use the graph to show that the overall reaction is first order. Explain your answer.
[2]
(b) In a different reaction, which is also a first order reaction, 75% of the reactant is consumed in 320 s.
Calcul(c) (i) Define standard electrode potential, $E^\circ$.
[1]
(ii) A salt bridge is used in an electrochemical cell.
State the function of the salt bridge. Explain your answer.
[1]
(iii) Complete the diagram of the apparatus that can be used to measure the $E^\circ$ of the $\text{Cr}_2\text{O}_7^{2-}(\text{aq})$, $\text{H}^+(\text{aq})/\text{Cr}^{3+}(\text{aq})$ electrode against the standard hydrogen electrode.
Your diagram should be fully labelled to identify all apparatus, substances and conditions.
[salt bridge]
[3]
(iv) The $E^\circ$ of the $\mathrm{Cr}_2\mathrm{O}_7^{2-}(\text {aq})$, $\text{H}^+$(aq)/$\text{Cr}^{3+}(\text {aq})$ electrode is +1.33 V.
Label the negative electrode and the direction of electron flow in the external circuit when the current flows in your diagram (d) Table 3.1 lists relevant electrode potentials for some electrode reactions for use in (d)(i) and (d)(ii).
Table 3.1
| electrode reaction | $E^\circ$/V |
| :--- | :--- |
| $\text{Cr}_2\text{O}_7^{2-} + 14\text{H}^+ + 6\text{e}^- \rightleftharpoons 2\text{Cr}^{3+} + 7\text{H}_2\text{O}$ | +1.33 |
| $\text{CH}_3\text{CHO} + 2\text{H}^+ + 2\text{e}^- \rightlefsharpoons \text{CH}_3\text{CH}_2\text{OH}$ | -0.61 |
| $\text{CH}_3\text{\text{COOH}} + 2\text{H}^+ +2\text{e}^- \rightlefshtriangleq \text{CH}_3\text{\text{CHO}} + \text{H}_2\text{O}$ | -0.94 |
| $\text{O}_2 + 4\text{H}^+ + 4\text{e}^- \rightlefhsarpoons 2\text{H}_2\text{O}$ | +1.23 |
(i) Ethanal is oxidised to ethanoic acid in the presence of $\text{Cr}_2\text{O}_{7}^{2-}$ ions.
Construct the ionic equation for the oxidation 4 (a) The 3d orbitals in an isolated Fe$^{2+}$ ion are degenerate.
Complete the diagram to show the splitting of the 3d orbital energy levels in an isolated Fe$^{2+}$ion and when Fe$^{2+}$ forms an octahedral complex.
[2]
(b) (i) Bipyridine, bipy, is a bidentate ligand.
Fig. 4.1
Explain what is meant by bidentate ligand.
... [2](ii) The complex $[Fe(bipy)_3]^{2+}$ exists as two stereoisomers.
Complete the three-dimensional diagrams to show the two stereoisomers of $[Fe(bipy)_3]^2+$.
State the type of stereoisomerism shown.
Use $N-N$ to represent bipy in your diagrams.
type of stereoisomerism ... [3]
(c) Standard electrode potentials can be used to compare the stability of different complex ions for a given transition element.
Table 4.1 lists electrode potentials for some electrode reactions for $Fe^{3+}/Fe^{2+}$ systems.
<table><thead><tr><th>electrode reaction</th><th>E°/V</th></tr></thead><tbody><tr><td>[Fe(H<sub>2</sub>O)<sub>6}]^{3+} + e^{-} ⇌ [Fe(H<sub>2</sub> O)<sub>6}]^{2+}$</td><td>$+0.77</td></tr><tr><td>[Fe(CN)<sub>6}]^{3-} + e^{-} ⇌ [ Fe(CN)<sub>6}]^{4-}$</td><td>$+0,36</td></tr><tr><td>[ Fe(bip(d) The ligand bipyridine consists of two pyridine rings.
Pyridine, $C_5H_5N$, and benzene, $C_6H_6$, have similar planar, cyclic structures.
Fig. 4.2
By reference to the hybridisation of the carbon atoms and the nitrogen atom, and orbital overlap, suggest how the $\sigma$ and $\pi$ bonds are formed in a pyridine molecule.
[3]
(e) Pyridine reacts with $Cl^2$ in the presence of $AlCl_3$ as shown in Fig. 4.3.
$$\text{pyridine} + Cl^2 \rightarrow AlCl_3 + HCl$$
Fig. 4.3
The mechanism of this reaction is similar to that of the chlorination of benzene. $AlCl_3$ reacts with chlorine to generate an electrophile, $Cl^+$.
Complete the diagram to show the mechanism for the reaction of pyridine with $Cl^+$. Include all relevant charges, dipoles, lone pairs of electrons and curly arrows as ap5 (a) Compare the relative acidities of benzoic acid ($C_6H_5COOH$), phenylmethanol ($C_6H_5CH_2OH$), and phenol ($C_6H_5OH$). Explain your reasoning. | most acidic | least acidic | | :---: | :---: | (b) A series of nine separate experiments is carried out as shown in Table 5.1. Complete the table by placing a tick ($\checkmark$) in the relevant box if a reaction occurs. Place a cross ($x$) in the box if no reaction occurs. Table 5.1 | | benzoic acid | phenylmethanol | phenol | | :---: | :---: | :---: | :--- | Na(s) | | | | | NaOH(aq) | | | | | $Na_2CO_3(aq)$ | | | | (c) (i) Benzoyl chloride, $C_6H_5COCl$, can be synthesised by the reaction of benzoic acid with either $PCl_5$ or $SOCl_2$. Complete the equations for these reactions. reaction 1 $C_6H_5COOH + PCl_5 \rightarrow C_6H_5C
(d) Benzoyl chloride is hydrolysed by water at room temperature to form benzoic acid.
(i) Complete the diagram to show the mechanism for the reaction between $C_6H_5COCl$ and $H_2O$.
Include charges, dipoles, lone pairs of electrons and curly arrows as appropriate.
$$\text{H}_2\text{O} \rightarrow \text{products}$$
[4]
(ii) Name the type of mechanism you showed in (d)(i).
... [1](e) Acyl chlorides react with sodium carboxylates to form acid anhydrides as shown in Fig. 5.1.
$$\text{acyl chloride} + \text{sodium carboxylate} \rightarrow \text{acid anhydride} + \text{NaCl}$$
Fig. 5.1
The condensation polymers, polyanhydride and polyester, are formed by similar methods.
The repeat unit for a polyanhydride is shown in Fig. 5.2.
Polyanhydride
Fig. 5.2
(i) Use Fig. 5.1 and Fig. 5.2 to suggest the structures of the two monomers used to make this polyanhydride.
[2]
(ii) Polyanhydrides are biodegradable polymers.
Suggest how this polyanhydride can be degraded.
[Total: 16]6 (a) Describe what is meant by a racemic mixture.
(b) Asparagine is an amino acid that contains a chiral carbon atom and displays stereoisomerism. Separate samples of asparagine are dissolved in CDCl$_3$ and analysed using carbon-13 and proton ($^1\text{H}$) NMR spectroscopy.
Fig. 6.1
Predict the number of peaks seen in the carbon-13 and proton ($^2\text{H}$) NMR spectra of asparagine.
| | carbon-13 NMR | proton ($^2\text{H}$ NMR |
| :--- | :---: | :---: |
| number of peaks | | |
(c) The isoelectric point of asparagine, asn, is at pH 5.4.
(i) Describe the meaning of the term isoelectric point.
(ii) Draw the structure of asparagine at pH 1.0.(d) Asparagine can polymerise to form poly(asparagine).
Draw the structure of poly(asparagine), showing two repeat units. The peptide linkage should be shown displayed.
(e) The isoelectric point of lysine, lys, is at pH 9.8.
$$\text{lysine}$$
$$(\text{CH}_2)_4$$
$H_2\text{N} \longrightarrow \text{C} \longrightarrow \text{COOH}$$
Fig. 6.2
A mixture of the dipeptide lys-asn and its two constituent amino acids, asparagine and lysine, is analysed by electrophoresis using a buffer at pH 5.0. The results obtained are shown in Fig. 6.3.
$$\text{mixture applied here}$$
E F G
Fig. 6.3
Suggest identities for the species responsible for spots E, F and G. Explain your answers.
| spot | identity |
| :--- | :--- |
| E | |
| F | |
| G | |(f) Thin-layer and gas-liquid chromatography can be used to analyse mixtures of substances. Each type of chromatography makes use of a stationary phase and a mobile phase. (i) Complete Table 6.1 with an example of each of these. Table 6.1 | | stationary phase | mobile phase | | :---: | :---: | :---: | | thin-layer chromatography | | | | gas-liquid chromatography | | | (ii) An unknown amino acid is analysed using thin-layer chromatography. Two chromatographs of the unknown amino acid and four reference amino acids, P, Q, R and S, are obtained using two different solvents. Fig. 6.4 Identify the unknown amino acid. Justify your answer. [1]
(g) A mixture containing three organic compounds is analysed by gas chromatography and mass spectrometry. The gas chromatogram is shown.
| peak | J | K | L |
| :---: | :---: | :---: | :---
| area/mm² | 8 | 44 | 58 |
Fig. 6.5
The area underneath each peak is proportional to the mass of the respective compound in the mixture.
The concentration of $K$ in the mixture is $5.52 \times 10^{-2} \text{ g dm}^{-3}$.
Calculate the concentration, in mol dm$^{-3}$, of compound $L$ in the mixture.
$$M_r: \text{L}, 116$$
concentration of $L = \dots\dots\dots\dots\mathrm{mol dm}^{-3}$ [1]
[Total: 12]7 Procaine is used as an anaesthetic in medicine. It can be synthesised from methylbenzene in five steps as shown in Fig. 7.1.  (a) (i) Name all the functional groups present in procaine. [1] (ii) A molecule of procaine has 13 carbon atoms. State the number of carbon atoms that are sp, sp² and sp³ hybridised in procaine. sp carbons = ... sp² carbons = ... sp³ carbons = [1] (b) The proton ($^1$H) NMR spectrum of procaine dissolved in D$_2$O is recorded. Predict the number of peaks observed. [1] (c) State why procaine can act as a base. [1]
(d) Compound X can be synthesised in two steps from methylbenzene.
(i) Draw the structure of compound W in the box provided. [1]
(ii) State the reagents and conditions for step 1 and step 2.
step 1 ...
step 2 ... [2]
(e) Procaine is synthesised in three steps from X.
Suggest the reagents and conditions for step 4 and for step 5 in Fig. 7.1.
step 4 ...
step 5 ... [3]
(f) (i) Explain what is meant by partition coefficient, $K_{pc}$.
... [2]
(ii) The partition coefficient of procaine between octan-1-ol and water is 1.77.
Octan-1-ol and water are immiscible. A solution containing 0.500 g of procaine in 75.0 cm$^3$ of water is shaken with 50.0 cm$^3$ of octan-1-ol.
Calculate the mass of procaine that is extracted into the octan-1-ol.
mass of procaine extracted = .....