A Level Chemistry 9701 Paper 41, Oct/Nov 2023

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9701/41 · Oct/Nov 2023

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Fluorine reacts with chlorine dioxide, $C l O_{2}$ , as shown. $F_{2} (g) + 2 C l O_{2} (g) \to 2 F C l O_{2} (g)$ The rate of the reaction is first order with respect to the concentration of $F_{2}$ and first order with respect to the concentration of $C l O_{2}$ . No catalyst is involved.

a(i)

Suggest a two-step mechanism for this reaction. step 1 $\to$ step 2 $\to$

[2]

a(ii)

Identify the rate-determining step in this mechanism. Explain your answer.

[1]

b(i)

When the rate of the reaction is measured in $m o l d m^{- 3} s^{- 1}$ the numerical value of the rate constant, $k$ , is 1.22 under certain conditions. Complete the rate equation for this reaction, stating the overall order of the reaction. rate = overall order of reaction =

[1]

b(ii)

Use your rate equation in (i) to calculate the rate of the reaction when the concentrations of $F_{2}$ and $C l O_{2}$ are both $2.00 \times 10^{- 3} m o l d m^{- 3}$ . rate = .............................. $m o l d m^{- 3} s^{- 1}$

[1]

c(i)

Under different conditions, and in the presence of a large excess of $C l O_{2}$ , the rate equation is as shown. $r a t e = k_{1} [F_{2}]$ The half-life, $t_{\frac{1}{2}}$ , of the concentration of $F_{2}$ is $4.00 s$ under these conditions. Calculate the numerical value of $k_{1}$ , giving its units. Give your answer to three significant figures. $k_{1} =$ .............................. units ..............................

[2]

c(ii)

An experiment is performed under these conditions in which the starting concentration of $F_{2}$ is $0.00200 m o l d m^{- 3}$ . Draw a graph on the grid in Fig. 1.1 to show how the concentration of $F_{2}$ changes over the first $12 s$ of the reaction.

[1]

c(iii)

Use your graph in Fig. 1.1 to find the rate of the reaction when the concentration of $F_{2}$ is $0.00100 m o l d m^{- 3}$ . Show your working on the graph. rate = .............................. $m o l d m^{- 3} s^{- 1}$

[1]

Define $K_{w}$ mathematically by completing the expression. $K_{w} =$ ..........................................................................................................................................

[1]

b(i)

Two solutions, $V$ and $W$ , are described. • $V$ is $H C l (a q)$ . • $W$ is $N a O H (a q)$ . • The concentration of $H C l$ in $V$ is the same as the concentration of $N a O H$ in $W$ . • The $p H$ values of $V$ and $W$ differ by exactly $11.00$ at $298 K$ . Calculate the concentration of $H C l$ in $V$ . concentration of $H C l$ in $V =$ .............................. $m o l d m^{- 3}$

[2]

b(ii)

Equal volumes of the two solutions $V$ and $W$ are mixed, giving solution $X$ . Name solution $X$ and state its $p H$ . solution $X$ .............................. $p H$ ..............................

[1]

b(iii)

A $1 c m^{3}$ sample of $1.0 m o l d m^{- 3} H N O_{3}$ is added to $100 c m^{3}$ of solution $X$ , forming mixture $Y$ . A $1 c m^{3}$ sample of $1.0 m o l d m^{- 3} K O H$ is added to $100 c m^{3}$ of solution $X$ , forming mixture $Z$ . Estimate the $p H$ of mixtures $Y$ and $Z$ . No calculations are required. mixture $Y$ .............................. mixture $Z$ ..............................

[1]

c(i)

$C H_{3} C H_{2} C O O H$ , $C H_{3} C C l_{2} C O O H$ and $H_{2} S O_{4}$ are all acidic. Suggest the trend in the relative acid strength of these three compounds. Explain your answer. ....................................... ....................................... ....................................... strongest acid weakest acid explanation

[3]

c(ii)

When concentrated $H_{2} S O_{4}$ is added to water a series of acid-base reactions occurs. There are three conjugate acid-base pairs that can be identified during this series of reactions. Write the formulae of these three conjugate acid-base pairs. conjugate acid 1 ......................................... conjugate base 1 ......................................... conjugate acid 2 ......................................... conjugate base 2 ......................................... conjugate acid 3 ......................................... conjugate base 3 .........................................

[2]

d(i)

The partition coefficient, $K_{p c}$ , of a substance, $Q$ , between hexane and water is $7.84$ at $298 K$ . $Q$ is more soluble in hexane than it is in water. Define partition coefficient, $K_{p c}$ .

[1]

d(ii)

$5.00 g$ of $Q$ is shaken with a mixture of $100.0 c m^{3}$ of water and $100.0 c m^{3}$ of hexane at $298 K$ and left until there is no further change in concentrations. Calculate the mass of $Q$ dissolved in the water. mass of $Q =$ .............................. $g$

[1]

d(iii)

A sample of $Q$ is shaken with a different mixture of water and hexane and left until there is no further change in concentrations. It is found that the mass of $Q$ dissolved in each solvent is the same. Use the $K_{p c}$ value to suggest possible values for the volume of water used and the volume of hexane used. volume of water = .............................. $c m^{3}$ volume of hexane = .............................. $c m^{3}$

[1]

d(iv)

$Q$ is more soluble in hexane than it is in water. It is suggested that $Q$ is one of $K C l$ , $C H_{3} (C H_{2})_{4} O H$ or $H C O O H$ . Identify $Q$ . Explain your answer.

[1]

Hydrogen peroxide is a liquid at $298 K$ . It is moderately stable under room conditions but will decompose quickly if a catalyst is added. $reaction 1 2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)$

a(i)

Define entropy.

[1]

a(ii)

Predict the sign of the standard entropy change of reaction 1. Explain your answer. sign .............................. explanation

[1]

Some bond energy data are shown in Table 3.1. Table 3.1

type of bond	bond energy / $k J m o l^{- 1}$
O–O	150
O–H	460
O=O	496

Use the data in Table 3.1 to show that the enthalpy change of the following reaction is $- 196 k J m o l^{- 1}$ . $2 H_{2} O_{2} (g) \to 2 H_{2} O (g) + O_{2} (g)$

[1]

Some standard entropies, $S^{⊖}$ , are shown in Table 3.2. Table 3.2

substance	$S^{⊖} / J K^{- 1} m o l^{- 1}$
$H_{2} O_{2} (l)$	$+ 102$
$H_{2} O (l)$	$+ 70$

The enthalpy change and Gibbs free energy change for the following reaction are shown. $2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g) Δ H^{⊖} = - 196 k J m o l^{- 1}, Δ G^{⊖} = - 238 k J m o l^{- 1}$ Use the data given to calculate the standard entropy of oxygen, $S^{⊖}, O_{2} (g)$ . $S^{⊖}, O_{2} (g) =$ .............................. $J K^{- 1} m o l^{- 1}$

[3]

The decomposition of $H_{2} O_{2} (a q)$ is catalysed by aqueous iron(III) chloride and by silver metal. Identify which of these two catalysts is acting as a homogeneous catalyst. Explain your answer. homogeneous catalyst .............................................................................................................. explanation

[1]

e(i)

The $E^{⊖}$ values for two electrode reactions are given. $H_{2} O_{2} + 2 H^{+} + 2 e^{-} ⇌ 2 H_{2} O E^{⊖} = + 1.77 V$ $C r^{3 +} + e^{-} ⇌ C r^{2 +} E^{⊖} = - 0.41 V$ An electrochemical cell is constructed with the following half-cells (electrodes): • an acidified solution of $H_{2} O_{2}$ , a platinum wire • $C r^{2 +}$ mixed with $C r^{3 +}$ , a platinum wire. Identify the positive half-cell and calculate the standard cell potential, $E_{c e l l}^{⊖}$ . positive half-cell .............................. $E_{c e l l}^{⊖} =$ .............................. $V$

[1]

e(ii)

Calculate the value of $Δ G^{⊖}$ for the cell reaction that occurs, per mole of $H_{2} O_{2}$ . $Δ G^{⊖} =$ .............................. $k J m o l^{- 1}$

[2]

f(i)

The $E^{⊖}$ values for two electrode reactions are given. $H_{2} O_{2} + 2 H^{+} + 2 e^{-} ⇌ 2 H_{2} O E^{⊖} = + 1.77 V$ $C o^{3 +} + e^{-} ⇌ C o^{2 +} E^{⊖} = + 1.82 V$ An electrochemical cell is constructed with the following half-cells. half-cell 1 an acidified solution of $H_{2} O_{2}$ under standard conditions, a platinum wire half-cell 2 a solution containing $0.020 m o l d m^{- 3} C o^{3 +}$ and $2.0 m o l d m^{- 3} C o^{2 +}$ , a platinum wire Use the Nernst equation to calculate the value of $E$ , the electrode potential of half-cell 2 under these conditions. $E =$ .............................. $V$

[2]

f(ii)

Write an equation for the cell reaction that occurs in this cell under these conditions.

[1]

g(i)

Define enthalpy change of hydration, $Δ H_{h y d}$ .

[1]

g(ii)

Aluminium fluoride, $A l F_{3}$ , is an ionic solid. Complete and label the energy cycle to show the relationship between: • the enthalpy change of solution of $A l F_{3}$ , $Δ H_{s o l}^{⊖}$ • the lattice energy of $A l F_{3}$ , $Δ H_{l a t t}^{⊖}$ • the enthalpy changes of hydration of $A l^{3 +}$ and $F^{-}$ , $Δ H_{h y d}^{⊖}$ . Include state symbols for all substances and ions.

[2]

g(iii)

Relevant data for this question are given. $Δ H_{s o l}^{⊖} A l F_{3} = - 209 k J m o l^{- 1}$ $Δ H_{h y d}^{⊖} A l^{3 +} = - 4690 k J m o l^{- 1}$ $Δ H_{h y d}^{⊖} F^{-} = - 506 k J m o l^{- 1}$ Use these data and your energy cycle in (g)(ii) to calculate the $Δ H_{l a t t}^{⊖}$ of $A l F_{3}$ . $Δ H_{l a t t}^{⊖}$ of $A l F_{3} =$ .............................. $k J m o l^{- 1}$

[1]

a(i)

Cobalt(II) nitrate, $C o (N O_{3})_{2}$ , is a reddish-brown crystalline solid. It dissolves in water to form a solution containing $[C o (H_{2} O)_{6}]^{2 +}$ complex ions. Complete Table 4.1 giving the formula of the cobalt-containing species that is formed in each of the three reactions described. Table 4.1

reaction	reagent added to $[C o (H_{2} O)_{6}]^{2 +} (a q)$	cobalt-containing species formed
1	$N a O H (a q)$
2	an excess of $N H_{3} (a q)$
3	an excess of conc. $H C l (a q)$

[2]

a(ii)

Describe the colour change seen in reaction 3. original colour of $[C o (H_{2} O)_{6}]^{2 +} (a q)$ .................................................................................... final colour after addition of an excess of conc. $H C l (a q)$ ..................................................

[1]

b(i)

Calcium nitrate, $C a (N O_{3})_{2}$ , is a white crystalline solid. When heated, it starts to decompose at approximately $500^{\circ} C$ . Write an equation for the decomposition of $C a (N O_{3})_{2}$ .

[1]

b(ii)

Suggest temperatures at which $M g (N O_{3})_{2}$ and $B a (N O_{3})_{2}$ start to decompose. Explain your answer. temperature at which $M g (N O_{3})_{2}$ starts to decompose ................................................. $^{\circ} C$ temperature at which $B a (N O_{3})_{2}$ starts to decompose ................................................... $^{\circ} C$ explanation

[3]

Transition elements behave as catalysts and can form complex ions.

Explain why transition elements behave as catalysts.

[2]

b(i)

Silver forms the linear complex ion $[A g (C N)_{2}]^{-}$ . Copper forms the tetrahedral complex ion $[C u (C N)_{4}]^{3 -}$ . Titanium forms the complex $[T i C l_{4} (d i a r s)_{2}]$ , where diars is a neutral bidentate ligand. State the oxidation state and the coordination number of titanium in $[T i C l_{4} (d i a r s)_{2}]$ . oxidation state .............................. coordination number ..............................

[1]

b(ii)

Draw three-dimensional diagrams to show the shapes of $[A g (C N)_{2}]^{-}$ and $[C u (C N)_{4}]^{3 -}$ , in the boxes. Label one bond angle on each diagram.

[2]

c(i)

The numerical value of the stability constant, $K_{s t a b}$ , of the copper(I) complex $[C u (C N)_{4}]^{3 -}$ is $2.0 \times 10^{27}$ . Write an expression for the $K_{s t a b}$ of $[\mathrm{Cu(CN)_4}]^{3-}. $K_{s t a b} =$

[1]

c(ii)

In a solution the concentrations of $C N^{-}$ and $[C u (C N)_{4}]^{3 -}$ are both $0.0010 m o l d m^{- 3}$ . Use your expression from (c)(i) and the value of $K_{s t a b}$ to calculate the concentration of $C u^{+} (a q)$ in this solution. concentration of $C u^{+} (a q) =$ .............................. $m o l d m^{- 3}$

[1]

d(i)

A piece of a copper-containing alloy has a mass of $0.567 g$ . It is dissolved in an acid giving $100.0 c m^{3}$ of a blue solution in which all the copper is present as $C u^{2 +}$ ions. An excess of $K I (a q)$ is added to a $25.0 c m^{3}$ sample of this solution. All of the copper is precipitated as white $C u I (s)$ . $C u^{2 +}$ ions are the only component in the solution that react with $K I (a q)$ . This is reaction 1. $reaction 1 2 C u^{2 +} + 4 I^{-} \to 2 C u I + I_{2}$ The liberated $I_{2}$ is then titrated with $0.0200 m o l d m^{- 3} S_{2} O_{3}^{2 -}$ . This is reaction 2. $reaction 2 I_{2} + 2 S_{2} O_{3}^{2 -} \to 2 I^{-} + S_{4} O_{6}^{2 -}$ The titration requires $20.10 c m^{3}$ of $0.0200 m o l d m^{- 3} S_{2} O_{3}^{2 -}$ to reach the end-point. Calculate the number of moles of $I_{2}$ that are reduced in this titration. number of moles of $I_{2} =$ .............................. $m o l$

[1]

d(ii)

Calculate the number of moles of copper in the original piece of alloy. number of moles of copper = .............................. $m o l$

[1]

d(iii)

Calculate the percentage of copper in the alloy. percentage of copper = .............................. %

[1]

d(iv)

Suggest why a solution of $C u^{2 +}$ is coloured but solid $C u I$ is white.

[2]

a(i)

Five ligands are listed in Table 6.1. Table 6.1

ligand	type of ligand
$N H_{3}$
$E D T A^{4 -}$
$C N^{-}$
$H_{2} N C H_{2} C H_{2} N H C H_{2} C H_{2} N H_{2}$	tridentate
$C_{2} O_{4}^{2 -}$

Complete Table 6.1 using the words monodentate, bidentate and polydentate only. Each of these three words may be used once, more than once, or not at all.

[2]

a(ii)

The molecule $H_{2} N C H_{2} C H_{2} N H C H_{2} C H_{2} N H_{2}$ is a tridentate ligand. Suggest the meaning of tridentate ligand.

[1]

a(iii)

Suggest how $H_{2} N C H_{2} C H_{2} N H C H_{2} C H_{2} N H_{2}$ acts as a tridentate ligand.

[1]

b(i)

Nickel forms the octahedral complex $[N i (e n)_{2} (H_{2} O)_{2}]^{2 +}$ . This complex can exist in three isomeric forms, listed in Table 6.2. One of these forms is a trans isomer, the other forms are two different cis isomers. Table 6.2

isomer	polarity
trans isomer
cis isomer 1
cis isomer 2

Complete Table 6.2 using the terms polar or non-polar. Each term may be used once, more than once, or not at all.

[1]

b(ii)

Describe the difference between cis isomer 1 and cis isomer 2.

[1]

Sunset Yellow is an additive used for colouring foods. A synthetic route for making Sunset Yellow is shown. Molecules $E$ and $G$ each contain one $- S O_{3}^{-}$ group. These groups are unchanged in the formation of Sunset Yellow.

State the molecular formula of the Sunset Yellow anion.

[1]

Deduce the structures of $E$ , $F$ and $G$ and draw them in the boxes in Fig. 7.1.

[3]

Suggest suitable reagents and conditions for step 1 and 2. step 1 ........................................................................................................................................ step 2 ........................................................................................................................................

[3]

Predict the number of peaks in the carbon-13 NMR spectrum of the Sunset Yellow anion.

[1]

Capsaicin is found in chilli peppers. You should assume the $C H_{3} O$ group is unreactive in the reactions involved in this question.

Name all the functional groups in capsaicin in addition to the $C H_{3} O$ group.

[1]

Complete the equation for the reaction of capsaicin with an excess of $B r_{2} (a q)$ in the dark. Draw the structure of the organic product in the labelled box.

[3]

Capsaicin is heated with an excess of hydrogen gas in the presence of platinum metal. The six-membered ring reacts in the same way as benzene under these conditions. Draw the structure of the organic product formed.

[2]

d(i)

When capsaicin is treated with reagent $J$ under suitable conditions one of the products is methylpropanoic acid, $C H_{3} C H (C H_{3}) C O O H$ . Identify reagent $J$ and any necessary conditions.

[1]

d(ii)

There are three different peaks in the proton ( $^{1} H$ ) NMR spectrum of $C H_{3} C H (C H_{3}) C O O H$ in $C D C l_{3}$ . Table 8.1

environment of proton	example	chemical shift range $δ$ / ppm
alkane	$- C H_{3}$ , $- C H_{2} -$ , $> C H -$	0.9–1.7
alkyl next to C=O	$C H_{3} - C = O$ , $- C H_{2} - C = O$ , $> C H - C = O$	2.2–3.0
alkyl next to aromatic ring	$C H_{3} - A r$ , $- C H_{2} - A r$ , $> C H - A r$	2.3–3.0
alkyl next to electronegative atom	$C H_{3} - O$ , $- C H_{2} - O$ , $- C H_{2} - C l$	3.2–4.0
attached to alkene	$= C H R$	4.5–6.0
attached to aromatic ring	$H - A r$	6.0–9.0
aldehyde	$H C O R$	9.3–10.5
alcohol	$R O H$	0.5–6.0
phenol	$A r - O H$	4.5–7.0
carboxylic acid	$R C O O H$	9.0–13.0

Use Table 8.1 to complete Table 8.2 and state: • the typical proton ( $^{1} H$ ) chemical shift values ( $δ$ ) for the protons • the splitting pattern (singlet, doublet, triplet, quartet or multiplet) shown by each peak • the explanation for the splitting patterns of the $C H_{3}$ protons and the $C H$ proton. Table 8.2

environment	$δ$ / ppm	splitting pattern	explanation for splitting pattern
$C H_{3}$
$C H$
$C O O H$

[3]

e(i)

Capsaicin is heated with an excess of hot aqueous $N a O H$ . Draw the structures of the two organic products $H$ and $K$ . $H C_{8} H_{10} N O_{2} N a K C_{10} H_{17} O_{2} N a$

[2]

e(ii)

Name the two types of reaction occurring in (e)(i).

[1]

Draw the structure of the organic product $L$ formed when capsaicin is treated with $L i A l H_{4}$ in dry ether.

[1]

a(i)

Benzoyl chloride, $C_{6} H_{5} C O C l$ , can be made from ethyl benzene in a two-step process. A reaction scheme is shown. Draw the intermediate organic compound $M$ in the box.

[1]

a(ii)

Suggest suitable reagents and conditions for step 1 and step 2. step 1 ................................................................................................................................. step 2 .................................................................................................................................

[2]

a(iii)

Identify the type of reaction in step 1 and step 2. step 1 ................................................................................................................................. step 2 .................................................................................................................................

[2]

b(i)

$C_{6} H_{5} C O C l$ reacts with phenol, $C_{6} H_{5} O H$ , to give the ester phenyl benzoate, $C_{6} H_{5} C O O C_{6} H_{5}$ . An incomplete description of the mechanism of this reaction is shown in Fig. 9.1. Complete the mechanism in Fig. 9.1 and include: • all relevant dipoles ( $δ +$ and $δ -$ ) and full electric charges ( $+$ and $-$ ) on the species in box one and in box two • all relevant lone pairs on the species in box one and in box two • all relevant curly arrows to show the movement of electron pairs in box one and in box two • the formula of the second product in box three.

[4]

b(ii)

Name this mechanism.

[1]

Benzoyl chloride, chlorobenzene and chloroethane differ in their rates of hydrolysis when each compound is added separately to water at $25^{\circ} C$ . Suggest the relative ease of hydrolysis of these three compounds. Explain your answer. ......................................... ......................................... ......................................... hardest to hydrolyse easiest to hydrolyse explanation

[3]

Mark scheme

9701/41 · Oct/Nov 2023

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1a(i) · 2 marks

M1
F2 + ClO2 → FClO2 + F OR F2 + ClO2 → F2ClO2
M2
ClO2 + F → FClO2 OR F2ClO2 + ClO2 → 2FClO2

1a(ii) · 1 mark

1 mark
first step AND has one mole / molecule of F2 and ClO2 OR same moles of reactants as orders in rate equation

1b(i) · 1 mark

1 mark
rate = k [F2][ClO2] / rate = 1.22 [F2][ClO2] AND second / 2 BOTH

1b(ii) · 1 mark

1 mark
rate = 1.22 × 2 × 10-3 × 2 × 10-3 = 4.88 x 10-6

1c(i) · 2 marks

1 mark
k1 = (0.693 / 4) = 0.173 OR 1.73 × 10–1 (MUST BE 3SF)
1 mark
s–1

1c(ii) · 1 mark

1 mark
at 4 s = 0.001 at 8 s = 0.0005 at 12 s = 0.00025 smooth curve ALL correct

1c(iii) · 1 mark

1 mark
tangent drawn at 0.00100 mol dm–3 AND gradient dependent on their rate = Y / X in the range = 1.5–2.0 ×10–4

2a · 1 mark

1 mark
(Kw =)[H+][OH–] OR (Kw =)[H3O+][OH–]

2b(i) · 2 marks

M1
pH values 1.5 AND 12.5
M2
conc of HCl = 10–1.5 = 0.0316 ecf

2b(ii) · 1 mark

1 mark
sodium chloride / NaCl AND 7

2b(iii) · 1 mark

1 mark
(mixture Y) 1 to 3 AND (mixture Z) 11 to 13

2c(i) · 3 marks

1 mark
H2SO4 > CH3CCl2COOH > CH3CH2COOH
2 marks
explanation: any two bullets [1], any four bullets [2]: - H2SO4 is fully dissociated / strong acid - CH3CH2COOH / CH3CCl2COOH are partly dissociated / weak acids - Cl / chlorine is electron-withdrawing / electronegative - alkyl group (in CH3CH2COOH) is electron donating - stabilises / destabilises anion OR weakens / strengthens O-H bond (linked correctly) - correct reference to release of / donation of / form H+ / proton

2c(ii) · 2 marks

1 mark
any one correct pair: H3O+ and H2O / H2SO4 and HSO4– / HSO4– and SO42–
1 mark
all three correct pairs

2d(i) · 1 mark

1 mark
(the) ratio of the concentrations (of a solute between) two solvents / two liquids (at) equilibrium

2d(ii) · 1 mark

1 mark
mass = 5-x / x = 7.84 OR mass = x / 5-x = 7.84 mass = 0.5656 g mass = 4.43 g

2d(iii) · 1 mark

1 mark
Any numbers in which volume of water is 7.84 times volume of hexane e.g. 78.4 cm3 water 10 cm3 hexane

2d(iv) · 1 mark

1 mark
Q is CH3(CH2)4OH AND it is least polar / contains a large non-polar hydrocarbon chain / stronger id-id forces with hexane in Q OWTTE

3a(i) · 1 mark

1 mark
(number of possible) arrangements of particles / energy in a system OR measure / degree of disorder in / of a system

3a(ii) · 1 mark

1 mark
positive / + AND more gas molecules / particles in products OR more moles / molecules in products / RHS

3b · 1 mark

1 mark
ΔH = (2 × 150) – (1 × 496) (= –196) OR ΔH = (2 × 150) + (4 × 460) – (1 × 496) – (4 × 460) (= –196)

3c · 3 marks

1 mark
ΔG = ΔH –TΔS seen or used with correct signs
1 mark
–238 = –196 – 298ΔS leading to ΔS = (+)0.141 / 0.1409 (kJ K–1 mol–1) OR (+)141 / 140.9 (J K–1 mol–1) ecf from ΔG = ΔH + TΔS
1 mark
141 = (2 × 70) + S(O2(g)) – (2 × 102) leading to S, O2(g) = 205 / 204.94 (J K–1mol–1) ecf

3d · 1 mark

1 mark
iron(III) chloride / FeCl3 AND same state / phase as reactants / H2O2

3e(i) · 1 mark

1 mark
hydrogen peroxide / H2O2 AND +2.18

3e(ii) · 2 marks

1 mark
ΔG = –nE⦵cellF
1 mark
ΔG = (–2 × 2.18 × 96500) = –420.7 (kJ mol–1) ecf

3f(i) · 2 marks

1 mark
Nernst: (E =) E⦵ + (0.059 / z)log[ox] / [red] OR (E =) E⦵ + (RT / zF)ln[ox] / [red] OR (E =) 1.82 + (0.059 / 1)log(0.02 / 2)
1 mark
E = 1.82 + (0.059 / 1)log(0.02 / 2) = (+)1.702 (V) min 2sf OR E = 1.82 + [(8.314 × 298 / 1) × (96 500) ] ln(0.02 / 2) = (+)1.702

3f(ii) · 1 mark

1 mark
H2O2 + 2H+ + 2Co2+ → 2H2O + 2Co3+

3g(i) · 1 mark

1 mark
enthalpy change when one mole of gaseous ions forms an aqueous solution / dissolves in water

3g(ii) · 2 marks

1 mark
Substances with state symbols: AlF3(s), AlF3(aq) OR Al3+(aq) + (3)F–(aq), Al3+(g) (3)F–(g)
1 mark
changes identified and three correct arrow directions (one given)

3g(iii) · 1 mark

1 mark
ΔHlatt = –4690 + (3 × – 506) – (–209) = –5999 (kJ mol–1)

4a(i) · 2 marks

1 mark
any two of: Co(OH)2 OR Co(OH)2(H2O)4; [Co(NH3)6]2+ OR [Co(NH3)6]3+; [CoCl4]2–
1 mark
all three correct

4a(ii) · 1 mark

1 mark
pink to blue

4b(i) · 1 mark

1 mark
2Ca(NO3)2 → 2CaO + 4NO2 + O2 OR Ca(NO3)2 → CaO + 2NO2 + ½O2

4b(ii) · 3 marks

M1
Mg(NO3)2 below 480 °C, Ba(NO3)2 above 520 °C BOTH
M2
ionic radii of M2+ increases down the group OR radii of Ba2+ is greater (than Mg2+) OR charge density of M2+ decreases down the group OR charge density of Ba2+ is smaller (than Mg2+) ORA
M3
(larger cations) polarise / distort anion / NO3– less OR (larger ions) weaken N-O / N=O (bond) less ORA

5a · 2 marks

1 mark
more than one (stable) oxidation state
1 mark
empty / vacant (d) orbitals are energetically accessible OR empty / vacant (d) orbitals can form dative bonds with ligands

5b(i) · 1 mark

1 mark
oxid. no. = + 4 AND coord. no. = 8

5b(ii) · 2 marks

1 mark
any two of: - for Ag: NC—Ag—CN - angle = labelled 180° - for Cu: tetrahedral diagram - angle = labelled 109–110°
1 mark
all four points

5c(i) · 1 mark

1 mark
Kstab = [[Cu(CN)4]3–] / [Cu+] [CN–]4

5c(ii) · 1 mark

1 mark
[Cu+] = 5.0 × 10–19 (mol dm–3)

5d(i) · 1 mark

1 mark
mol of I2 = 0.5 × 0.02 × 20.1 / 1000 = 2.01 × 10–4

5d(ii) · 1 mark

1 mark
mol of Cu = 2.01 × 10–4 × 2 × 4 = 1.608 / 1.61 × 10–3

5d(iii) · 1 mark

1 mark
% of Cu = 100 × (1.608×10–3 × 63.5) / 0.567 = 18.0

5d(iv) · 2 marks

1 mark
Cu2+ is d9 / d shell / sub-shell / orbitals is / are not full AND Cu+ is d10 / d shell / sub-shell / orbitals is / are full
1 mark
d-d* transitions / d electron promotion not possible / possible (linked correctly)

6a(i) · 2 marks

1 mark
any two of: NH3 = monodentate; EDTA4– = polydentate / hexadentate; CN– = monodentate; C2O42– = bidentate
1 mark
all four correct

6a(ii) · 1 mark

1 mark
(ligand that) donates 3 lone pairs to central metal atom / ion OR (ligand that) forms 3 dative bonds to central metal atom / ion

6a(iii) · 1 mark

1 mark
ref to using the electrons / lone pair on (each) N / amine group

6b(i) · 1 mark

1 mark
trans = non-polar cis isomer 1 = polar cis isomer 2 = polar ALL

6b(ii) · 1 mark

1 mark
optical isomers / non-superimposable mirror images

7a · 1 mark

1 mark
C16H10N2O7S22– OR C16H10N2O7S2

7b · 3 marks

1 mark
Structure of E (4-aminobenzenesulfonate)
1 mark
Structure of F (benzenediazonium-4-sulfonate)
1 mark
Structure of G (4-hydroxynaphthalene-1-sulfonate)

7c · 3 marks

M1
step 1: HNO2 OR NaNO2 + HCl
M2
step 1: T ⩽ 10 °C
M3
step 2: NaOH(aq) / alkaline conditions

7d · 1 mark

1 mark
14 / fourteen

8a · 1 mark

1 mark
phenol, amide AND alkene / C=C all three needed

8b · 3 marks

M1
+ HBr
M2
structure of the organic product (brominated on benzene ring and across double bond)
M3
correct balanced equation

8c · 2 marks

M1
ring reduced
M2
alkene reduced

8d(i) · 1 mark

1 mark
hot AND concentrated acidified AND MnO4– / KMnO4 all

8d(ii) · 3 marks

1 mark
δ values: 0.9-1.7, 2.2-3.0, 9.0-13.0
1 mark
splitting: doublet, multiplet / heptet / septet, singlet
1 mark
explanations for SP: 1H on neighbouring C / next to CH / one vicinal proton; 6H on neighbouring C / next to 2 x (CH3) / six vicinal protons

8e(i) · 2 marks

1 mark
structure of H
1 mark
structure of K

8e(ii) · 1 mark

1 mark
hydrolysis AND neutralisation / acid-base

8f · 1 mark

1 mark
structure of L

9a(i) · 1 mark

1 mark
structure of M (benzoic acid)

9a(ii) · 2 marks

1 mark
hot (alkaline) KMnO4 / MnO4–
1 mark
SOCl2 OR PCl5 OR PCl3 + heat

9a(iii) · 2 marks

1 mark
oxidation
1 mark
(nucleophilic) substitution

9b(i) · 4 marks

1 mark
any two of points 1 to 10
1 mark
any five of points 1 to 10
1 mark
any eight of points 1 to 10
1 mark
all ten points

9b(ii) · 1 mark

1 mark
(nucleophilic) addition-elimination

9c · 3 marks

1 mark
order: chlorobenzene, chloroethane, benzoyl chloride
2 marks
explanation linked to their order: any two [1] any three [2]: - correct link to: strengthening (ArCl / RCl) C-Cl bond OR weakening (RCOCl) C-Cl bond OR C-Cl bond has partially double bond character (ArCl) OR C-Cl is more difficult to break (linked correctly) - chlorobenzene: lone pair / p-orbital on Cl overlaps / delocalised / incorporated with ring - benzoyl chloride: C of C-Cl has most electron deficient OR has an electronegative oxygen atom / two electronegative atoms / electron withdrawing C=O group - chloroethane: electron donating effect / positive inductive effect of alkyl / R group

Questions

1
Question 19 marks
Mark scheme ›
2
Question 214 marks
Mark scheme ›
3
Question 317 marks
Mark scheme ›
4
Question 47 marks
Mark scheme ›
5
Question 512 marks
Mark scheme ›
6
Question 66 marks
Mark scheme ›
7
Question 78 marks
Mark scheme ›
8
Question 814 marks
Mark scheme ›
9
Question 913 marks
Mark scheme ›

A Level Chemistry 9701 Paper 41, Oct/Nov 2023

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Mark scheme

1a(i) · 2 marks

1a(ii) · 1 mark

1b(i) · 1 mark

1b(ii) · 1 mark

1c(i) · 2 marks

1c(ii) · 1 mark

1c(iii) · 1 mark

2a · 1 mark

2b(i) · 2 marks

2b(ii) · 1 mark

2b(iii) · 1 mark

2c(i) · 3 marks

2c(ii) · 2 marks

2d(i) · 1 mark

2d(ii) · 1 mark

2d(iii) · 1 mark

2d(iv) · 1 mark

3a(i) · 1 mark

3a(ii) · 1 mark

3b · 1 mark

3c · 3 marks

3d · 1 mark

3e(i) · 1 mark

3e(ii) · 2 marks

3f(i) · 2 marks

3f(ii) · 1 mark

3g(i) · 1 mark

3g(ii) · 2 marks

3g(iii) · 1 mark

4a(i) · 2 marks

4a(ii) · 1 mark

4b(i) · 1 mark

4b(ii) · 3 marks

5a · 2 marks

5b(i) · 1 mark

5b(ii) · 2 marks

5c(i) · 1 mark

5c(ii) · 1 mark

5d(i) · 1 mark

5d(ii) · 1 mark

5d(iii) · 1 mark

5d(iv) · 2 marks

6a(i) · 2 marks

6a(ii) · 1 mark

6a(iii) · 1 mark

6b(i) · 1 mark

6b(ii) · 1 mark

7a · 1 mark

7b · 3 marks

7c · 3 marks

7d · 1 mark

8a · 1 mark

8b · 3 marks

8c · 2 marks

8d(i) · 1 mark

8d(ii) · 3 marks

8e(i) · 2 marks

8e(ii) · 1 mark

8f · 1 mark

9a(i) · 1 mark

9a(ii) · 2 marks

9a(iii) · 2 marks

9b(i) · 4 marks

9b(ii) · 1 mark

9c · 3 marks

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