plumiKinetics II: Edexcel A‑Level Chemistry questions
Every Edexcel A-Level Chemistry exam question on 16 Kinetics II, 2016–2025, with its mark scheme and examiner’s report.
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Calculations
Q5(d)
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Q9(a)(i)
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Q9(a)(ii)
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Q9(a)(iii)
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Q9(b)(i)
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Q9(b)(ii)
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Q4(a)
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Q4(b)(i)
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Q4(b)(ii)
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Q4(c)
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Q4(d)
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Q4(e)(i)
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Q4(e)(ii)
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Q4(e)(iii)
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Q3(c)(i)
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Q3(c)(ii)
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Q3(c)(iii)
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Q3(e)(i)
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Q3(e)(ii)
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Q3(f)
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All 94 questions on Kinetics II, as a list
- June 2025, Paper 2, Q5(d) (2 marks): A third student, in order to obtain the rate of reaction, measured the volume of gas produced at various times and used their data to plot the graph shown. 100
- June 2025, Paper 2, Q9(a)(i) (2 marks): Complete the table of data. (2)
- June 2025, Paper 2, Q9(a)(ii) (5 marks): Plot a graph of ln k against 1/T and use it to determine the activation energy, Ea, for this reaction in kJ mol–1. You must show your working on the graph and i
- June 2025, Paper 2, Q9(a)(iii) (2 marks): The rate constant for the reaction of 1‑bromopropane with aqueous potassium hydroxide has the units of dm3 mol–1 s–1. Explain why it can be deduced that the rea
- June 2025, Paper 2, Q9(b)(i) (3 marks): Draw the SN1 reaction mechanism for this hydrolysis. Include curly arrows and any relevant dipoles and lone pairs of electrons. (3)
- June 2025, Paper 2, Q9(b)(ii) (1 mark): State how your mechanism is consistent with the rate of reaction being independent of hydroxide ion concentration. (1)
- June 2025, Paper 3, Q4(a) (2 marks): Before carrying out Step 2, a student noticed droplets of an unknown colourless aqueous solution in the pipette. Describe how the pipette should be treated befo
- June 2025, Paper 3, Q4(b)(i) (2 marks): Explain why quenching is necessary. (2)
- June 2025, Paper 3, Q4(b)(ii) (2 marks): State a compound which can be added to the reaction mixture to quench the reaction. Include an equation for the reaction that takes place during the quenching p
- June 2025, Paper 3, Q4(c) (2 marks): One of the products of the reaction, iodopropanone (CH3COCH2I) is corrosive, strongly irritating to the eyes and can cause breathing difficulties. Explain why a
- June 2025, Paper 3, Q4(d) (4 marks): Show, by calculating the initial quantities of the reactants involved, that this experiment provides evidence for the order with respect to iodine only. (4)
- June 2025, Paper 3, Q4(e)(i) (2 marks): Plot a graph of titre against time. (2)
- June 2025, Paper 3, Q4(e)(ii) (1 mark): Give the reason why it is not necessary to calculate the concentration of iodine so that the order can be deduced. (1)
- June 2025, Paper 3, Q4(e)(iii) (2 marks): Deduce the order with respect to iodine. Justify your answer. (2)
- June 2024, Paper 2, Q3(c)(i) (2 marks): Deduce the order of reaction with respect to hydrogen peroxide and to iodide ions. (2) Order with respect to hydrogen peroxide Order with respect to iodide ions
- June 2024, Paper 2, Q3(c)(ii) (1 mark): Write the rate equation for the reaction using your answer to (c)(i). (1)
- June 2024, Paper 2, Q3(c)(iii) (2 marks): Calculate the rate constant, k, using data from Experiment 3. Include units in your answer. (2)
- June 2024, Paper 2, Q3(e)(i) (3 marks): Determine the gradient of the graph. Include units in your answer. You must show your working on the graph. (3)
- June 2024, Paper 2, Q3(e)(ii) (1 mark): Calculate the activation energy, Ea, of the reaction, in kJ mol–1, using your answer to (e)(i) and the Arrhenius equation shown. ln k = – E a × 1 + constant R T
- June 2024, Paper 2, Q3(f) (2 marks): Another way to write the Arrhenius equation is shown. k = Ae–Ea/RT The constant A is often called the collision factor as it is linked to the orientation of the
- June 2024, Paper 3, Q10(a)(i) (2 marks): Explain the purpose of the crushed ice in Step 3. (2)
- June 2024, Paper 3, Q10(a)(ii) (2 marks): Explain why Step 6 is carried out before the final sample is removed and titrated in Step 7. (2)
- June 2024, Paper 3, Q10(b)(i) (3 marks): Plot a graph of the Vfinal – Vt of sodium hydroxide against the time the reaction sample is added to the crushed ice. (3)
- June 2024, Paper 3, Q10(b)(ii) (2 marks): Explain why Vfinal – Vt is plotted rather than the concentration of sodium hydroxide solution for each titre. (2)
- June 2024, Paper 3, Q10(b)(iii) (2 marks): Determine two half-lives for the reaction, showing your working on the graph. (2)
- June 2024, Paper 3, Q10(b)(iv) (1 mark): Deduce the order of the reaction, using your answer from (b)(iii) to justify your deduction. (1)
- June 2024, Paper 3, Q10(c) (2 marks): Ethyl ethanoate can also be hydrolysed under alkaline conditions. A student researching the mechanism for the reaction found this example. O– O + OH– Step 1 O O
- June 2023, Paper 2, Q5(a)(i) (1 mark): Give a reason why this method can be used in this reaction. (1)
- June 2023, Paper 2, Q5(a)(ii) (1 mark): State two factors, other than initial amounts of reactants, that must be kept constant for this method to work. (1)
- June 2023, Paper 2, Q5(b)(i) (1 mark): Which line shows the relationship between the concentration of nitrogen monoxide (Y) and time (X)? (1) A line P B line Q C line R D line S
- June 2023, Paper 2, Q5(b)(ii) (1 mark): Which line shows the relationship between rate (Y) and concentration of oxygen (X)? (1) A line P B line Q C line R D line S
- June 2023, Paper 2, Q5(c) (1 mark): The rate of this reaction is z mol dm–3 s–1 under certain conditions. The concentration of nitrogen monoxide is doubled and the concentration of oxygen is halve
- June 2023, Paper 2, Q6(a)(i) (1 mark): State how the student could ensure that the concentrations of propanone and acid are effectively constant throughout the experiment. (1)
- June 2023, Paper 2, Q6(a)(ii) (2 marks): Explain why sodium hydrogencarbonate is added. (2)
- June 2023, Paper 2, Q6(b)(i) (1 mark): Give a reason why it is not necessary to calculate the concentration of iodine at each time to work out the order of reaction with respect to iodine. (1)
- June 2023, Paper 2, Q6(b)(ii) (2 marks): Plot a graph to show that the order of reaction with respect to iodine is zero. (2)
- June 2023, Paper 2, Q6(b)(iii) (1 mark): Give a reason why the graph shows that the order of reaction with respect to iodine is zero. (1)
- June 2023, Paper 2, Q6(c)(i) (2 marks): Deduce a possible rate determining step in the mechanism of this reaction. Curly arrows are not required. (2)
- June 2023, Paper 2, Q6(c)(ii) (1 mark): Data from two experiments carried out at the same temperature are shown. [H+(aq)] / mol dm–3 [I2(aq)] / mol dm–3 [CH3COCH3(aq)] / mol dm–3 Rate / mol dm–3 s–1 E
- June 2023, Paper 2, Q6(c)(iii) (2 marks): The experiment in (a) is repeated but using aqueous bromine instead of aqueous iodine. All other conditions are kept the same. Explain how you would expect the
- June 2023, Paper 3, Q8(a)(i) (2 marks): The iodine clock reaction with hydrogen peroxide involves the reaction shown. H2O2 + 2I– + 2H+ → I2 + 2H2O Deduce two possible experimental techniques which cou
- June 2023, Paper 3, Q8(a)(ii) (1 mark): The iodate(V) reaction has the rate determining step IO3 – + 3HSO3 – → I– + 3HSO4 – Give a possible reason why this is the slowest step. (1)
- June 2023, Paper 3, Q8(a)(iii) (1 mark): The chlorate(V) reaction has the rate determining step – + 2H+ + I– → HIO + HClO2 ClO3 Deduce the rate equation for this iodine clock reaction. (1)
- June 2023, Paper 3, Q8(c)(i) (3 marks): The rate constant, k, for the isomerisation of cyclopropane to propene was measured at various temperatures. The data obtained were used to draw the graph shown
- June 2023, Paper 3, Q8(c)(ii) (3 marks): At a temperature T, the fraction of molecules with energy equal to or greater than the activation energy is given by the expression − E a fraction of molecules
- June 2022, Paper 2, Q9(a) (1 mark): Write the rate equation for this reaction. (1)
- June 2022, Paper 2, Q9(b) (1 mark): Deduce the units of the rate constant given that the units of rate are mol dm–3 s–1. (1)
- June 2022, Paper 2, Q9(c) (2 marks): The table shows the concentration of ethanal in a sample at different times. Concentration of ethanal / mol dm–3 Time / s 0 0.72 420 0.36 1260 0.18 Calculate av
- June 2022, Paper 2, Q9(d) (2 marks): Explain why the data given and your answers in (c) show that the reaction is neither zero order nor first order. (2)
- June 2022, Paper 2, Q9(e) (7 marks): The rate constant for the reaction was determined at five temperatures. The results are given in the table. Temperature (T) 1/ Temperature (1/T) Rate constant (
- June 2022, Paper 3, Q10(a)(i) (2 marks): Explain why sodium hydrogencarbonate is added in Step 4. (2)
- June 2022, Paper 3, Q10(b)(i) (2 marks): Plot a graph of the volume of sodium thiosulfate against the time the sodium hydrogencarbonate is added. (2)
- June 2022, Paper 3, Q10(b)(ii) (3 marks): Explain how the graph of volume of thiosulfate against time confirms the reaction is zero order with respect to iodine, I2. (3)
- June 2022, Paper 3, Q10(c)(i) (2 marks): Predict which of the three steps is the rate‑determining step. Justify your answer. (2)
- June 2022, Paper 3, Q10(c)(ii) (2 marks): The student stated that ‘The hydrogen ions cannot be acting as a catalyst. One hydrogen ion is a reactant in Step 1 but two hydrogen ions are formed as products
- November 2021, Paper 2, Q6(c)(i) (1 mark): Complete the data in the table. (1)
- November 2021, Paper 2, Q6(c)(ii) (3 marks): Calculate the activation energy, Ea , for the reaction without plotting a graph. Include a sign and units in your answer. The Arrhenius equation may be written
- November 2021, Paper 2, Q6(d)(i) (1 mark): Deduce the order of reaction with respect to haemoglobin. (1)
- November 2021, Paper 2, Q6(d)(ii) (2 marks): Determine the order with respect to carbon monoxide using your answer to (d)(i) and the data in the table. Justify your answer. (2)
- November 2021, Paper 2, Q6(d)(iii) (1 mark): Write the rate equation for this reaction using your answers to (d)(i) and (d)(ii). (1)
- November 2021, Paper 2, Q6(d)(iv) (3 marks): Calculate the rate constant, k, for the reaction, using the data from Experiment 1 and the rate equation from (d)(iii). Include units in your answer. (3)
- November 2021, Paper 2, Q11(a) (2 marks): Plot a graph of the concentration of the hydroxide ions against time. (2)
- November 2021, Paper 2, Q11(b) (2 marks): State the order with respect to hydroxide ions. Justify your answer by reference to your graph in (a). (2)
- November 2021, Paper 2, Q11(c) (2 marks): Deduce the type of mechanism occurring. Justify your answer. (2)
- November 2021, Paper 2, Q11(d) (1 mark): Give the classification of the chloroalkane in this reaction. (1)
- October 2020, Paper 2, Q3(a)(ii) (1 mark): What is the overall order of this reaction? (1) A 3 B 6 C 12 D cannot tell from this information
- October 2020, Paper 2, Q6(b) (3 marks): Plot a graph of [RBr] against time. (3)
- October 2020, Paper 2, Q6(c) (2 marks): Explain how the graph shows that the reaction is first order with respect to RBr. Include the values of two consecutive half-lives. You must show your working
- October 2020, Paper 2, Q6(d)(i) (1 mark): Deduce the value of x in the rate equation. rate = k[RBr]1[OH−]x (1)
- October 2020, Paper 2, Q6(d)(ii) (3 marks): Give the mechanism for the reaction that is consistent with the orders of reaction with respect to R Br and hydroxide ions. Include curly arrows and relevant l
- October 2020, Paper 2, Q9(b) (5 marks): The rate constant for the decomposition of nitrogen(V) oxide was determined at two temperatures. Rate constant / s−1 Temperature / K 328 1.50 × 10−3 338 4.87 ×
- June 2019, Paper 2, Q7(b)(i) (2 marks): Complete the table by adding the missing values. [NO]/ moldm-3 [CL,] / moldm" Rate/moldm35' Experiment 1.09 × 102 0.122 0.241 1 8.72 × 10-2 0.482 2 4.91 × 102 0
- June 2019, Paper 2, Q7(b)(ii) (3 marks): Calculate the rate constant, k, using data from Experiment 1. Include units with your answer. (3)
- June 2019, Paper 2, Q7(b)(iii) (2 marks): Explain how using a catalyst increases the rate constant, k. (2)
- June 2019, Paper 2, Q8(b)(i) (1 mark): Complete the data in the table. (1)
- June 2019, Paper 2, Q8(b)(ii) (6 marks): Plot a graph and use it to determine the activation energy for the reaction in kJmol'. You should include the value and units of the gradient of the line. The A
- June 2019, Paper 3, Q6(c)(i) (2 marks): Plot a graph of partial pressure of ammonia against time. (2)
- June 2019, Paper 3, Q6(c)(ii) (2 marks): Deduce the rate equation for this reaction by using your graph in (c)(i). Justify your answer. (2)
- June 2019, Paper 3, Q6(c)(iii) (2 marks): Use the graph to calculate the rate constant. Include units in your answer. (2)
- June 2018, Paper 2, Q6(d) (6 marks): Compare and contrast the mechanism of hydrolysis, using aqueous potassium hydroxide, of the primary halogenoalkane, RCH2X, with that of the tertiary halogenoalk
- June 2018, Paper 2, Q9(a) (1 mark): State why the order of reaction with respect to iodide ions cannot be five, even though 5 mol of iodide ions are shown in the equation. (1)
- June 2018, Paper 2, Q9(b)(i) (1 mark): In experiment 6, the student forgot to add deionised water to keep the total volume the same for each experiment. State why the total volume should be kept the
- June 2018, Paper 2, Q9(b)(ii) (4 marks): Complete the table and use the results from experiments 1, 2, 3, 4 and 5 to plot a graph of 1000/t against volume of iodate(V) ions. (4)
- June 2018, Paper 2, Q9(b)(iii) (2 marks): Deduce the order of reaction with respect to the iodate(V) ions. Justify your answer. (2)
- June 2018, Paper 2, Q9(c)(i) (2 marks): In one experiment, the following data were obtained: Reactants Initial concentration / mol dm−3 H2O2(aq) 1.50 × 10−3 I−(aq) 2.10 × 10−3 H+(aq) 2.10 × 10−3 Initi
- June 2018, Paper 2, Q9(c)(ii) (2 marks): Explain the purpose of the starch present in the reaction mixture when starch is neither in the rate equation, nor in the reaction equation. (2)
- June 2018, Paper 2, Q9(d)(i) (3 marks): The Arrhenius equation can be expressed as 1 + E × ln k = − a constant R T From the gradient of the graph, determine the activation energy, Ea, for th
- June 2018, Paper 2, Q9(d)(ii) (1 mark): Give a reason for the point at ln k = −7 not being included in the line drawn on the graph. (1)
- June 2017, Paper 2, Q9(a) (1 mark): Compound A decomposes in a first order reaction. Calculate the time it takes for the mass of A to decrease from 600 g to 37.5 g if the decomposition has a const
- June 2017, Paper 2, Q9(b)(i) (3 marks): Calculate the orders with respect to X, Y and Z. (3) X Y Z
- June 2017, Paper 2, Q9(b)(ii) (4 marks): Give the rate equation for the reaction and hence calculate the rate constant, k, to an appropriate number of significant figures. Include units in your answer.
- June 2017, Paper 2, Q9(c)(i) (1 mark): What is the overall reaction order? (1) A First B Second C Third D Fourth
- June 2017, Paper 2, Q9(c)(ii) (2 marks): Calculate the concentration of bromide ions required to produce a reaction rate of 4.08 × 10−3 mol dm−3 s−1 at 298 K given that k = 8.00 dm9 mol−3 s−1 [BrO3 −]
- June 2017, Paper 2, Q9(d) (7 marks): The rate constant for the reaction between bromoethane and aqueous hydroxide ions was determined at five different temperatures. The results are given in the ta
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