0654.C6.2.05 — Describe collision theory in terms of: (a). number of particles per unit volume (b). frequency of collisions between particles (c). kinetic : past paper questions
Real questions on 0654.c6.2.05 — describe collision theory in terms of: (a). number of particles per unit volume (b). frequency of collisions between particles (c). kinetic
The newest 15 of 15 written questions. Open one to see it on the real paper.
- 0973/41 · May/June 2026 · Q7b[4]
The student uses dilute hydrochloric acid at a temperature of 50°C. The student measures the total loss in mass of the reaction mixture every 25 seconds for 150 seconds. Figure 7.1 shows a graph of the results. 1.10 1.00 0.90 aa 0.80 0.70 7 0.60 total loss in mass/g I 0.50 — 0.40 = 0.30 0.20 — 0.10 = 0.00 0 25 50 75 10...
See it on the paper → - 0973/41 · May/June 2026 · Q7c[2]
The student repeats the experiment using dilute hydrochloric acid at a temperature of 30°C. All other conditions remain the same. Describe how the shape of the graph in Figure 7.1 would be different at 30°C.
See it on the paper → - 0973/42 · May/June 2026 · Q7b(i)[1]
Identify which concentration of aqueous sodium thiosulfate gave the fastest reaction.
See it on the paper → - 0973/42 · May/June 2026 · Q7b(ii)[2]
Identify the least concentrated solution of aqueous sodium thiosulfate. Explain your answer.
See it on the paper → - 0973/42 · May/June 2026 · Q7d(ii)[3]
Explain your answer using collision theory.
See it on the paper → - 0973/41 · October/November 2025 · Q7b(iii)[2]
The reaction between dilute sulfuric acid and copper oxide is faster when more concentrated acid is used. Explain why, using collision theory.
See it on the paper → - 0973/42 · May/June 2024 · Q5b[3]
The students did the experiments at 20 °C. State how the rate of reaction will change if they do the experiments again at 40 °C. Explain your answer using ideas about collisions between particles.
See it on the paper → - 0973/42 · May/June 2024 · Q11b(ii)[2]
Fig. 11.2 shows the energy level diagram for the reaction to make sulfur trioxide. energy reactants products progress of reaction Fig. 11.2 Draw and label on Fig. 11.2: • the energy change in the reaction
See it on the paper → - 0973/41 · October/November 2022 · Q5c(i)[2]
Water reacts with magnesium metal. The reaction is very slow. The reaction is faster if hot water is used. Explain why. Use ideas about collisions between particles.
See it on the paper → - 0973/41 · October/November 2022 · Q5c(ii)[2]
The reaction between water and magnesium is faster if powdered magnesium is used instead of strips of magnesium. Explain why. Use ideas about collisions between particles.
See it on the paper → - 0973/42 · May/June 2022 · Q2b(ii)[2]
The rate of this reaction increases as the temperature inside the car engine increases. Explain why. Use ideas about collisions between particles.
See it on the paper → - 0973/42 · May/June 2022 · Q2b(iii)[2]
The rate of this reaction increases as the concentration of the oxygen gas increases. Explain why. Use ideas about collisions between particles.
See it on the paper → - 0973/41 · October/November 2020 · Q5b[3]
The reaction with warm acid is faster than the reaction with cold acid. Explain why reactions are faster at higher temperatures. Explain your answer in terms of collisions between particles.
See it on the paper → - 0973/41 · May/June 2019 · Q11a(ii)[3]
He carries out the experiment using dilute hydrochloric acid at 20 °C. He repeats the experiment at 30 °C. Fig. 11.2 shows his results. 100 80 Key volume of gas / cm 3 30 °C 20 °C 60 40 20 0 0 2 4 6 8 10 12 14 time / min 16 Fig. 11.2 State and explain the differences between the graphs in terms of the movement of react...
See it on the paper → - 0973/42 · May/June 2019 · Q11b(iii)[3]
State and explain why a low temperature is not used in stage 2. Explain your answer in terms of particle movement in stage 2.
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What examiners said
Explanations of the dependence of reaction rate on temperature usually referred correctly to the kinetic energy of particles and the rate of collision. Full credit was obtained by recognising the important fact that, at higher temperature, more colliding particles possess the minimum energy or activation energy to react, rather than making vague reference to the number of successful collisions.
— Examiner report, October/November 2020, 0973/41 Q5(b) (Cambridge)
Many candidates were aware that the rate of reaction was greater at higher temperature. They may have found the explanation more straightforward had they concentrated on the initial rate. Good responses went on to identify the cause as increased rate of collision of particles and that more collisions would be successful. A few candidates explained that more particles would have the activation ener...
— Examiner report, May/June 2019, 0973/41 Q11(a)(ii) (Cambridge)
Many candidates referred to less kinetic energy of the particles. Some candidates described this as decreasing the number of collisions rather than referring to collision frequency. The stronger candidates linked this with a decreased rate of reaction.
— Examiner report, May/June 2019, 0973/42 Q11(b)(iii) (Cambridge)
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