A gaseous reaction is carried out at two different temperatures. The amounts of reactants and the volume of the reaction vessel are the same in both experiments.
The table shows data for the collisions between reacting particles.
| Temperature in ∘C^\circ\text{C}∘C | Total number of collisions per second | Collisions with at least the activation energy in % |
|---|---|---|
| 25 | 6.0 × 1020 | 0.25 |
| 45 | 6.2 × 1020 | 1.0 |
Calculate the number of successful collisions per second at each temperature.
Explain why the reaction is faster at 45 ∘C45\ ^\circ\text{C}45 ∘C.
Use the data, and use your answers to part (a) to calculate how many times faster the reaction is at 45 ∘C45\ ^\circ\text{C}45 ∘C.
127 exam-style questions on AQA GCSE Chemistry 6.1 Rate of reaction, covering 6.1.1a Calculating rates of reactions, 6.1.1b Gradient of a tangent as rate, 6.1.2 Factors which affect the rates of chemical reactions, 6.1.3 Collision theory and activation energy, and 6.1.4 Catalysts. Each one has a worked solution and a mark scheme showing where the marks go.