C18 Rates of reaction

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Across
  1. 8. A chemical technique used to determine the concentration of a reactant at set time intervals during an experiment (9)
  2. 9. Increasing this property of a solid reactant increases the frequency of collisions (7, 4)
  3. 13. The power to which a reactant's concentration is raised in the rate equation (5)
  4. 14. The slowest step in a reaction mechanism, which dictates the overall rate of reaction (4, 11, 4)
  5. 15. An experimental method where the time taken for a sudden, visible change (such as a colour change) is measured to find the initial rate (5, 8)
  6. 16. A mathematical expression showing how the rate of reaction depends on the concentration of reactants (4, 8)
  7. 18. The equation that links the rate constant with activation energy and temperature (9, 8)
  8. 19. The minimum energy that colliding particles must possess for a reaction to occur (10, 6)
  9. 21. An experimental method used to follow a reaction by measuring light absorbed by a coloured solution (11)
  10. 22. A straight line drawn touching a concentration–time curve at a specific point to calculate the rate at that moment (7)
  11. 24. Theory stating that reactions only occur when particles collide with sufficient energy and the correct orientation (9, 6)
  12. 25. The change in concentration of a reactant or product per unit time (4, 2, 8)
  13. 28. Increasing this factor increases the kinetic energy of particles and shifts the Boltzmann peak to the right (11)
  14. 29. A reaction order where doubling the concentration of a reactant causes the rate to quadruple (6, 5)
  15. 30. Type of catalyst that is in a different physical state from the reactants (13)
Down
  1. 1. Type of catalyst that is in the same physical state as the reactants (11)
  2. 2. The gradient of a tangent drawn to a concentration–time graph at t = 0 (7, 4)
  3. 3. A reaction order where the rate is directly proportional to the concentration of a reactant (5, 5)
  4. 4. The proportionality constant in a rate equation, which increases with temperature (4, 8)
  5. 5. The graph showing the spread of molecular energies in a gas at a given temperature (9, 12)
  6. 6. Term used to describe a reactant whose concentration has no effect on the rate of reaction (4, 5)
  7. 7. The time taken for the concentration of a reactant to reduce by half (4, 4)
  8. 10. The sequence of bond-breaking and bond-making steps that shows how reactants are converted into products (8, 9)
  9. 11. A term in the Arrhenius equation representing the frequency of collisions with the correct orientation (14, 6)
  10. 12. The sum of all the individual orders in a rate equation (7, 5)
  11. 17. A species formed during one step of a reaction mechanism and consumed in a subsequent step (12)
  12. 20. A substance that increases the rate of a chemical reaction without being used up in the overall process (8)
  13. 23. Increasing the amount of solute per unit volume of solution, which increases the frequency of collisions (13)
  14. 26. The steepness of a line or tangent on a graph, used to determine the rate of reaction (8)
  15. 27. Increasing this factor in gases forces particles closer together, increasing collision frequency (8)