Chemical Kinetics

2. A reaction intermediate is a compound _______ in one step and consumed in another
3. A very exothermic reaction may be slow because it has a ______ activation energy
6. Rate of reaction is expressed as ___________ over time
13. When __________ increases, particles move faster and with more energy ∴ speeding up the reaction rate
14. In a potential energy diagram, activation energy is represented by a _____
15. The minimum potential energy that particles have to collide with before they react
17. The rate of the reaction can be affected differently by each _______
21. The ________ mechanism determines the overall rate of the reaction
22. When the concentration of a reactant is doubled, and it is a 2nd order reaction, the reaction rate will _____
23. The slow step mechanism has the _____ order
25. Decreasing surface area will _______ the rate of the reaction
26. If particles do not collide in the correct __________ the reaction will not occur
27. The ________________ is a high energy state between reactants and products
29. A heterogeneous catalyst is where the catalyst and reactants are in _______ states
30. In terms of molecularity, a mechanism with 3 reacting molecules is called __________

1. Activation energy can be determined by the______
4. Step-by-step sequence of elementary reactions by which an overall chemical change occurs
5. A reaction involving two reactant molecules is ________
7. Reactions often don’t occur in the __________ indicated by the chemical equation
8. The time required for half of a sample to decay
9. In the equation r=K[X]ˢ[Y]ⁿ, k represents a ________
10. The difference in potential energy between products and reactants is _____
11. A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation
12. On a maxwell-boltzmann distribution graph, adding a catalyst makes the activation energy move _______
16. A negative sign indicates the rate of _________ of a reactant
18. Adding a _____ to a reaction ∴ speeds up the reaction rate
19. Chemical kinetics is used to determine ways to control the______ of a reaction
20. A reaction whose rate is independent of the concentration of the reactant(s)
24. the sum of the exponents in the rate law equation
28. 1st order reactions occur in both chemical and _____ changes