define ‘chemical kinetics’; *9.2 Rate and Order of Reaction 9.2.1 define the terms:a. rate of reactionb. rate lawc. order of reactiond. rate constante. rate determining step;*9.2.2 explain the significance of the rate determining step on theoverall rate of a multistep reaction;*9.2.3 determine the rate law for the given reactions; *9.2.4 deduce the order of reaction using the method of initial rate; *9.3 Collision Theory, Transition Stateand Activation Energy9.3.1 relate activation energy and activated complex to the rate ofreaction;*9.3.2 calculate the initial rate using concentration data of givenreactions;*9.3.3 draw a labelled energy diagram for a chemical reactionrepresenting the activation energy and the effect of catalyst;*9.3.4 describe collision theory; *9.3.5 explain the effect of concentration, temperature and surfacearea on rate of reaction by using collision theory;*9.4 Catalysis 9.4.1 define the term ‘catalyst’; *9.4.2 explain homogeneous and heterogeneous catalysis; *9.4.3 explain the effect of catalyst on the rate of reaction. *

Sure, here are the definitions and explanations for the terms and concepts you've listed:

1. Chemical kinetics: This is the study of rates of chemical processes.

2. Rate of reaction: This is the speed at which reactants are converted into products in a chemical reaction.

3. Rate law: This is an equation that links the reaction rate with concentrations or pressures of reactants and constant parameters.

4. Order of reaction: This refers to the power dependence of the rate on the concentration of each reactant.

5. Rate constant: This is a proportionality constant in the rate law, which is specific for a given reaction at a particular temperature.

6. Rate determining step: This is the slowest step in a reaction mechanism, which determines the overall rate of the reaction.

7. The rate determining step affects the overall rate of a multistep reaction because it is the slowest and thus limits the rate at which the reaction can proceed.

8. The rate law for a given reaction can be determined experimentally through a series of experiments.

9. The order of reaction can be deduced using the method of initial rates, by observing how the rate changes with changes in concentration.

10. Activation energy is the minimum energy required for a reaction to occur. The activated complex is the structure at the maximum energy point along the reaction path.

11. The initial rate can be calculated using concentration data of the given reactions.

12. An energy diagram for a chemical reaction represents the activation energy and the effect of a catalyst.

13. Collision theory describes how reactions occur and why reaction rates differ for different reactions.

14. The rate of reaction can be affected by concentration, temperature and surface area. Increasing these factors increases the rate of reaction.

15. A catalyst is a substance that increases the rate of a chemical reaction by lowering the activation energy.

16. Homogeneous catalysis refers to the process where the catalyst and the reactants are in the same phase, while heterogeneous catalysis refers to the process where the catalyst and the reactants are in different phases.

17. A catalyst increases the rate of reaction by providing an alternative reaction pathway with a lower activation energy.

Sure, I can do that. Here are the definitions and explanations for the terms and concepts you've asked about:

1. Chemical kinetics: This is the study of rates of chemical processes.

2. Rate of reaction: This is the speed at which reactants are converted into products in a chemical reaction.

3. Rate law: This is an equation that links the rate of a reaction to the concentrations of the reactants.

4. Order of reaction: This refers to the power dependence of the rate on the concentration of each reactant.

5. Rate constant: This is a proportionality constant in the rate law, which is specific for a particular reaction at a particular temperature.

6. Rate determining step: This is the slowest step in a reaction mechanism, which determines the overall rate of the reaction.

7. The rate determining step is significant because it controls the rate of the reaction. If this step is slow, the overall