Table of Contents
- 1 How is activation energy related to rate of reaction?
- 2 What is the activated complex or transition state and how is it related to reaction rates?
- 3 Can the activated complex be the same as the reaction intermediate?
- 4 How does transition state theory describe activated complex and activation energy?
The activation energy of a chemical reaction is closely related to its rate. Specifically, the higher the activation energy, the slower the chemical reaction will be. The higher the barrier is, the fewer molecules that will have enough energy to make it over at any given moment.
What is the role of activated complex in a reaction?
An activated complex acts as an intermediary between the reactants and the products of the reaction. Not every collision is successful, that is, produces a chemical reaction. For a successful collision to occur, reactants require a minimum amount of energy, called the activation energy.
How is activation energy related to the activated complex of a reaction?
Activation energy is the minimum amount of energy that is needed to start a chemical reaction. Figure 12.4: The energy changes that take place during an exothermic reaction. The activation energy is the difference between the energy of the reactants and the maximum energy (i.e. the energy of the activated complex).
transition-state theory, also called activated-complex theory or theory of absolute reaction rates, treatment of chemical reactions and other processes that regards them as proceeding by a continuous change in the relative positions and potential energies of the constituent atoms and molecules. (See chemical kinetics.)
What happens during the brief existence of an activated complex?
When two reactant particles collide, they may form an activated complex. An activated complex is an unstable arrangement of atoms that forms for a moment at the peak of the activation-energy barrier. Its brief existence ends with the reformation of the reactants or with the formation of products.
What is an activated complex class 12?
An Activated Complex is a high energy state that a reaction goes through in order to change reactants to products.
Can the activated complex be the same as the reaction intermediate?
Essentially, an intermediate is a structure formed in the course of conversion of reactants to products. On the other hand, the activated complex is specifically the structure at the maximum energy point along the reaction path.
What is an activated complex quizlet?
Activated Complex. A short-lived, unstable arrangement of atoms that may break apart and re-form the reactants or may form products; also sometimes referred to as the transition state.
Is activation energy inversely proportional to rate of reaction?
The rate of reaction is directly proportional to the activation energy.
How does transition state theory describe activated complex and activation energy?
According to transition state theory, between the state in which molecules exist as reactants and the state in which they exist as products, there is an intermediate state known as the transition state. The species that forms during the transition state is a higher-energy species known as the activated complex.
What do you mean by activated complex?
An activated complex is an unstable arrangement of atoms that exists momentarily at the peak of the activation energy barrier. Because of its high energy, the activated complex exists for an extremely short period of time (about 10 −13 s).