Activation energy is often studied under physical chemistry and it is a very important concept related to chemical kinetics in JEE. The term Activation Energy was first used by a Swedish scientist named Svante Arrhenius in the year 1889. Today, we learn about this concept as it helps us understand the energy requirements for a chemical reaction which further gives us control over our actions and the environment.
Almost all the chemical reactions require some activation energy to go forward. Therefore, it is important for students to know what is activation energy. We shall learn more about this concept in this lesson.
Table of Content
- Activation Energy Definition
- Factors Affecting Activation Energy
- Activation Energy Examples
- Activated Complex
- Activation Energy Formula
Activation Energy Definition
Activation energy is defined as the minimum amount of extra energy required by a reacting molecule to get converted into product. It can also be described as the minimum amount of energy needed to activate or energize molecules or atoms so that they can undergo a chemical reaction or transformation.
What is the SI Unit of Activation Energy?
Factors Affecting Activation Energy
Activation energy depends on two factors.
1. Nature of Reactants
In the case of ionic reactant, the value of (Ea) will be low because there is an attraction between reacting species. While in the case of covalent reactant the value of Ea will be high because energy is required to break the older bonds.
Also Read: Chemical Kinetics
2. Effect of Catalyst
Positive catalyst provides such an alternate path in which the value of Ea will be low, while the negative catalyst provides such an alternate path in which the value of Ea will be high.
Activation Energy Examples
Activation energy for Forward reaction (Ea)f
Activation energy for Forward reaction (Ea)b
(Ea)f < (Ea)b
(ROR)f > (ROR)b
△H = (Ea)f – (Ea)b
△H = -ve value
(Ea)f = △H Only one can be possible for Exothermic Reaction
(Ea)f > △H
(Ea)f < △H
(Ea)f > (Ea)b
(ROR)f < (ROR)b
△H = (Ea)b – (Ea)f
△H = +ve value
(Ea)f > △H (Always )…………universal
A catalyst is a chemical substance that either increases or decreases the rate of a chemical reaction. In the case of activation energy, a catalyst lowers it. However, the energies of the original reactants remain the same. A catalyst only alters the activation energy.
Types of Catalysts
A catalyst which helps to increase the rate of reaction or which support the reaction to carry out quicky is called a positive catalyst. Such catalyst decreases activation energy by accepting a smaller path, so the rate of reaction is increased.
Negative Catalysts (Inhibitors)
A catalyst which decreases or retards or helps in slowing down the rate of reaction is called negative catalysts.
It is because a negative catalyst increases activation energy by taking a longer alternative path.
Points to Remember
Forward Reaction: Those reactions in which the product formed are produced from reactants
When reactant molecules collide with each other at it’s highest energy point, an intermediate is formed which remains in equilibrium with the main reactant. If this intermediate complex has energy equal to or greater than the Threshold Energy then it will be converted into product.
Activation Energy Formula
The formula used to find the value of Activation Energy, Ea is;
K = Ae-Ea/RT
K = Rate Constant
A = Arrhenius Constant
Ea = Activation Energy
R = Gas constant = 8.34J/K/mol
= 2 cal/K/mol
= 0.0821 lit atm/K/mol
K = Ae-Ea/RT
Taking log on both sides
ln K = ln A – (Ea /RT)ln e
2.303 log K = 2.303 log A – Ea/RT
log K = log A – Ea /2.303RT