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What is activation energy for a chemical reaction?

   What is activation energy for a chemical reaction?

Introductory Chemistry

Introductory Chemistry

Nivaldo J. Tro 5th Edition

Chapter 15, Problem 32

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Solved by Expert Lottie Adams

09/03/2020

Step 1

According to this theory, for a reaction to occur, it is not enough for reactant molecules to collide with each other. They must also possess a certain minimum amount of energy, known as the activation energy. Show more…

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What is activation energy for a chemical reaction?

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Key Concepts

Activation Energy

Activation energy is the minimum amount of energy required for reactant molecules to reach a state where they can successfully collide and convert into products. It represents the energy barrier that must be overcome for a chemical reaction to occur.

Transition State Theory

Transition state theory explains that reactant molecules go through a high-energy, unstable intermediate state known as the transition state or activated complex. The difference in energy between the reactants and this transition state is defined as the activation energy.

Arrhenius Equation

The Arrhenius equation quantitatively relates the rate constant of a chemical reaction to the activation energy and temperature. It shows how even small changes in activation energy or temperature can significantly affect the reaction rate, making it essential for understanding reaction kinetics.

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