Which of the following statements is true regarding activation energy?a)It is the energy required for a reaction to proceed.b)It determines the overall energy change of a reaction.c)It remains constant for all chemical reactions.d)It depends on the concentration of reactants.Correct answer is option 'A'. Can you explain this answer?

Question

Answer

Activation energy is the minimum amount of energy required for a chemical reaction to occur. It represents the energy barrier that reactant molecules must overcome to transform into products. Activation energy is specific to each reaction and depends on the nature of the reactants and the reaction pathway.

Answer

Statement: Activation energy is the energy required for a reaction to proceed.

Explanation:
Activation energy is a fundamental concept in chemistry that refers to the minimum amount of energy required to start a chemical reaction. It is represented by the symbol Ea.

Key Points:

1. Definition: Activation energy is the energy required for a reaction to proceed, specifically the energy needed to break the bonds in the reactant molecules.
2. Barrier: Activation energy acts as a barrier that reactant molecules must overcome in order to transform into product molecules.
3. Transition State: During a chemical reaction, reactant molecules transition into an intermediate state called the transition state, which has higher energy than both the reactants and products. The activation energy is the energy difference between the reactants and the transition state.
4. Reaction Rate: The magnitude of the activation energy determines the rate at which a reaction occurs. Reactions with higher activation energies generally proceed slower compared to reactions with lower activation energies.
5. Temperature Dependence: Increasing the temperature generally increases the reaction rate because it provides the reactant molecules with more kinetic energy, allowing them to overcome the activation energy barrier more easily.
6. Catalysts: Catalysts are substances that can lower the activation energy of a reaction, thereby increasing the reaction rate. They achieve this by providing an alternative reaction pathway with a lower activation energy.
7. Variability: Activation energy varies from reaction to reaction and depends on factors such as the nature of the reactants, the reaction mechanism, and the reaction conditions.

Conclusion:
In summary, activation energy is the energy required for a reaction to proceed. It acts as a barrier that reactant molecules must overcome, and its magnitude determines the rate of the reaction. Activation energy varies depending on the specific reaction and is influenced by factors such as temperature and the presence of catalysts.

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