The addition of a catalyst to a system at equilibrium decreases the activation energy.
What is a catalyst?
A molecule or element that accelerates a chemical process without itself being a product of the reaction is known as a catalyst. In general, a catalyst is not damaged or altered throughout the reaction.
What is activation energy?
Activation energy is the least amount of energy necessary to activate atoms or molecules so they can go through a chemical reaction.
Effect of catalyst on activation energy
- In order to speed up a reaction, a catalyst lowers its activation energy. A reaction requires less energy to initiate when the activation energy is lower.
- The reaction's transition state is altered by a catalyst, lowering the activation energy.
- After then, the reaction follows a different mechanism/pathway than the uncatalyzed process.
- The net energy difference between reactant and product is unaffected by the catalyst.
- Even though the transition state varies between a catalyzed and an uncatalyzed process, the net equation will remain the same in both cases.
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