How does the PE of the activated complex compare to that of the reactants?

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The potential energy (PE) of the activated complex is higher than that of the reactants, as the activated complex requires additional energy to be formed. This higher activation energy is necessary for the reaction to proceed, influencing whether the reaction is exothermic or endothermic. An exothermic reaction occurs when the PE of the reactants is greater than that of the products, while an endothermic reaction has the opposite relationship. Some participants mistakenly connect activation energy directly to thermicity, which is not accurate. Understanding the relationship between activation energy and potential energy is crucial for grasping reaction dynamics.
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"How does the PE of the activated complex compare to that of the reactants?"
anyone know~~~ ><
pleasez~~~ thankyou in advance! :wink:
 
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What do you think ? What does the verb 'activate' suggest to you ?

Also, what do you know about the stability of an activated complex, and how is stability related to PE ?
 
the PE is higher than the reactants. The activated complex needs more energy in order to be 'activated'.
 
more activation energy yields an exothermic reaction while the less act. energy gives you the endothermic reaction.
 
1+1=1, I think u mean the more potential energy in the reactants than in the products yields an exothermic reaction and vice versa. Activation energy is always more than potential energy of reactants. If it wasnt, the reaction would just go on spontainouesly and never stop.
 
1+1=1 said:
more activation energy yields an exothermic reaction while the less act. energy gives you the endothermic reaction.

Not true. Thermicity has nothing to do with Activation Energy.
 
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