The relationship between reaction rate and activation energy
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According to physical chemistry, the reaction rate is related to temperature, the concentration of reactants, and the properties of the reaction itself. I suddenly thought of a question: what is the relationship between reaction rate and activation energy?
The lower the activation energy of a reaction, the greater the number of activated molecules at a given temperature, and the faster the reaction proceeds.
There should be no connection at all; activation energy is a thermodynamic concept, representing the minimum amount of energy required for a substance to undergo a change or reaction, while reaction rate is a kinetic concept.
The activation energy should be inversely proportional to the reaction rate; the function of a catalyst is to reduce the activation energy and thereby facilitate the reaction
The basic formula is: r=k0*e(-E/RT)*C^n, where E is the activation energy, which is somewhat related to it!
Ea is the activation energy; the higher Ea, the greater the difficulty of carrying out the reaction. You can think of it as the peak of a Gaussian function – the higher the peak, the greater the difficulty