Hi, I would appreciate it if you could explain to me which equation is correct for the second-order reaction. In the most textbooks I see "K" instead of "2K" in the equation. Please also see the attached pictures.
Regards,
Both are correct, just different meaning of k. Since two molecules of A are consumed, A + A -> Products, the reaction rate constant is commonly defined as 2k.
Both are correct, One is written based on the rate of consumption of reactants or formation of products, but the other is written based on the rate of reaction. indeed, the relationship between the rate constants depends on the stoichiometry.
Both are correct, that's just the way the equation would be written.
good luck
As mentioned by others, both are correct. In this case values of "k" will be different and the second one will be 2 times higher as the stoichiometric coefficient is hidden inside of k. Substance A at the same time is of 2nd order in this equation and two molecules are used in single reaction - elementary reaction. I would say that the first one is more transparent. The most common and easy to understand form of this equation would be (d[A]/dt)=-2k[A]^2
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