Integrated Rate Law for 2nd Order Reactions

AI Thread Summary
The discussion centers on the definition and formulation of the rate law for second-order reactions in kinetics. It questions why the rate is not expressed as rate = -1/2(d[1]/dt) and why stoichiometric coefficients are often ignored in this context. The rate of reaction is typically defined as (1/a)*d[A]/dt, where 'a' represents the stoichiometric coefficient, which can vary depending on the reaction equation. The conversation emphasizes the importance of discussing the rate of change of concentration for specific reactants, highlighting that the formulation can differ based on the reaction's stoichiometry, such as in the examples of A → ½B or 4A → 2B.
samy4408
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hello i have a question about kinetics : to have the integrated rate law for second order reaction the professor write the following
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why we don't write the rate like this : rate = -1/2(d[1]/dt) ?
why we ignore the stoichiometric coefficient ?
 
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Rate is defined as a speed of change of the concentration, period.
 
"Rate of reaction" is often defined as (1/a)*d[A]/dt, where a is the stoichiometric coefficient of A (negative for reactants, positive for products). Then it's the same whichever reagent you look at, but it depends how you write the equation, e.g. it would be different for A → ½B or 4A → 2B. My preference is always to talk in terms of the rate of change of concentration of a specified reagent.
 
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