Is a first order reaction always slower than a second order reaction

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SUMMARY

A first-order reaction is not always slower than a second-order reaction. The rate of a first-order reaction increases linearly with concentration, while the rate of a second-order reaction increases with the square of the concentration. This means that under certain conditions, particularly when both reactant concentrations are less than 1, a second-order reaction can yield a smaller rate than a first-order reaction. Understanding this relationship is crucial for applying collision theory effectively in chemical kinetics.

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lalaland432
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This is a concept question i was wondering.
in what instances would this be true and in what instances would this be false.
im in general chem 2.
 
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i no that when the reaction is of second order the rate is squared according to how much the factor of the reactant is increased by. The first order reaction increases by the same factor by how much the concentration increases by.
 
I guess the question wants you to think in terms of collision theory.
 
well, i played around with it and i know that this circumstance is true when both concentrations are less than 1.
a second reaction concentration squared of a fraction equals a smaller fraction. :/
 

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