Second Order Reactions

[Johnathan Smith 1D]

What determines a reaction as a second order reaction and not as a first order reaction?

[Alice Chang 2H]

In a first order reaction, there will be one reactant present in the rate law. For a second order reaction, you can either have a rate law with one reactant to the second order, or with two reactants both to the first order.

Found this answer (and others) here: https://lavelle.chem.ucla.edu/forum/viewtopic.php?t=28639

[Maia_Jackson_2C]

I think there would just be two reactants, so it would be bimolecular.

[KarineKim2L]

One way is to graph the reaction and see which equation results in a linear graph. A linear graph that plots [R] to time is zero order, ln[R] to time is first order, and 1/[R] to time is second order.

[Kaylee Sepulveda 4G]

A second-order reaction (where order = 2) has a rate proportional to the concentration of the square of a single reactant or the product of the concentration of two reactants. The formula is:

rate = k[A]² (or substitute B for A or k multiplied by the concentration of A times the concentration of B), with the units of the rate constant M^-1sec^-1

For a first order reaction, the rate law would be = k[A] (or B instead of A), with k having the units of sec^-1

[Nathan Rothschild_2D]

Where in the book can we find examples of first and second order reactions?