deletions | additions       diff --git a/Pseudo-First Order Reactions.tex b/Pseudo-First Order Reactions.tex  index 9366a3d..cb5c71f 100644  --- a/Pseudo-First Order Reactions.tex  +++ b/Pseudo-First Order Reactions.tex 
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Second order kinetics can easily be simplified using the isolation method.[cite] The isolation method involves an using excess of one reactant and reacting it with a much smaller amount of a second reactant. While the excess reactant's concentration essentially remains constant over time, the other reactant's concentration varies at a measurable rate over time, allowing the order of that reactant to be determined, giving details about the reaction's mechanism. In essence, the isolation methodcan  simply turn turns  a second order reaction into a first order reaction, or vice versa. The rate law of a second order irreversible decay reaction between A and B, where the reaction is first order in both A and B, decaying into products is \begin{equation}  \frac{-d[A]}{dt}=\omega{[A][B]}  \end{equation}