deletions | additions       diff --git a/Pseudo-First Order Reactions.tex b/Pseudo-First Order Reactions.tex  index 324abf9..a3cd1ff 100644  --- a/Pseudo-First Order Reactions.tex  +++ b/Pseudo-First Order Reactions.tex 
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In practice, second order reactions can be difficult to analyze because it can be difficult to precisely measure the concentration of two reactants at the same time. Pseudo first Second  order kinetics can easily  be used to accommodate this issue by 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, which gives giving  details about the reaction's mechanism. In essence, the isolation method can simply turn 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}