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Michael edited 2.tex
almost 9 years ago
Commit id: a9b081dfb535c44b155bbab2d849ee362ed4d0e8
deletions | additions
diff --git a/2.tex b/2.tex
index d3342fd..b4c4cad 100644
--- a/2.tex
+++ b/2.tex
...
-\frac{d[A]}{dt}=k_{1}[A]-k_{-1}[B]
\end{equation}
\begin{equation}
\frac{d[B]}{dt} = k_1[A]-k_{-1}[B]-k_2[B]+k_{-2}[C]
\end{equation}
\begin{equation}
\frac{d[C]}{dt} = k_2[B]-k_{-2}[C]
\end{equation}
Note that, for the purposes of this work, the conversion of isomer C to A is ignored. This is a valid assumption if the rate of inter-conversion of \textit{ A } $\longleftrightarrow$ \textit{ C } is small.
Given the experimental data, a steady-state approximation for the system of rate equations is not valid for isomer \textit{B} because its concentration is rather close to those of \textit{A} and \textit{C} and changes appreciably. Thus, the differential equations in (2)-(4) must be solved explicitly. The exact solutions to these equations are:
\begin{equation}
A(t)
&= = A_0[\frac{k_{-1}k_{-2}}{mn}+\frac{k_1(m-k_2-k_{-2})}{m(m-n)}*\mathrm{e}^{-mt}+\frac{k_1(k_2+k_{-2}-n)}{n(m-n)}*\mathrm{e}^{-nt}]
\\ \end{equation}
\begin{equation}
B(t)
&= = A_0[\frac{k_{1}k_{-2}}{mn}+\frac{k_1(k_{-2}-m)}{m(m-n)}*\mathrm{e}^{-mt}+\frac{k_1(n-k_{-2})}{n(m-n)}*\mathrm{e}^{-nt}]
\\ \end{equation}
\begin{equation}
C(t)
&= = A_0[\frac{k_{1}k_{2}}{mn}+\frac{k_1k_{2}}{m(m-n)}*\mathrm{e}^{-mt}-\frac{k_1k_{2}}{n(m-n)}*\mathrm{e}^{-nt}]
\end{equation}
Where,
\begin{equation}