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Jason R. Green edited Nonlinear irreversible kinetics.tex
over 9 years ago
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\begin{equation}
\frac{dC_i(t)}{dt} = k_i(t)\left[C_i(t)\right]^i.
\end{equation}
Experimental data is typically a concentration profile corresponding to the integrated form of the rate law.
For example, in Normalizing the
case of the $i^{th}$-order reaction, concentration profile, by comparing the
traditional integrated rate law and concentration at a
rate ``constant'', $k_i(t)\to\omega$, is time $t$ to the initial concentration, leads to the survival function
\begin{equation}
\frac{1}{C_i(t)^{i-1}} = \frac{1}{C_i(0)^{i-1}}+(i-1)\omega t.
\end{equation}
Normalizing the concentration profile, by comparing the concentration at a time $t$ to the initial concentration, leads to the survival function
\begin{equation} S_i(t) =
\frac{C_i(t)}{C_i(0)} = \sqrt[i-1]{\frac{1}{1+(i-1)\omega tC_i(0)^{i-1}}}, \frac{C_i(t)}{C_i(0)},
\end{equation}
which we will use as the input to our theory. Namely, we define the effective rate coefficient, $k_i(t)$, through an appropriate time derivative of the survival function that depends on the order $i$ of reaction
\begin{equation}
...
\displaystyle +\frac{d}{dt}\frac{1}{S_i(t)^{i-1}} & \text{if } i \geq 2.
\end{cases}
\end{equation}
For example, in the case of the $i^{th}$-order reaction, the traditional integrated rate law and a rate ``constant'', $k_i(t)\to\omega$, is
\begin{equation}
\frac{1}{C_i(t)^{i-1}} = \frac{1}{C_i(0)^{i-1}}+(i-1)\omega t.
\end{equation}
Normalizing the concentration profile, by comparing the concentration at a time $t$ to the initial concentration, leads to the survival function
\begin{equation}
S_i(t) = \sqrt[i-1]{\frac{1}{1+(i-1)\omega tC_i(0)^{i-1}}},
\end{equation}
In traditional kinetics, the rate coefficient of irreversible decay is assumed constant, in which case $k(t)\to\omega$. However, this will not be the case when the kinetics are statically or dynamically disordered. In these cases, we will use the above definitions of $k(t)$.