$\definecolor{red}{RGB}{255,0,0}$$\definecolor{black}{RGB}{0,0,0}$
- $c_{A0}$
- $c_{A0}$
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- $c_{A0}$
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- $c_{B0}$
- $c_{B0}$
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- $c_{B0}$
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- $c_A$
- $c_A$
- $c_A$
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- $$\color{blue}{\rightarrow}\color{black}\;c_{A} \;= \;\frac{c_{B}\cdot c_{A0}}{c_{B0}}\cdot e^{k\cdot (c_{A0}-c_{B0})\cdot t}$$
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- $c_B$
- $c_B$
- $c_B$
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- $$\color{blue}{\rightarrow}\color{black}\;c_{B} \;= \;\frac{c_{A}\cdot c_{B0}}{c_{A0}}\cdot e^{-k\cdot (c_{A0}-c_{B0})\cdot t}$$
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- k
- k
- k
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- $$\color{blue}{\rightarrow}\color{black}\;k \;= \;-\frac{v}{ c_{A}\cdot c_{B}} $$
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- t
- t
- t
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- $$\color{blue}{\rightarrow}\color{black}\;t \;= \;\frac{1}{k\cdot (c_{A0}-c_{B0})}\cdot ln\frac{c_{A}\cdot c_{B0}}{c_{B}\cdot c_{A0}} $$
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- v
- v
- v
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- $$\color{blue}{\rightarrow}\color{black}\;v \;= \;k\cdot c_{A}\cdot c_{B} $$
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: Chemische Kinetik: Reaktionsgeschwindigkeit, Ordnung 2, zwei Reagentien
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