$\definecolor{red}{RGB}{255,0,0}$$\definecolor{black}{RGB}{0,0,0}$
- $c_{A0}$
- $c_{A0}$
- $c_{A0}$
-
- $$\color{blue}{\rightarrow}\color{black}\;c_{A0} \;= \;\frac{c_{A}}{1-c_{A}\cdot k\cdot t}$$
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- $c_A$
- $c_A$
- $c_A$
-
- $$\color{blue}{\rightarrow}\color{black}\;c_{A} \;= \;\frac{c_{A0}}{1+c_{A0}\cdot k\cdot t}$$
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- t
- t
- t
-
- $$\color{blue}{\rightarrow}\color{black}\;t \;= \;\frac{c_{A0}-c_{A}}{k\cdot c_{A}\cdot c_{A0}} $$
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- k
- k
- k
-
- $$\color{blue}{\rightarrow}\color{black}\;k \;= \;\frac{c_{A0}-c_{A}}{t\cdot c_{A}\cdot c_{A0}} $$
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- $t_{\frac{1}{2}}$
- $t_{\frac{1}{2}}$
- $t_{\frac{1}{2}}$
-
- $$\color{blue}{\rightarrow}\color{black}\;t_{\frac{1}{2}} \;= \;\frac{1}{k\cdot c_{A0}} $$
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- v
- v
- v
-
- $$\color{blue}{\rightarrow}\color{black}\;v \;= \;k\cdot c_{A}^2 $$
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: Chemische Kinetik: Reaktionsgeschwindigkeit, Ordnung 2, ein Reagens
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