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

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