A reaction takes place in three steps. The rate constants are k1,k2 and k3. The overall rate constant k=k1k3k2. If (energy of activation) E1,E2 and E3 are 60, 30 and 10 kJ. The overall energy of activation is :

K=Ae−Ea/RT ∴ Ae−Ea/RT=Ae-E1-E3+E2RTEa=E1+E3−E2=60+10−30=40 kJ

A reaction takes place in three steps. The rate constants are k1,k2 and k3. The overall rate constant k=k1k3k2. If (energy of activation) E1,E2 and E3 are 60, 30 and 10 kJ. The overall energy of activation is :

K=Ae−Ea/RT ∴ Ae−Ea/RT=Ae-E1-E3+E2RTEa=E1+E3−E2=60+10−30=40 kJ

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A reaction takes place in three steps. The rate constants are $k_{1}, k_{2} and k_{3}$ . The overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}}$ . If (energy of activation) $E_{1}, E_{2} and E_{3}$ are 60, 30 and 10 kJ. The overall energy of activation is :

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$\begin{array}{l} K = {Ae}^{- Ea / RT} ∴ {Ae}^{- E_{a} / RT} = {Ae}^{\frac{- E_{1} - E_{3} + E_{2}}{RT}} \\ E_{a} = E_{1} + E_{3} - E_{2} = 60 + 10 - 30 = 40 kJ \end{array}$

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A reaction takes place in three steps. The rate constants are k1,k2 and k3. The overall rate constant k=k1k3k2. If (energy of activation) E1,E2 and E3 are 60, 30 and 10 kJ. The overall energy of activation is :

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A reaction takes place in three steps. The rate constants are $k_{1}, k_{2} and k_{3}$ . The overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}}$ . If (energy of activation) $E_{1}, E_{2} and E_{3}$ are 60, 30 and 10 kJ. The overall energy of activation is :