A reaction takes place in three steps- The rate constant are k1- k2- and k3- The overall rate constant k - k1k3-k2- If E1- E2 and E3 energy of activation are 60- 30 and 10 kJ- respectively- the overall energy of activation is-

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Standard XII

Chemistry

Arrhenius Equation

A reaction ta...

Question

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

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400

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Solution

The correct option is A 40
$k_{1} = A e^{- E_{a} / R T}$
$k_{2} = A e^{- E_{a} / R T}$
$k_{3} = A e^{- E_{a} / R T}$
Overall rate :
$k = \frac{k_{1} k_{3}}{k_{2}}$
$∴ O v e r a l l E_{a} = E_{a_{1}} = E_{a_{3}} + E_{a_{2}}$
= 60 + 10 - 30
= 40 kJ

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A reaction takes place in three steps. The rate constant of the three steps are $k_{1}, k_{2}$ and $k_{3}$ respectively. The overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}} .$ The energy of activation for the three steps are 40, 30 and 20 kJ respectively. Therefore: