A reaction takes place in three steps- The rate constants are k1- k2 and k3- The over all rate constant k - k1k3k2- If energy of activation E1- E2 and E3 are 60- 30 and 10 kJ- the overall energy of activation is-

The correct option is B 40 k=Ae^ E_aRT ∴ k=k_1k_2k_2=A_1A_3A_2× e^ E_a^(1)+E_a^(3) E_a^(2)RT E_a=E_a^(1)+E_a^(3) E_a^(2) =40KJ ...

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Byju's Answer

Standard XII

Chemistry

Activation Energy

A reaction ta...

Question

A reaction takes place in three steps. The rate constants are $k_{1}, k_{2}$ and $k_{3}$ . The over all 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 $10 k J$ , the overall energy of activation is:

40

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30

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400

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60

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Solution

The correct option is B $40$
$k = A e^{- \frac{E_{a}}{R T}}$
$∴ k = \frac{k_{1} k_{2}}{k_{2}} = \frac{A_{1} A_{3}}{A_{2}} \times e^{- \frac{E_{a}^{(1)} + E_{a}^{(3)} - E_{a}^{(2)}}{R T}}$
$E_{a} = E_{a}^{(1)} + E_{a}^{(3)} - E_{a}^{(2)}$
$= 40 K J$

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(energy of activation) are 60, 30 and 10 kJ, respectively, the overall energy of activation is:

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: