A reaction takes place in three steps- The rate constant of the three steps are k1- k2 and k3 respectively- The overall rate constant k-k1 k3-k2- The energy of activation for the three steps are 40- 30 and 20 kJ respectively- Therefore-

Since, overall rate constant k=k_1 k_3/k_2 So, total energy of activation is Ea_1+Ea_3 Ea_2 ⇒ 40+20 30=30 kJ 2A ^∗A^∗+A; A^∗ Product This satisfied the conditio ...

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Standard XII

Chemistry

First Order Reaction

A reaction ta...

Question

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:

Overall energy of activation is 10 kJ.

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Overall energy of activation is 30 kJ.

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The reaction mechanism is $2 A \frac{k_{1}}{k_{2}} A^{*} + A; A^{*} k_{3} - - \to r d s$ Product and overall order is one.

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The reaction mechanism is $A k_{1} - \to B; B k_{2} - \to C; C k_{3} - \to$ Product and overall order is one.

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Solution

The correct option is C
The reaction mechanism is $2 A \frac{k_{1}}{k_{2}} A^{} + A; A^{} k_{3} - - \to r d s$ Product and overall order is one.

Since, overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}}$
So, total energy of activation is
$E a_{1} + E a_{3} - E a_{2} \Rightarrow 40 + 20 - 30 = 30 k J$
$2 A^{} k_{1} - \to k_{2} A^{} + A; A^{*} k_{3} - -- \to R D S$ Product
This satisfied the condition $k = \frac{k_{1} k_{3}}{k_{2}}$ and overall order is one.

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