Consider the following transformation involving first order elementary reaction in each step at constant temperature as shown below. {\A}+ {\B} \stackrel{\text{ Step }{ {⇌} 1}_{\text{ Step } 3}} {\C} \stackrel{\text{ Step 2 }\xrightarrow} {\P} Some details of the above reaction are listed below. Step \text{ Rate constant } ( \sec ^{-1}) \text{ Activation } \ \text{ energy } ( {\kJ} {\mol}^{-1}) 1 {\k}_1 300 2 {\k}_2 200 3 {\k}_3 {\Ea}_3 If the overall rate constant of the above transformation (k) is given as {\k}= { {\k}_1 {\k}_2}/{ {\k}_3} and the overall activation energy ( {\E}_{ {\a}}) is 400 {\kJ} {\mol}^{-1}, then the value of {\Ea}_3 is ______ {\kJ} {\mol}^{-1} (nearest integer) [4 Apr 2024 Shift 1]

Chemical Kinetics Part 2

Section: Chemistry

Question : 50 of 111

Marks: +1, -0

Consider the following transformation involving first order elementary reaction in each step at constant temperature as shown below.
A+B‌

‌ Step ‌1

⇌

‌ Step ‌3

‌ Step 2 ‌

───────▶

P
Some details of the above reaction are listed below.

If the overall rate constant of the above transformation (k) is given as k=‌

k1k2

and the overall activation energy (Ea) is 400‌kJ‌mol−1, then the value of Ea3 is ______ kJ‌mol−1 (nearest integer)

[4 Apr 2024 Shift 1]

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