A reaction takes place in three steps with activation energy Ea1=180 kJ/mol, Ea2=80 kJ/mol and Ea3=50 kJ/mol respectively. Overall rate constant of the reaction is k=[(k1 k2/k3)]2 / 3 . The activation energy of the reaction will be

Question

A reaction takes place in three steps with activation energy Ea1=180 kJ/mol, Ea2=80 kJ/mol and Ea3=50 kJ/mol respectively. Overall rate constant of the reaction is k=[(k1 k2/k3)]2 / 3 . The activation energy of the reaction will be (A) 140 kJ/mol (B) 150 kJ/mol (C) 43.44 kJ/mol (D) 100 kJ/mol

Tardigrade Admin · Accepted Answer

The rate of constant of the reaction is k=[(k1 k2/k3)]2 / 3 Activation energy of the reaction will be Ea=(2/3)[.Ea1+Ea2-Ea3]. =(2/3)[.180+80-50]. =140 kJ/mol.

Q. A reaction takes place in three steps with activation energy $E_{a_{1}} = 180$ kJ/mol, $E_{a_{2}} = 80$ kJ/mol and $E_{a_{3}} = 50$ kJ/mol respectively.
Overall rate constant of the reaction is $k = [\frac{k _{1} k _{2}}{k _{3}}]^{2/3}$ .
The activation energy of the reaction will be

140 kJ/mol

150 kJ/mol

43.44 kJ/mol

100 kJ/mol

The rate of constant of the reaction is
$k = [\frac{k _{1} k _{2}}{k _{3}}]^{2/3}$
Activation energy of the reaction will be
$E_{a} = \frac{2}{3} [E_{a_{1}} + E_{a_{2}} - E_{a_{3}}]$
$= \frac{2}{3} [180 + 80 - 50]$
$= 140$ kJ/mol.

Q. A reaction takes place in three steps with activation energy Ea1​​=180 kJ/mol, Ea2​​=80 kJ/mol and Ea3​​=50 kJ/mol respectively. Overall rate constant of the reaction is k=[k3​k1​k2​​]2/3 . The activation energy of the reaction will be