(C) The overall rate constant is given by $K = \frac{K_1 K_2}{K_3}$.Substituting the Arrhenius equation $K = A \cdot e^{-E_a / RT}$ for each step:$A \

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(C) The overall rate constant is given by $K = \frac{K_1 K_2}{K_3}$.Substituting the Arrhenius equation $K = A \cdot e^{-E_a / RT}$ for each step:$A \cdot e^{-E_a / RT} = \frac{(A_1 e^{-E_{a1} / RT}) \cdot (A_2 e^{-E_{a2} / RT})}{(A_3 e^{-E_{a3} / RT})}$$A \cdot e^{-E_a / RT} = \frac{A_1 A_2}{A_3} \cdot e^{-(E_{a1} + E_{a2} - E_{a3}) / RT}$Comparing the exponents,we get $E_a = E_{a1} + E_{a2} - E_{a3}$.Substituting the given values: $E_a = 40 + 50 - 60 = 30 \ kJ/mol$.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

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For a reaction taking place in three steps at the same temperature,the overall rate constant is $K = \frac{K_1 K_2}{K_3}$. If $E_{a1}$,$E_{a2}$,and $E_{a3}$ are $40 \ kJ/mol$,$50 \ kJ/mol$,and $60 \ kJ/mol$ respectively,the overall activation energy $E_a$ is . . . . . . $kJ/mol$.

JEE MAIN 2024 All JEE MAIN

A
$20$
B
$10$
C
$30$
D
$45$

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Collision theory, Energy of activation and Arrhenius equation

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For a reaction taking place in three steps at the same temperature,the overall rate constant is $K = \frac{K_1 K_2}{K_3}$. If $E_{a1}$,$E_{a2}$,and $E_{a3}$ are $40 \ kJ/mol$,$50 \ kJ/mol$,and $60 \ kJ/mol$ respectively,the overall activation energy $E_a$ is . . . . . . $kJ/mol$.

Similar Questions

The equation $k = (6.5 \times 10^{12} \, s^{-1}) e^{-26000 \, K / T}$ is followed for the decomposition of compound $A$. The activation energy for the reaction is $..... \, kJ \, mol^{-1}$. [nearest integer] (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$)

For a reaction,activation energy $E_a = 0$ and rate constant $K = 3.2 \times 10^6 \ s^{-1}$ at $300 \ K$. What is the value of the rate constant at $300 \ K$?

The enthalpy $(H)$ of an elementary exothermic reaction,$A \rightleftharpoons B$ is schematically plotted against the reaction coordinate. The plots in the presence and absence of a catalyst are shown in dashed and solid lines,respectively. Identify the correct plot for the reaction.

$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$The curves $M$ and $N$ represent the variation of energy with reaction coordinate for the reaction in absence and presence of catalyst.Which value represents the activation energy $(E_a)$ for the backward reaction in the presence of catalyst?

The rate of the process doubles with every $10 \ K$ increase in temperature. When the temperature is increased from $303 \ K$ to $353 \ K$,how much will the rate of the process increase?

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