(C) The fraction of molecules having energy equal to or greater than the activation energy $(E_a)$ is given by the Arrhenius factor $f = e^{-E_a / RT}

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(C) The fraction of molecules having energy equal to or greater than the activation energy $(E_a)$ is given by the Arrhenius factor $f = e^{-E_a / RT}$.Given:$E_a = 80.9 \, kJ \, mol^{-1} = 80900 \, J \, mol^{-1}$$T = 700 \, K$$R = 8.31 \, J \, K^{-1} \, mol^{-1}$Comparing $e^{-E_a / RT}$ with $e^{-x}$,we get:$x = \frac{E_a}{RT}$Substituting the values:$x = \frac{80900}{8.31 \times 700}$$x = \frac{80900}{5817}$$x \approx 13.907$Rounding off to the nearest integer,we get $x = 14$.

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

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If the activation energy of a reaction is $80.9 \, kJ \, mol^{-1}$,the fraction of molecules at $700 \, K$,having enough energy to react to form products is $e^{-x}$. The value of $x$ is ....... . (Rounded off to the nearest integer) $[$Use $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$

JEE MAIN 2021 All JEE MAIN

A
$17$
B
$16$
C
$14$
D
$15$

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Collision theory, Energy of activation and Arrhenius equation

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If the activation energy of a reaction is $80.9 \, kJ \, mol^{-1}$,the fraction of molecules at $700 \, K$,having enough energy to react to form products is $e^{-x}$. The value of $x$ is ....... . (Rounded off to the nearest integer) $[$Use $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$

Similar Questions

For an effective collision to occur,the colliding molecules must possess:

If for a hypothetical reaction,$E_a = 0$ at $273 \ K$,then find the ratio of the rate constants at $383 \ K$ and $273 \ K$.

Explain: How is the value of activation energy determined based on the Arrhenius equation?

Calculate the activation energy of a reaction,whose rate constant doubles on raising the temperature from $300 \ K$ to $600 \ K$.

For a first-order gaseous reaction,a plot of $\log \, k$ versus $1/T$ gives a straight line with a slope of $-8000$. Calculate the activation energy $(E_a)$ of the reaction in $cal$.

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