(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 $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$

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$17$
B
$16$
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$14$
D
$15$

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Collision theory, Energy of activation and Arrhenius equation

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The rate constant of a first order reaction was doubled when the temperature was increased from $300 \ K$ to $310 \ K$. What is its approximate activation energy (in $kJ \cdot mol^{-1}$)? ($R = 8.3 \ J \cdot mol^{-1} \cdot K^{-1}$; $\log 2 = 0.3$)

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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 $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$

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For $N_2 + 3H_2 \rightarrow 2NH_3$,$\Delta H = -22 \ kcal$,and $E_a = 70 \ kcal$. Hence $E_a$ for $2NH_3 \rightarrow N_2 + 3H_2$ is $.....$ $kcal$.

$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$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 constant of a first order reaction was doubled when the temperature was increased from $300 \ K$ to $310 \ K$. What is its approximate activation energy (in $kJ \cdot mol^{-1}$)? ($R = 8.3 \ J \cdot mol^{-1} \cdot K^{-1}$; $\log 2 = 0.3$)

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