(C) According to the Arrhenius theory,activation energy $(E_a)$ is defined as the additional energy that the reactant molecules must acquire over and

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The energy it has to acquire further so that it can enter into an effective collision

(C) According to the Arrhenius theory,activation energy $(E_a)$ is defined as the additional energy that the reactant molecules must acquire over and above their average kinetic energy to reach the threshold energy required for an effective collision.Therefore,the correct statement is that it is the energy the molecules have to acquire further so that they can enter into an effective collision.

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

Easy

According to Arrhenius theory,the activation energy is

A
The energy it should possess so that it can enter into an effective collision
B
The energy which the molecule should possess in order to undergo reaction
C
The energy it has to acquire further so that it can enter into an effective collision
D
The energy gained by the molecules on colliding with another molecule

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Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

Which equation is true to calculate the energy of activation,if the rate of reaction is doubled by increasing temperature from $T_1 \ K$ to $T_2 \ K$?

EasyGUJCET 2008

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The reaction: $Cr_{2}O_{3} + 2 Al \rightarrow Al_{2}O_{3} + 2 Cr$ $\quad (\Delta_{r}G^{\Theta} = -421 \ kJ)$ is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

Medium

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For the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the rate is given by $Rate = K[NO]^2[Cl_2]$. How can the rate constant $(K)$ of the reaction be increased?

Easy

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$A$ catalyst lowers the activation energy for a certain reaction from $83.314 \, kJ \, mol^{-1}$ to $75 \, kJ \, mol^{-1}$ at $500 \, K$. What will be the rate of reaction as compared to the uncatalysed reaction? Assume other things being equal.

Medium

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The reaction $X \to Y$ is an exothermic reaction. The activation energy of the forward reaction $X \to Y$ is $150\,kJ\,mol^{-1}$. The enthalpy of the reaction is $-135\,kJ\,mol^{-1}$. The activation energy for the reverse reaction,$Y \to X$,will be $.......\,kJ\,mol^{-1}$.

DifficultJEE MAIN 2013

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According to Arrhenius theory,the activation energy is

Similar Questions

Which equation is true to calculate the energy of activation,if the rate of reaction is doubled by increasing temperature from $T_1 \ K$ to $T_2 \ K$?

The reaction: $Cr_{2}O_{3} + 2 Al \rightarrow Al_{2}O_{3} + 2 Cr$ $\quad (\Delta_{r}G^{\Theta} = -421 \ kJ)$ is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

For the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the rate is given by $Rate = K[NO]^2[Cl_2]$. How can the rate constant $(K)$ of the reaction be increased?

$A$ catalyst lowers the activation energy for a certain reaction from $83.314 \, kJ \, mol^{-1}$ to $75 \, kJ \, mol^{-1}$ at $500 \, K$. What will be the rate of reaction as compared to the uncatalysed reaction? Assume other things being equal.

The reaction $X \to Y$ is an exothermic reaction. The activation energy of the forward reaction $X \to Y$ is $150\,kJ\,mol^{-1}$. The enthalpy of the reaction is $-135\,kJ\,mol^{-1}$. The activation energy for the reverse reaction,$Y \to X$,will be $.......\,kJ\,mol^{-1}$.

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