Q

# Can someone explain - Chemical kinetics - JEE Main-2

Rate of a reaction can be expressed by Arrhenius equation as : $\dpi{100} k=Ae^{-E/RT}$  . In this equation, $\dpi{100} E$ represents

• Option 1)

the energy above which all the colliding molecules will react

• Option 2)

the energy below which colliding molecules will not react

• Option 3)

the total energy of the reacting molecules at a temperature , $T$

• Option 4)

the fraction of molecules with energy greater than the activation energy of the reaction.

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As we learnt in

Arrhenius Equation -

Arrhenius gave the quantitative dependence of rate constant on temperature by the Arrhenius equation.

- wherein

$k = A e^{-E_{a}/RT}$

$In k=InA-\frac{E_{a}}{RT}$

$k$ = Rate constant

Activation Energy -

The minimum kinetic energy that reactants must have in order to form products.

- wherein

Description:

E.g.: In a gas phase reaction numerous collisions take place but only a tiny proportion which has sufficient energy to cross the energy barrier leads to product formation.

$K = A\times e^{\frac{-Ea}{rt}}$

Ea = Activation energy is energy below which colliding molecules will not react.

Option 1)

the energy above which all the colliding molecules will react

This option is incorrect

Option 2)

the energy below which colliding molecules will not react

This option is correct

Option 3)

the total energy of the reacting molecules at a temperature , $T$

This option is incorrect

Option 4)

the fraction of molecules with energy greater than the activation energy of the reaction.

This option is incorrect

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