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(B) According to the Arrhenius equation,the rate constant $k$ is given by $k = A e^{-E_a/RT}$.As the temperature $T$ increases,the fraction of molecul

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Increase in the number of activated molecules

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(B) According to the Arrhenius equation,the rate constant $k$ is given by $k = A e^{-E_a/RT}$.As the temperature $T$ increases,the fraction of molecules having energy equal to or greater than the activation energy $(E_a)$ increases significantly.This leads to a larger number of effective collisions,resulting in a substantial increase in the reaction rate.Therefore,the correct reason is the increase in the number of activated molecules.

$A$ large increase in the rate of reaction for a small increase in temperature is due to:

Similar Questions

The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^/RT}$. The activation energy $(E^)$ of the reaction can be calculated by plotting:

Explain the collision theory of chemical reactions.

Reactant $A$ shows two reactions:
$A \xrightarrow{K_1} B$,activation energy $= Ea_1$
$A \xrightarrow{K_2} C$,activation energy $= Ea_2$
If $Ea_1 = \frac{Ea_2}{3}$,then the relation between $K_1$ and $K_2$ is:

Activation energy is given by the formula

The following energy profile diagram is given for the reaction $A + B \to C + D$. The enthalpy change and activation energy for the reverse reaction $C + D \to A + B$ are respectively:

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