The activation energy of a reaction is zero. The rate constant of this reaction

Question

The activation energy of a reaction is zero. The rate constant of this reaction (A) increases with an increase of temperature (B) decreases with an increase of temperature (C) decreases with decrease of temperature (D) is independent of temperature

Tardigrade Admin · Accepted Answer

From Arrhenius equation, log k= log A-(Ea/2.303 R T) As the activation energy of a reaction is zero, the rate constant of this reaction becomes zero. It shows that the reaction is independent of temperature.

Q. The activation energy of a reaction is zero. The rate constant of this reaction

increases with an increase of temperature

decreases with an increase of temperature

decreases with decrease of temperature

is independent of temperature

From Arrhenius equation,
$lo g k = lo g A - \frac{E _{a}}{2.303 RT}$
As the activation energy of a reaction is zero, the rate constant of this reaction becomes zero.
It shows that the reaction is independent of temperature.

Q. The activation energy of a reaction is zero. The rate constant of this reaction

increases with an increase of temperature

decreases with an increase of temperature

decreases with decrease of temperature

is independent of temperature

From Arrhenius equation, logk=logA−2.303RTEa​​ As the activation energy of a reaction is zero, the rate constant of this reaction becomes zero. It shows that the reaction is independent of temperature.

From Arrhenius equation,
$lo g k = lo g A - \frac{E _{a}}{2.303 RT}$
As the activation energy of a reaction is zero, the rate constant of this reaction becomes zero.
It shows that the reaction is independent of temperature.