Activation energy of a reaction

Question

Activation energy of a reaction (A) is independent of temperature (B) increases with temperature (C) gets doubled for every 10 degree rise in temperature (D) decreases with temperature

Tardigrade Admin · Accepted Answer

According to Arrhenius equation, the relationship between the activation energy and temperature is

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

lo g k = \frac{- E _{a}}{2.303 RT} + lo g A

∴

Activation energy decreases with rise in temperature, thereby increasing the rate of the reaction.

Q. Activation energy of a reaction

is independent of temperature

increases with temperature

gets doubled for every 10 degree rise in temperature

decreases with temperature

According to Arrhenius equation, the relationship between the activation energy and temperature is k=Ae−Ea​/RT logk=2.303RT−Ea​​+logA ∴ Activation energy decreases with rise in temperature, thereby increasing the rate of the reaction.

According to Arrhenius equation, the relationship between the activation energy and temperature is
$k = A e^{- E_{a} / RT}$
$lo g k = \frac{- E _{a}}{2.303 RT} + lo g A$
$∴$ Activation energy decreases with rise in temperature, thereby increasing the rate of the reaction.