Is the activation energy-dependent on temperature?

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Solution

When the temperature rises, the molecules obtain more energy and begin to move faster and quicker.
As the temperature rises, the likelihood of molecules moving with the required activation energy for collision increases.
The activation energy is the smallest amount of energy required for molecules to collide. Because the amount of energy required for the collision is constant, the activation energy remains constant.
The formula used to find the value of Activation Energy, $E_{a}$ is: : $K = A e^{\frac{- E a}{R T}}$ Where $K =$ Rate Constant, $A =$ Arrhenius Constant, $E_{a} =$ Activation Energy, $R =$ Gas constant $= 8.34 \frac{J}{K / mol}$
Hence, No the activation energy is not dependent on temperature.

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