1. The given equation is the Arrhenius equation in chemical kinetics:

$k = A e^{-E_a/(RT)}$

where:

• $k$ = rate constant
• $A$ = frequency factor (or pre-exponential factor)
• $E_a$ = activation energy
• $R$ = universal gas constant
• $T$ = absolute temperature

2. Now evaluate each option:

Option A: $A$ is adsorption factor
This is incorrect. In the Arrhenius equation, $A$ is the frequency factor, not adsorption factor.

Option B: $E_a$ is energy of activation
This is correct. $E_a$ denotes the activation energy required for the reaction.

Option C: $R$ is Rydberg’s constant
This is incorrect. Here $R$ is the universal gas constant, not Rydberg’s constant.

Option D: $k$ is equilibrium constant
This is incorrect. $k$ represents the rate constant, not the equilibrium constant.

3. Therefore, the correct option is:

$\boxed{\text{B}}$

4. Comparison with stored correct answer:

Stored correct answer = B
Derived answer = B

So, the derived answer agrees with the stored correct answer.