The number of given statement/s which is/are correct is______
(A) The stronger the temperature dependence of the rate constant, the higher is the activation energy.
(B) If a reaction has zero activation energy, its rate is independent of temperature.
(C) The stronger the temperature dependence of the rate constant, the smaller is the activation energy.
(D) If there is no correlation between the temperature and the rate constant then it means that the reaction has negative activation energy.

Analyzing each statement using the Arrhenius equation $$k = Ae^{-E_a/RT}$$:

A: "The stronger the temperature dependence of the rate constant, the higher is the activation energy."

From the Arrhenius equation, $$\frac{d(\ln k)}{dT} = \frac{E_a}{RT^2}$$. Higher $$E_a$$ means $$k$$ changes more rapidly with temperature. This is correct. ✓

B: "If a reaction has zero activation energy, its rate is independent of temperature."

If $$E_a = 0$$, then $$k = A$$ (a constant), independent of temperature. This is correct. ✓

C: "The stronger the temperature dependence of the rate constant, the smaller is the activation energy."

This is the opposite of statement A and is incorrect. ✗

D: "If there is no correlation between temperature and rate constant, it means the reaction has negative activation energy."

No correlation means $$k$$ doesn't change with $$T$$, which implies $$E_a = 0$$, not negative. This is incorrect. ✗

Number of correct statements = 2 (A and B).