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.

<p>Clearly, if $\mathrm{E}_a=0, \mathrm{~K}$ is temperature independent if $\mathrm{E}_a&gt;0, \mathrm{~K}$ increase with increase in temperature if $\mathrm{E}_a&lt;0, \mathrm{~K}$ decrease with increase in temperature</p> <ul> <li>Rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy.</li><br/> <li>Higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant.</li><br/> <li>The pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.<br/><br/> a. A high activation energy usually implies a slow reaction.<br/><br/> b. $k=\mathrm{P} \times \mathrm{Z} \times \mathrm{e}^{-\mathrm{E}_a / \mathrm{RT}}$<br/><br/> c. The pre-exponential factor $(\mathrm{A}=\mathrm{P} \times \mathrm{Z})$ is independent of the activation energy and the energy of molecules.</li> </ul>