According to the Arrhenius equation,the slope of the $\log k$ vs. $\frac{1}{T}$ plot is . . . . . . .

For a reaction,given below is the graph of $\ln k$ vs $\frac{1}{T}$. The activation energy for the reaction is equal to $...... \ cal \ mol^{-1}$. (Nearest integer). (Given : $R = 2 \ cal \ K^{-1} \ mol^{-1}$)

For the following two reactions,which statement is true?

$A$ reaction is catalysed by $X$. Here $X$:

The minimum energy required for molecules to enter into the reaction is called

For a reaction,activation energy $E_a = 0$ and rate constant $K = 3.2 \times 10^6 \ s^{-1}$ at $300 \ K$. What is the value of the rate constant at $300 \ K$?