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

For reactions $M, N, O$ and $P$,the activation energy order is $E_M < E_N < E_O < E_P$. For which reaction will the ratio $K_{310}/K_{300}$ be maximum?

The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

For a reaction,the rate constants $K_1$ and $K_2$ are given by $10^{16} \cdot e^{-2000/T}$ and $10^{15} \cdot e^{-1000/T}$ respectively. At what temperature will $K_1 = K_2$?

The equation $k = (6.5 \times 10^{12} \, s^{-1}) e^{-26000 \, K / T}$ is followed for the decomposition of compound $A$. The activation energy for the reaction is $..... \, kJ \, mol^{-1}$. [nearest integer] (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$)

On increasing the temperature,the rate of the reaction increases because of