At $527 \, ^{\circ}C$ temperature,the activation energy is $54.7 \, kJ/mol$. The value of the Arrhenius factor is $4 \times 10^{10}$. The rate constant will be:

Consider an endothermic reaction $X \to Y$ with the activation energies $E_b$ and $E_f$ for the backward and forward reactions,respectively. In general:

Consider the following plots of rate constant versus $\frac{1}{T}$ for four different reactions. Which of the following orders is correct for the activation energies of these reactions?

Which among the following is correct when energy of activation,$E_a$ of the catalyzed reaction decreases at constant temperature and for same concentration?

For a first order reaction,the rate of reaction is $2.4 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$ at $27 \ ^\circ C$. The activation energy of the reaction is $24.942 \ kJ \ mol^{-1}$. The rate of reaction at $327 \ ^\circ C$ is ....... $mol \ L^{-1} \ s^{-1}$ [Take $e^5 = 150$,$e^{0.005} = 1$,$e^4 = 55$].

Among the following,the $INCORRECT$ statement regarding the collision theory of chemical reaction is: