What is the activation energy $$(\mathrm{kJ} / \mathrm{mol})$$ for a reaction if its rate constant doubles when the temperature is raised from $$300 \mathrm{~K}$$ to $$400 \mathrm{~K}$$ of these $$(R=8.314 \mathrm{~Jmol}^{-1} \mathrm{~K}^{-1})$$

Among the following statements, the correct statement about the half-life period for a first order reaction is

The rate constant for the first order decomposition of a certain reaction is described by the equation $$\ln k\left(\mathrm{~s}^{-1}\right)=14.34-\frac{1.25 \times 10^4 \mathrm{~K}}{T}$$. The energy of activation for this reaction is

Assertion (A) The reaction

$$\begin{aligned} 2 \mathrm{NO}+\mathrm{O}_2 & \longrightarrow 2 \mathrm{NO}_2 \\ \text { and } \quad 2 \mathrm{CO}+\mathrm{O}_2 & \longrightarrow 2 \mathrm{CO}_2 \end{aligned}$$

proceeds at the same rate because they are similar.

Reason (R) Both the reactions have same activation energy.