At a certain temperature, the first order rate constant $k_1$ is found to be smaller than the second order rate constant $k_2$. If the $E_a$ (1) of the first order reaction is greater then $E_a$ (2) of the second order reaction, then as temperature is raised:

For a first-order gas-phase reaction:

${\mathrm{A}}_{\left(\mathrm{g}\right)}\to 2{\mathrm{B}}_{\left(\mathrm{g}\right)}+{\mathrm{C}}_{\left(\mathrm{g}\right)}$

${\mathrm{P}}_{\mathrm{o}}$ be initial pressure of $\mathrm{A}$ and ${\mathrm{P}}_{\mathrm{t}}$ the total pressure at time $\text{'}\mathrm{t}\text{'}$, Integrated rate equation is:

Assertion: Two different reactions can never have same rate of reaction.

Reason: Rate of reaction always depends only on frequency of collision and Arrhenius factor.

Select the rate law that corresponds to the data shown for the following reaction:

$\mathrm{A}+\mathrm{B}⟶\mathrm{C}$

Assertion: If the activation energy of a reaction is zero, the temperature will have no effect on the rate constant.

Reason: Lower the activation energy, faster is the reaction.

A reaction which is of the first order with respect to a reactant $\mathrm{A}$, has a rate constant of $6 {\min }^{-1}$. If we start with $\left[\mathrm{A}\right]=0.5 \mathrm{mol} {\mathrm{L}}^{-1}$, when would $\left[\mathrm{A}\right]$ reach the value of $0.05 \mathrm{mol} {\mathrm{L}}^{-1}$?