For a first-order reaction $\mathrm{A}\to \mathrm{B}$ the plot of $\log [\mathrm{A}{]}_{\mathrm{t}}$ versus $\mathrm{t}$ is linear with a:

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.

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.