The temperature dependence of the rate constant (k) of a chemical reaction is written in terms of the Arrhenius equation $\mathrm{k}={\mathrm{Ae}}^{-{\mathrm{E}}_{\mathrm{a}}/\mathrm{RT}}$. The activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$ of the reaction can be calculated by plotting.

Statement-$1$: The order of a reaction can have a fractional value.

Statement-$2$: The order of a reaction cannot be written from the balanced equation of a reaction.

$3{\mathrm{BrO}}^{-}⟶{\mathrm{BrO}}_3^{\text{- }}+2{\mathrm{Br}}^{-}$

If $-\frac{\mathrm{d}\left[{\mathrm{BrO}}^{-}\right]}{\mathrm{dt}}={\mathrm{k}}_1 {\left[\mathrm{BrO}-\right]}^2;+\frac{\mathrm{d}\left[{\mathrm{BrO}}_3^{-}\right]}{\mathrm{dt}}={\mathrm{k}}_2 [\mathrm{BrO}-{]}^2;+\frac{\mathrm{d}\left[{\mathrm{Br}}^{-}\right]}{\mathrm{dt}}={\mathrm{k}}_3 {\left[\mathrm{BrO}-\right]}^2$ the correct relation between ${\mathrm{k}}_1,{\mathrm{k}}_2$ and ${\mathrm{k}}_3$ is:

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:

$\mathrm{A}+\mathrm{B}⟶\mathrm{C}$