According to the Arrhenius equation, the rate constant $\mathrm{k}$ is equal to ${\mathrm{Ae}}^{-\mathrm{E}}{\mathrm{a}}^{/\mathrm{RT}}$. Which of the following options represents the graph of $\ln \mathrm{k} \mathrm{vs}\frac{1}{ \mathrm{T}}?$

$\mathrm{k}={\mathrm{Ae}}^{-\mathrm{E}}{\mathrm{a}}^{/\mathrm{RT}}$

Consider the graph given below. Which of the following options does not show an instantaneous rate of reaction at ${40}^{\mathrm{th}}$ second?

Which of the following graphs represents exothermic reaction?

Rate law for the reaction $\mathrm{A}+2 \mathrm{B}⟶\mathrm{C}$ is found to be
Rate$=\mathrm{k}[ \mathrm{A}]\left[\mathrm{B}\right]$

Concentration of reactant ' $\mathrm{B}$ ' is doubled. Keeping the concentration of '$\mathrm{A}$' constant, the value of rate constant will be :