The rate $(r)$ of a chemical reaction is plotted against time $(t)$ in graph 1 . The initial rate of the reaction is $r_0$. The plot of $\ln \left(r / r_0\right)$ with time is shown in graph 2. The correct statement(s) is/are

• A

  The rate $(r)$ always decreases with time irrespective of the order of the reaction.
• Correct answer
  B

  After 69.3 s , the concentration of the reactant will be reduced to $(1 / 32)$ times of its initial concentration.
• Correct answer
  C

  Both the graphs represent the kinetics of a first order reaction.
• Correct answer
  D

  Initial concentration of the reactant is $500 \mathrm{~mol} \mathrm{~L}^{-1}$.

Hence, the correct answer is options: 'B', 'C', 'D'.