The rate equation for the reaction $2 \mathrm{~A}+\mathrm{B} \longrightarrow \mathrm{C}$ is found to be: rate $\mathrm{k}[\mathrm{A}][\mathrm{B}]$. The correct statement in relation to this reaction is that the

• A

  unit of $\mathrm{K}$ must $\mathrm{be} \mathrm{s}^{-1}$
• Correct answer
  B

  values of $\mathrm{k}$ is independent of the initial concentration of $A$ and $B$
• C

  rate of formation of $C$ is twice the rate of disappearance of $A$
• D

  $t_{1 / 2}$ is a constant

Hence, the correct answer is option: 'B'.