Consider the following reaction
$\mathrm{A}(\mathrm{~g}) \rightarrow \mathrm{B}(\mathrm{~g})+\mathrm{C}(\mathrm{~g})$

The following data were obtained in a 500 ml flask at 300 K

$\begin{array}{|c|c|} \hline \text{Time (s)} & \text{Total Pressure (Torr)} \\ \hline 0 & 80 \\ \hline 2 & 120 \\ \hline 4 & 140 \\ \hline \end{array}$

The rate of reaction (in Torr $\mathrm{s}^{-1}$ ) at $\mathrm{t}=8 \mathrm{~s}$ is

• Correct answer
  A

  $2.5 \ln 2$
• B

  $0.5 \ln 2$
• C

  $2.0 \ln 2$
• D

  $1.5 \ln 2$

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