The following equation is obtained for a first order reaction at 300 K . $\log _{10} \frac{\mathrm{k}}{\mathrm{~A}}=0.00174$ What is the activation energy (in $\mathrm{J} \mathrm{mol}^{-1}$ ) of the reaction? $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

• Correct answer
  A

  $10.0$
• B

  $100.0$
• C

  $0.1$
• D

  $1.0$

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