• # question_answer The decomposition of ${{N}_{2}}O$ into ${{N}_{2}}$ and O in the presence of gaseous argon follows second order kinetics with $=K(5.0\times {{10}^{11}}L\,mo{{l}^{-1}}\,{{S}^{-1}}){{e}^{-29000K/T}}$Activation energy of the reaction is A)  $121\,KJ\,\,mo{{l}^{-1}}$             B)  $241\,KJ\,\,mo{{l}^{-1}}$C)  $201\,KJ\,\,mo{{l}^{-1}}$     D)  $280\,KJ\,\,mo{{l}^{-1}}$

On comparing the equation of K with $K=A{{e}^{{}^{-Ea}/{}_{RT}}}$ ${}^{Ea}/{}_{RT}=29000{}^{K}/{}_{T}$ $Ea=(29000\,K)R=241\,KJ\,mo{{l}^{-1}}$