What is the activation energy ( kJ / mol ) for a reaction if its rate constant doubles when the temperature is raised from 300 ~K to 400 ~K ? (R=8.314 ~J ~mol ⁻¹ ~K ⁻¹ )

Step-by-step solution

aligned & k₂ k₁ = E_a 2.303 R ( 1 T₁ - 1 T₂ ) & 2 1 = E_a 2.303 8.314 ( 1 300 - 1 400 ) & 0.3010= E_a 2.303 8.314 ( 100 300 400 ) & E_a=0.3010 2.303 8.314 3 400 & =6.916 ~kJ ~mol ⁻¹ aligned