An industrial synthesis step involves an elementary reaction with an activation energy of 92 kJ·mol⁻¹. The process is currently operated at 300 K.
(a) By how many kelvin must the temperature be increased to double the rate constant, assuming the pre-exponential factor remains constant? Express your answer to the nearest kelvin.
(b) Alternatively, the company could introduce a catalyst at 300 K. By how many kJ·mol⁻¹ must the activation energy be lowered to achieve the same doubling of the rate constant?
(c) Compare the relative magnitudes of the temperature increase and the activation-energy decrease you calculated in parts (a) and (b). Based on your results and practical industrial considerations, discuss which strategy is likely to be more feasible.