The rate constant is given by the equation $\mathrm{k}={\mathrm{Ae}}^{-{\mathrm{E}}_{\mathrm{a}}/\mathrm{RT}}$which factor should register a decrease for the reaction proceed more rapidly

Arrhenius Equation is expressed as $\mathrm{K}={\mathrm{Ae}}^{-{\mathrm{E}}_{\mathrm{a}}/\mathrm{RT}}$

In terms of natural logarithmic form the equation is written as

$\mathrm{Ink}=\mathrm{InA}-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{RT}}$

To increase the rate of reaction rapidly the rate constant should be increased. Thus the factor that is activation energy need to decrease to speed up the reaction.