The activation energy of an uncatalyzed reaction is 99 kJ/mol. The addition of a catalyst lowers the activation energy to 62 kJ/mol. Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 124 C? Express the ratio to two significant digits. ? ke/ky = 8.2. 104 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining The factor by which the rate increases is equal to the ratio of catalyzed rate constant (ke) over the uncatalyzed rate constant (ku). The ratio can be determined using the Arrhenius equation. Setting up a ratio using the Arrhenius equation for each reaction condition results in the following equation: ke ku -Eq.c+E, RT =e Use the temperature (T), gas constant (R), and activation energies (Eq,c and Eq,u) to determine the relative change to the rate of the reaction