Reaction A and reaction B have identical frequency factors. However, reaction B has a higher activation energy than reaction A. Part A Which reaction has a smaller rate constant at room temperature?

reaction B

Explanation:

From Arrhenius equation

k=A e-Ea/RT

Where

K= rate constant

Ea= activation energy

R= universal gas constant

T= temperature in kelvin

A= frequency factor

The higher the activation energy, the lower the value of e-Ea/RT. If A is constant for reaction A and B, then the reaction with lower activation energy will have a higher value of rate constant, k because e-Ea/RT will have a higher value. Hence reaction B having a greater activation energy will have a smaller value of rate constant k.

they both have a y in them

the increase of protons   hope this