Well, the Arrhenius equation gives you the reaction rate based on the energy of activation and temperature. So the best way to understand it is to dissect it. First, collision theory predicts that reactions occur when molecules collide. When reactants A and B collide, they form an activated complex that has enough energy to go over the energy barrier. But these activated complexes may not be in the right geometry to do so. Imagine an SN2 reaction where the nucleophile is on the wrong side of the sigma anti-bonding orbital that is attacked. So the colliding species must also be in the correct orientation. Finally, if collisions occur a lot, there is a greater chance for reaction as opposed to if collision frequency is low.
So the Arrhenius equation is k = A*e^-E/RT. The pre-exponential term A combines the frequency and orientation factors. So if frequency is high, the reaction is more likely to occur and occurs faster. The E takes into account the energy barrier. If the energy barrier is high, the rate approaches zero - what you would expect if molecules were in an infinite potential well. Finally, T takes into account temperature. If temperature is high, there is a greater chance that the colliding molecules will have enough energy to go over the energy barrier. Thus, as T increases, k also increases.
You can derive the Arrhenius equation but I won't do it here - just Google that.
The Eyring equation is : k = (kb*T/h)*e^(-delta H/RT)*e^(delta S/R), where the thermodynamic parameters refer to the transition state. So you can see that the Eyring equation has basically set the pre-exponential factor. In addition, the "transition state" referred to by these two equations are not identical but I believe that is beyond the scope of the MCAT. You can also derive the Eyring equation but it is not intuitive at all and definitely beyond the scope of the MCAT.
You can also parse through the terms of the Eyring equation as well to rationalize the roles enthalpy and entropy play in determining rate constant.