Are the reaction rates of these equations equal?
For the reaction kinetic rate constants, there is the well known Arrhenius equation:

$$k=A \cdot \exp{\left(-\frac{E_\mathrm{a}}{RT}\right)}$$

$A$ is sometimes called frequency factor, interpreted as the rate of collisions with the proper orientation of molecules.

It has 2 terms:


The rate of general collisions, that is function of temperature and molecular masses, which determine speed of molecular motion (close relation to the kinetic theory of gases). Note that the temperature dependence is much smaller than for the exponential Boltzmann term.
The probability of the proper orientation of molecules, what depends on the molecular geometry. For molecules of  otherwise the same geometry, it depends on covalent atom radii. 


The exponential term follows the Boltzmann statistical distribution, determining the probability molecules would have enough kinetic energy to overcome the reaction activation energy barrier.

All 3 terms (2 for $A$ and the exponential term) Are different for different halogen atoms.


The mass molecules increases fluorine &lt; iodine, so collision frequency as the rate constant term is the lowest for iodine.
As the reaction mechanism I suppose SN2. The geometrical aspects of $\ce{-CH2X}$ is tricky to determine from basic principles. Bigger halogen is more sterically blocking, but is also farther from the central carbon. More polar bond of the smaller halogen should cause stronger  repelling of the other 3 bonds, so the other side is more open for sn2 reaction.
Activation energy would decrease ( and the Boltzmann term for the rate constant increase) in order F ... I


That about the principles. To compare the particular rates, it is matter of experimental data.