Reaction rate is determined by the activation energy for the reaction.
The thermodynamic product is the one which is the most stable once formed.
The kinetic product is the one that is easiest to form. This is the product with the lowest activation energy barrier to formation. k=Ae^(-E/RT) where k is the rate constant, A is the Arrhenius factor, R is the gas constant, T is the temperature in Kelvin, and E is the activation energy.
Sometimes the thermodynamic product is also the product that is formed the fastest, sometimes it is not.
If the thermodynamic product is also the product with the lowest activation energy, then it will also be the kinetic product.
For free radical halogenation, the activation energy is lowest for tertiary carbons, so tertiary halogenation will occur the fastest. This is probably due to the stability of the radical intermediate formed in tertiary halogenation. That said, this question was unanswerable without looking up rate data or having memorized that the activation energy for primary alkanes is higher than tertiary alkanes.