Why does increasing the temperature affect the rate constant for a reaction? A.
increasing the temperature increases the average kinetic energy
B.
increasing the temperature increases the activation energy
C.
increasing the temperature decreases the average kinetic energy
D.
increasing the temperature causes the reaction to occur more slowly

Hope this answer helps I don't know for sure which one it is but here is some information.

Explanation:

Increasing the temperature increases the kinetic energy of reactant molecules. Therefore they move around more and they move faster. As a result, collisions between reactant molecules are more frequent and the energy at which they collide is also sufficient enough to overcome the activation energy of the reaction. Hence a greater proportion of reactant molecules successfully collide, leading to an increase in the rate of reaction.