Question

how does increasing temperature generally increase reaction rate?
at higher temperatures, a greater proportion of particles have the sufficient energy, aka the activation energy, $e_a$, necessary for a successful collision.
at higher temperatures, a majority of particles have the sufficient energy, aka the enthalpy, $delta h$, necessary for a successful collision.
at higher temperatures, the majority of particles have the sufficient energy, aka the activation energy, $e_a$, necessary for a successful collision.
at higher temperatures, a greater proportion of particles have the sufficient energy, aka the enthalpy, $delta h$, necessary for a successful collision.

Explanation:

In chemical kinetics, the activation energy ($E_a$) is the minimum energy required for a reaction - causing collision between particles. Increasing temperature increases the average kinetic energy of particles. So, a greater proportion of particles have energy equal to or greater than the activation energy, leading to more successful collisions and a higher reaction rate. Enthalpy ($\Delta H$) is the heat - content change of a reaction and not the energy for successful collisions.

Answer:

At higher temperatures, a greater proportion of particles have the sufficient energy, aka the activation energy, $E_a$, necessary for a successful collision.