(a) What factors determine whether a collision between two molecules will lead to a chemical reaction? (b) According to the collision model, why does temperature affect the value of the rate constant? (c) Does the rate constant for a reaction generally increase or decrease with an increase in reaction temperature?

(a) Two main factors determine whether a collision between two molecules will lead to a chemical reaction: 1. Reactive orientation - molecules must collide with the correct orientation. 2. Activation energy - colliding molecules must possess sufficient energy to overcome the activation energy barrier. (b) According to the collision model, temperature affects the rate constant because an increase in temperature causes molecules to move faster, collide more frequently, and with greater energy, leading to a higher probability of effective collisions. This relationship is described by the Arrhenius equation: \(k = Ae^{\frac{-Ea}{RT}}\). (c) The rate constant for a reaction generally increases as the reaction temperature increases, as there are more effective collisions and the Arrhenius equation shows a direct relationship between temperature and the rate constant.