Question

choose one of the factors from the previous question and explain how it affects the rate of the reaction, using collision theory in your response. (2 pts)

Explanation:

To answer this, we first recall factors affecting reaction rates (e.g., temperature, concentration, surface area, catalyst). Let's take temperature as an example. Collision theory states reactions occur when particles collide with sufficient energy (activation energy) and correct orientation. Increasing temperature increases the kinetic energy of particles. This leads to more frequent collisions and a higher proportion of collisions with energy ≥ activation energy. So, reaction rate increases. For a catalyst: it provides an alternate pathway with lower activation energy. More particles now have energy ≥ new (lower) activation energy, increasing effective collisions and thus reaction rate. For concentration: higher concentration means more particles per unit volume, increasing collision frequency, so more effective collisions and faster rate. For surface area (in solids): increasing surface area (e.g., powder vs. lump) exposes more particles, increasing collision frequency with reactant particles, boosting reaction rate.

Answer:

Let's choose "Temperature" as the factor. According to collision theory, reaction rate depends on effective collisions (sufficient energy + correct orientation). Increasing temperature increases particles’ kinetic energy. This causes: 1) More frequent collisions (due to higher speed). 2) A larger fraction of collisions with energy ≥ activation energy. Both increase effective collisions, so reaction rate rises. (Other valid factors: Concentration - more particles → more collisions; Catalyst - lowers activation energy → more effective collisions; Surface Area - more exposed particles → more collisions.)