Collision Theory Flashcards

All 6 cards in this deck

According to collision theory, what two conditions must be met for a reaction to happen?

Particles must collide, and the collision must have enough energy (the activation energy) — a successful collision.

In terms of collisions, why does increasing the temperature increase the rate of reaction?

Particles move faster so collide more frequently, and more collisions have enough energy — so more frequent successful collisions.

In terms of collisions, why does increasing the concentration of a solution increase the rate of reaction?

There are more particles in the same volume, so collisions are more frequent.

In terms of collisions, why does increasing the pressure of reacting gases increase the rate of reaction?

The same number of particles are squeezed into a smaller volume, so collisions are more frequent.

In terms of collisions, why does using smaller pieces of a solid reactant increase the rate of reaction?

Smaller pieces have a larger surface area to volume ratio, so more particles are exposed and collisions are more frequent.

True or false? Increasing the concentration of an acid makes its particles move faster.

False. Higher concentration means more particles in the same volume, so collisions are more frequent; only raising the temperature makes particles move faster.