Kinetics and Collision Theory

Front

What happens if reactant particles collide with less than the activation energy?

Back

The particles will rebound, and no reaction will occur.

Front

What does more collisions correspond to in terms of reaction rate?

Back

Faster reaction rate.

Front

What does the collision theory qualitatively explain?

Back

How chemical reactions occur and why reaction rates differ for different reactions.

Front

Under the collision theory, what must particles do for a reaction to occur?

Back

Collide with sufficient energy and correct orientation.

Front

What are the fundamental ideas of collision theory?

Back

1. Molecules react by colliding together. 2. Effective collisions must occur with certain minimum amounts of energy. 3. In a large sample, the greater the number of effective collisions, the faster the rate of reaction.

Front

Define activation energy.

Back

The minimum energy required for a chemical reaction to occur.

Front

What is the role of orientation in collisions according to collision theory?

Back

Particles must collide in the correct orientation for a reaction to occur.

Front

How does temperature affect reaction rates according to collision theory?

Back

Increasing temperature increases the kinetic energy of particles, leading to more frequent and effective collisions.

Front

What is the effect of concentration on reaction rates?

Back

Higher concentration increases the number of particles in a given volume, leading to more collisions and a faster reaction rate.

Front

Explain the concept of effective collisions.

Back

Effective collisions are those that result in a chemical reaction, requiring sufficient energy and proper orientation.