Unit 10a: Kinetics Review

Flashcards for Kinetics Review

Collision Theory

For a chemical reaction to occur, there must be an effective collision between reactant particles.

Effective Collisions

Sufficient kinetic energy (speed) and proper orientation (facing the correct way).

Rates of Chemical Reactions

How fast products are produced; the more effective collisions, the faster the rate.

Temperature effect on reaction rate

Higher temps = faster rate.

Concentration of Reactants effect on reaction rate

High concentration = faster rate.

Nature of Reactants in reaction rate

Ionic compounds react faster than covalent compounds.

Surface Area effect on reaction rate

Smaller particles = greater surface area = faster rate.

Catalyst

Lowers the activation energy, by creating an alternate pathway thus speeding up reaction rates.

Phase of Reactants effect on reaction rate

Gases and aqueous solutions react faster than solids.

Activation Energy

Energy needed to start a chemical reaction; higher activation energy = slower reaction.

Entropy

Disorder; gases > liquids > solids.

Temperature effect on Entropy

Higher temps = more entropy.

Nature's tendency

Systems tend to undergo changes towards lower energy and higher entropy.