Aim 61

Chemical Kinetics

Study of reaction rates and mechanisms in chemistry.

Reaction Rate

Speed at which reactants convert to products.

Effective Collisions

Collisions with proper orientation and sufficient energy.

Homogeneous Reactions

Reactions where all reactants share the same phase.

Heterogeneous Reactions

Reactions with reactants in different phases.

Concentration of Reactants

Higher concentration usually increases reaction rate.

Temperature Effect

Higher temperature increases reaction rate significantly.

Catalysts

Substances that speed up reactions without permanent change.

Pressure (Gases)

Increased pressure raises reaction rate for gases.

Mechanism of Reaction

Step-by-step sequence of reactions in a process.

Rate Determining Step

Slowest step that controls overall reaction rate.

Intermediates

Substances produced and consumed during a reaction.

Collision Theory

Theory explaining how reactions occur through collisions.

Activation Energy

Minimum energy required for a reaction to occur.

Enzymes

Biological catalysts that speed up biochemical reactions.

Ba(NO3)2 Reaction

Example of a double displacement reaction.

Na2S2O3 Reaction

Example of a reaction producing sulfur and water.

H2O2 Decomposition

Reaction producing water and oxygen from hydrogen peroxide.

Kinetic Energy

Energy of particles related to temperature.

Reaction Mechanism Steps

Individual steps that lead to product formation.

Overall Reaction Rate

Determined by the slowest step in the mechanism.