The study of energy and its transformations; in chemistry, it determines if a reaction can occur (spontaneity).

The study of reaction rates and mechanisms; it determines how fast a reaction occurs.

The minimum energy required for a reaction to occur.

A substance that speeds up a reaction by providing an alternative reaction pathway with a lower activation energy; it doesn't change the thermodynamics (ΔG).

How quickly reactants turn into products, measured as the change in concentration over time.

A situation where the rate of a reaction is slow due to a high activation energy, even if the reaction is thermodynamically favorable (spontaneous).

Thermodynamics: Determines if a reaction *can* happen (spontaneous/non-spontaneous), considers Gibbs Free Energy (ΔG). | Kinetics: Determines *how fast* a reaction happens, considers reaction rates and activation energy.

Catalyzed Reaction: Lower activation energy due to an alternative pathway. | Uncatalyzed Reaction: Higher activation energy, requiring more energy for the reaction to occur.

Spontaneous Reaction: A reaction that has a negative ΔG and is thermodynamically favorable. | Fast Reaction: A reaction that proceeds quickly due to a low activation energy or the presence of a catalyst.

ΔG: Catalyst has no effect on the Gibbs Free Energy change of the reaction. | Activation Energy (Ea): Catalyst lowers the activation energy, speeding up the reaction.

The reaction proceeds slowly, even if it is thermodynamically favorable.

The reaction rate increases because the catalyst provides an alternative pathway with a lower activation energy.

The reaction is spontaneous, meaning it is thermodynamically favorable, but it doesn't guarantee a fast reaction.

The reaction rate increases, as the catalyst lowers the activation energy, allowing the reaction to proceed faster.

The reaction rate generally increases, as described by the rate law (R = k[A]^n[B]^m).