chemistry chapter 6 - rates of reaction

Rate of Reaction

The speed at which reactants are converted into products.

Collision Theory

The theory that chemical reactions occur when reactant particles collide with sufficient energy.

Activation Energy

The minimum amount of energy required for reactants to undergo a reaction.

Catalyst

A substance that increases the rate of a reaction by lowering the activation energy without being consumed.

Surface Area

The total area of the surface of a reactant that is exposed for reaction; increasing this area increases the reaction rate.

Effects of Temperature on Reaction Rate

Increasing the temperature raises particle energy, leading to more frequent collisions.

Reversible Reactions

Reactions where products can revert back to reactants when conditions change.

Equilibrium

A state in a closed system where the rate of the forward reaction equals the rate of the reverse reaction.

Le Chatelier's Principle

The principle stating that if a change is made to a system in equilibrium, the system will adjust to counteract the change.

Mean Rate of Reaction

Calculated as the amount of product formed or reactant used divided by the time taken.

Visual Change Method

A method of measuring the rate of reaction based on observable changes such as cloudiness or color change.

Gas Collection Method

A method to measure the rate of reaction by collecting gas produced and measuring its volume.

Concentration

The amount of a substance in a given volume; higher concentration increases the frequency of collisions.

Pressure

In gases, increasing pressure can affect reaction rates by changing particle collisions.

Turbidity

The cloudiness of a solution due to the presence of particles.