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Chapter 14 explores chemical kinetics, discussing topics like collision theory, rate laws, orders, and Arrhenius's equation.
Kinetics
The study of the change in the concentrations of reactants and products over a period of time.
Collision Theory
A theory that states for a reaction to occur, particles must collide with sufficient energy and proper orientation.
Effective Collision
A collision between reactants that results in a chemical reaction.
Activation Energy (Ea)
The minimum energy required for a chemical reaction to occur.
Catalyst
A substance that increases the rate of a reaction without undergoing permanent change itself.
Reaction Rate
The speed at which reactants are converted into products over time.
Rate Law
An equation that relates the reaction rate to the concentration of reactants.
Zero Order Reaction
A reaction where the rate is independent of the concentration of the reactant.
First Order Reaction
A reaction where the rate is directly proportional to the concentration of one reactant.
Second Order Reaction
A reaction where the rate is proportional to the square of the concentration of one reactant.
Half-life
The length of time it takes for half of the reactant to be consumed.
Arrhenius Equation
An equation that shows the relationship between temperature and the rate constant.
Temperature Effect on Reaction Rate
Increasing temperature by 10°C often doubles the reaction rate for many reactions.
Surface Area
Increasing the surface area of a solid reactant increases the reaction rate by making more atoms accessible for collision.
Relative Rate Law
Comparative rate law used to compare the rate of 1 compound to another in the same reaction.
Reaction Energy Diagram
A graphical representation of the energy change during a chemical reaction, illustrating the activation energy.
Decreasing Reaction Rate
The reaction rate decreases over time due to the decreasing concentration of reactants.
Effective Collision
A collision that leads to the formation of products as reactants overcome the activation energy barrier.
Collision Frequency
The number of effective collisions that occur in a certain period of time.
Positive Rate Value
The rate of a reaction is always expressed as a positive value.
