In layman’s terms, equilibrium is defined as a state of balance due to equal reactions of opposing forces, and today we’ll be talking all about it with regards to the scientific study of chemistry, focusing on such topics as reaction rates. What can you tell us? Let’s find out.
Rates of chemical change are usually expressed as the amount of energy changing per unit time.
Rates of chemical change are usually expressed as the amount of non- reactant changing per unit time.
Rates of chemical change are usually expressed as the amount of reactant changing per unit time.
Reactant, product
Cataltyst, energy
Inhibitor, equilibrium
Collision theory states that the particles must have enough kinetic energy when they collide to form products.
Collision theory states that the particles must have enough potential energy when they collide to form products.
Collision theory states that the particles must have enough no kinetic energy when they collide to form products.
Reactant
Changed
Unchanged
Reactants
Activated complex
Products
Kinetic energy
Activation energy
Potential energy
Collision energy
Product
Reactant
Peak
10–15 s
10 13 s
10–13 s
10–1 s
It is called the transition state because an activated complex is unstable and is as likely to re-form reactants as it is to form products.
It is called the transition state because an activated complex is stable and is as likely to re-form reactants as it is to form products.
It is called the transition state because an activated complex is unstable and is as likely to re-form reactants as it is to form reactant.
Reactant, product, and activation
Temperature, concentration, and particle size
Collision, intervals, and kenetic energy
Increase
Decrease
Interpret
The concentration of reactants increases, the collision frequency increases, and, therefore, the reaction rate decreases.
The concentration of reactants increases, the collision frequency increases, and, therefore, the reaction rate increases.
The concentration of reactants decreases, the collision frequency increases, and, therefore, the reaction rate increases.
Absorbant of a particle.
Mass of a particle.
Release of a particle.
One way is to dissolve the solid; another way is to grind the solid into a fine powder.
One way is to leave it as a solid; another way is to make it into a liquid.
One way is to make into a vapor; another way is to change it into rough powder.
Product
Reactant
Catalyst
A catalyst permits reactions to proceed at a lower energy than is normally required. A catalyst lowers the activation energy.
A catalyst permits reactions to proceed at a higher energy than is normally required. A catalyst lowers the activation energy.
A catalyst permits reactions to proceed at a lower energy than is normally required. A catalyst raises the activation energy.
The catalyst is often written above the stop arrow in the equation.
The catalyst is often written below the yield arrow in the equation.
The catalyst is often written above the yield arrow in the equation.
Particle size
Reactant
Inhibitor
In reversible reactions, two opposite products occur simultaneously.
In reversible reactions, two opposite reactions occur simultaneously.
In reversible reactions, two of the same reactions occur simultaneously.
Not equal
Are equal
The same at some points
Pressure
Concentration
Temperature
3
6
9
Le Châtelier’s principle states that if a stress is applied to a system in dynamic no equilibrium, the system changes to relieve the stress.
Le Châtelier’s principle states that if a stress is applied to a system in dynamic equilibrium, the system changes to relieve the stress.
Le Châtelier’s principle states that if a stress is applied to a system in dynamic equilibrium, the system stays the same to relieve the stress.
Kentic, potinial, and reactants
Reactant, products, and balance
Concentration, pressure, and temperature.
Products
Reactants
Equilbrium