Test #3 Kinetics, Equilibrium, and Acids and Bases Flashcards
Define Kinetics.
The study of the factors that affect reaction rates and the mechanism by which the reaction proceeds.
Define reaction rate.
The change in concentration of a reactant within a given period of time.
The concentration of reactants ____ over time.
Decreases
The concentration of products ____ overtime.
Increase
What are the factors that affects rate?
Physical state of reactants.
Concentration of reactants(the higher the concentration, the more likely of collision; faster reaction).
Reaction temperature(increase temp, increases the kinetic energy).
Catalysts(substances used to speed up reactions but not consumed by the reaction).
What are the kinetic relationships?
Rate and stoichiometry.
Rate and concentration.
Concentration and time.
Rate and temperature.
Define rate and concentration.
Effect of concentration on rate of a reaction can be expressed using rate laws.
What does Le Chatlier’s Principle states?
If a system at equilibrium is disturbed, the equilibrium will shift in a way that will counteract the disturbance and re-establish equilibrium.
Equilibrium can be disturbed in three ways:
Addition or removal of a product or reactant.
Change in pressure.
Change in temperature.
What are equilibrium constants?
Used to describe the ratios of products to reactants at equilibrium.
Derived from a balanced chemical reaction.
Can be used to determine the favored direction of a reaction.
If Kc>1 what is favored?
Foward reaction
If Kc<1 what is favored?
Reverse reaction
What are some rules of heterogeneous equilibrium?
Not all substances are the same state of matter.
Solids and pure liquids are not included in the equilibrium constant expression.
Gases and aqueous solutions are included in the equilibrium constant expression.
Generally the rate of reaction is directly propotional to the concentration of reactants. Why is that?
Collisons
Rate and Concentration
0 Order: rate independent of [A].
Rate law: rate=k[A]0
1st Order: rate directly proportional to [A].
Rate law: Rate=k[A]1
2nd Order: rate proportional to [A]2.
Rate law: Rate=k[A]2
