Equilibrium
Equilibrium Stress
Kinetics
Graphing/Figures
Random
100
What defines dynamic equilibrium in IB Chemistry?
The rate of the forward reaction equals the rate of the reverse reaction.
100
What principle predicts how equilibrium responds to stress?
Le Chatelier’s principle.
100
What is the IB definition of reaction rate?
Change in concentration per unit time.
100
At equilibrium, is the reaction product or reactant favored?
Product favored
100
Dynamic equilibrium must occur in a _________ system.
Closed
200
In a closed system at equilibrium, what happens to concentrations?
They remain constant.
200
What happens to equilibrium if you remove a product?
Equilibrium shifts toward products.
200
What theory explains reaction rate in IB Chemistry?
Collision Theory
200
Is this reaction exothermic or endothermic?
Exothermic.
200
What is the value of ΔH for an exothermic reaction?
Negative
300
What does the equilibrium constant (Kc) measure conceptually?
The position of equilibrium.
300
Increasing concentration of products causes equilibrium to…
shift toward the reactants.
300
What makes a collision successful?
Correct orientation and energy ≥ activation energy.
300
Which sample has a lower molecular mass?
Y. With a lower mass, more particles will have a higher velocity (more spread out Maxwell-Boltzmann distribution).
300
What is the only factor that changes K (equilibrium constant)?
Temperature
400
What happens to equilibrium when a catalyst is introduced?
Equilibrium is reached faster. The equilibrium itself does not shift or change.
400
In an exothermic reaction, increasing the temperature causes the equilibrium to...
shift towards the reactants.
400
What does increasing temperature do to rate?
Increases frequency of successful collisions.
400
What does "n" represent on the energy profile diagram?
Activation energy when a catalyst is introduced.
400
Explain equilibrium at a particle level for a reaction with a K value of 4.2 x 10^34.
At equilibrium, the reaction consists of majority products with a negligible amount of reactants.
500
How do you construct a Kc expression (IB wording)?
Concentration of products divided by concentration of reactants, each raised to stoichiometric coefficients.
500
Increasing pressure shifts equilibrium toward…
The side with fewer moles of gas.
500
How does a catalyst speed up a reaction?
Decreases activation energy so more particles have enough energy to college and form products.
500
At equilibrium, would you expect the equilibrium constant to be less than, equal to, or greater than 1?
Reactant favored. K is less than 1.
500
When using Hess's Law for equilibrium, if you have to flip an equation, what do you do with the K value?
Inverse of K.