Chapter 6.1 Flashcards
1
Q
What is the difference between dynamic equilibrium reactions and static equilibrium reactions
A
Dynamic equilibrium
- > forward and reverse reactions are still occurring
- > these reactions are occurring at the same rate so there is no net change in the concentrations of the products or reactants
Static equilibrium
->forward and reverse reactions have stopped occurring
2
Q
What is the relationship between equilibrium, entropy and Gibbs free energy
A
-equilibrium will be reached when the systems entropy is at a maximum, and the Gibbs free energy is at a minimum
3
Q
What is the point of the reaction quotient
A
- it tells you about the timing of the reaction
- > whether it has proceeded to equilibrium or not
- > also allows you to calculate the concentration of all the reactants and products during any time during a reaction
4
Q
Describe the relation of Q to Keq and how that describes the position of the reaction
A
- Qgreater concentration of reactants and smaller concentration of products
- > the forward rate of the reaction needs to be increased to restore equilibrium
- Q=Keq, then the reaction is in dynamic equilibrium
- > reactants and products are present in equilibrium proportions
- > the forward and reverse rates of the reaction are equal
- Q>Keq, then the forward reaction has exceed equilibrium
- > there is a greater concentration of products than at equilibrium
- > the reverse rate of the reaction is increased to restore equilibrium
5
Q
Is the equilibrium constant temperature dependent
A
- yes
- > Keq is a characteristic of a particular reaction at a given temperature
- > the larger the value of Keq, the farther right to the equilibrium position
