5. Equilibrium
Equilibrium is a state in which there are no
observable changes as time goes by.
Chemical equilibrium is achieved when:
1.) the rates of the forward and reverse
reactions are equal and
2.) the concentrations of the reactants
and products remain constant
6. Equilibrium
There are two types of equilibrium:
Physical and Chemical.
Physical Equilibrium: Equilibrium between two
phases of the same substance. Changes that occur are
physical.
Chemical Equilibrium: Chemical equilibrium is
the point at which the rate of the forward reaction is
equal to the rate of the reverse reaction.
9. Definition of phase:
Any part of a system which is physically separated
from other parts of the system by a distinct boundary.
A phase can be a solid, liquid, vapour (gas) or aqueous
solution which is uniform in both chemical constitution
and physical state.
10. Phase Equilibrium:
A phase equilibrium is a balance between phases, that is
the coexistence of two or more phases in a state of dynamic
equilibrium.
11. Heterogeneous system ---- system with more than one phase
Homogeneous system ---- system consists of one phase only
Example of Phase Equilibrium:
12. Homogeneous:
The prefix “homo” – indicate sameness
Homogeneous – A homogeneous mixture
has the same uniform appearance
throughout
13. Heterogeneous:
The prefix “hetero” – indicate difference
Heterogeneous - A heterogeneous mixture
consists of visibly different substances or
phases.
14. PHASE
system
1) The mixture of ice and water = have two
phase which is solid and liquid
2) The mixture of oxygen gas and nitrogen
gas = have one phase which is gas
phase (the system is homogen)
3) The mixture of oil and water = have 2
same phase(liquid). Oil and water are
not homogen and have the boundaries to
separate both phase
4) CaCO3(s) CaO(s) + CO2(g)
= 3 phase (2 solid,1 gas)
Heterogeneous system
Heterogeneous system
Heterogeneous system
Homogeneous system
EXAMPLES of