CHM101(3) – General Physical Chemistry
Atoms, Dalton’s Atomic Theory and Atomic Masses, Fundamental
particles of the Atom and Atomic structure, Modern electronic theory of
atoms; Periodicity of the elements, Mole concept, Chemical formulae
equations and calculations, States of matter: gas, liquid and solid,
Energetics and Thermochemistry, Chemical kinetics, Equilibria and
Electrochemistry
Dr. S.O. Owalude
45h (T), C
1
, CHEMICAL KINETICS
The study of chemical phenomenon can be approached from two
angles, THERMODYNAMICS and CHEMICAL KINETICS.
THERMODYNAMICS involves the driving potential which is a
measure of the tendency of a system to change from one state to
another.
CHEMICAL KINETICS deals with the rate of change from initial to
final state under non-equilibrium conditions.
The ultimate goal of chemical kinetics is a theory interrelating
energies, structures and time for the single chemical event.
2
, Slow and fast reactions
(a) Slow reactions: these are reactions that proceed slowly and
their rates can be measured by conventional methods.
Example:
C12H22O11 + H2O C6H12O6 + C6H12O6
(b) Fast reactions: The rates of these reactions are too fast to be
measured by conventional methods. The half-lives of such
reactions are less than I second.
Example:
i. Organic substitution reactions
ii. Explosive reactions of O2 and H2 and HCs
iii. Many ionic reactions such as the neutralization of acids and
bases. 3
, REACTION RATES
The rate of a chemical reaction is defined as the change in
concentration of a reactant in a particular time interval.
The units of reaction rate are unit of concentration divided by the
unit of time.
Since concentration is normally measured in moles per liter (mol
L-1), the rate of reaction is specified as mol L-1 s-1 and if the time is
measured in minutes, the rate will become mol L-1 min-1.
Example:
2N2O5(s) 4NO2(g) + O2(g)
The rate for this reaction can be determined by measuring the
increase in the molar concentration of O2 in a given time interval.
4
Atoms, Dalton’s Atomic Theory and Atomic Masses, Fundamental
particles of the Atom and Atomic structure, Modern electronic theory of
atoms; Periodicity of the elements, Mole concept, Chemical formulae
equations and calculations, States of matter: gas, liquid and solid,
Energetics and Thermochemistry, Chemical kinetics, Equilibria and
Electrochemistry
Dr. S.O. Owalude
45h (T), C
1
, CHEMICAL KINETICS
The study of chemical phenomenon can be approached from two
angles, THERMODYNAMICS and CHEMICAL KINETICS.
THERMODYNAMICS involves the driving potential which is a
measure of the tendency of a system to change from one state to
another.
CHEMICAL KINETICS deals with the rate of change from initial to
final state under non-equilibrium conditions.
The ultimate goal of chemical kinetics is a theory interrelating
energies, structures and time for the single chemical event.
2
, Slow and fast reactions
(a) Slow reactions: these are reactions that proceed slowly and
their rates can be measured by conventional methods.
Example:
C12H22O11 + H2O C6H12O6 + C6H12O6
(b) Fast reactions: The rates of these reactions are too fast to be
measured by conventional methods. The half-lives of such
reactions are less than I second.
Example:
i. Organic substitution reactions
ii. Explosive reactions of O2 and H2 and HCs
iii. Many ionic reactions such as the neutralization of acids and
bases. 3
, REACTION RATES
The rate of a chemical reaction is defined as the change in
concentration of a reactant in a particular time interval.
The units of reaction rate are unit of concentration divided by the
unit of time.
Since concentration is normally measured in moles per liter (mol
L-1), the rate of reaction is specified as mol L-1 s-1 and if the time is
measured in minutes, the rate will become mol L-1 min-1.
Example:
2N2O5(s) 4NO2(g) + O2(g)
The rate for this reaction can be determined by measuring the
increase in the molar concentration of O2 in a given time interval.
4
