Transcript эритмалар. эритмалар назарияси. эритмаларнинг хоссалари

Department of Bioorganic and Biological Chemistry.
Bioinorganic chemistry
I COURSE
LECTURE 2.
THE CHEMICAL THERMODYNAMICS AND
BIOENERGETICS
LECTURER: Professor A.D.DZHURAEV
PURPOSE OF LECTURES:
• Give an idea of ​thermodynamics, noting the
universality of the laws of thermodynamics to
the animate and inanimate nature.
• Acquaint with the basic laws of
thermodynamics, to give an idea about the
systems and their types. Provide insight into
the relationship between the processes of
metabolism and energy in the body. To
familiarize with the laws of thermodynamics,
drawing attention to the irreversible processes
in the body.
THE LECTURE PURPOSE:
• The notion about laws of the thermodynamics
are given, as they universal for alive and not
alive nature. Must know, as it is filled up the
lost by organism energy in process of vital
activity, and what types of energy is act in
organism. The breach of the energy exchange
is a reason of the row of hard treatment
diseases of the person therefore physician must
know the mechanism of the transformation
different material in energy.
DEALT of questions
• The object and purpose of thermodynamics
• The value of the laws of thermodynamics in
medicine
• Thermodynamic
systems
and
thermodynamic parameters
• The internal energy
• The first law of thermodynamics
• Isobaric and isochoric heat effects
• Enthalpy
DEALT of questions
• Chemical Thermodynamics. thermal effects
• Hess's Law and its consequences
• The second law of thermodynamics
• Entropy and Free Energy
• Conditions of thermodynamic equilibrium
• Spontaneous thermodynamic processes and
conditions of their orientation
The subject of thermodynamics
Thermodynamics -- the science of the laws of
different types of energy transformation in each
other.
Its object of study - thermodynamic systems
Systems and their classification...
• Part of the space arbitrarily limited the interface from
the environment is called a system.
•
On the principle of exchange with the environment of
the system are:
• Open - exchange of matter and energy and
• Closed - only exchanged energy
• Isolated - do not share neither substance nor energy
Thermodynamic system and its internal
energy
• Any system characterized by the so-called state of
thermodynamic parameters - mass, volume, pressure,
temperature swarm, composition, specific heat, and
internal energy.
• The internal energy of the system - a combination of
all kinds of energy in the system.
•  U =  Ukinetic +  Upotential +  Uвн
 Uвн = U2 - U1
The first law of thermodynamics
• In any process of energy does not disappear
and does not appear out of nothing, it just
changes from one form to another in
equivalent amounts.
• The first law of thermodynamics, applied to
the activity of a living organism
• The chemical energy of metabolism is
transformed into other forms of energy and
allows the flow of the vital processes in the
body.
The mathematical expression of the first law
of thermodynamics
U = Q – A or Q = U + A
Where:
Q – the amount of heat
U – Changing the internal energy::
A - amount of work is done under the
effect of external forces
Chemical Thermodynamics
• Section thermodynamics studies of energy conversion
in chemical process called chemical thermodynamics
• Processes occur with heat are called exothermic
processes occur with the absorption of heat are called
endothermic
• The amount of heat absorbed or released in the
course of chemical reactions called the heat of
reaction.
Hess's Law
"The thermal effect of the chemical
reaction (enthalpy) depends on the type
and condition of the starting materials
and reaction products and not on the path
of transition from the initial to the final “
Q = Q1 + Q 2 = Q 3 + Q 4 + Q 5
Q1
Q2
Q
Q3
Q5
Q4
Hess's Law
Pb + S + 2O2 = PbSO4 + 919,7
I. Pb + S
= PbS + 94,5
II. PbS + 2O2 = PbSO4 + 825,2
919,7
The thermal effect of the isothermal
process
An isothermal process t = const, heat is transferred
from one body to another without changing the
temperature, than,
Q т = рV
Thermal effect isochoric process
Isochoric process when the volume is constant, than,
V = const
With unchanged quantities: V = 0
when work is not done: рV = 0
In such conditions, according to the first law of
thermodynamics, the total amount of heat supplied to
the system spent to increase the internal energy:
QV = U
Thermal effect of isobaric process
When the process of isobaric pressure is constant: P =
const
For such a state of expression for the first law of
thermodynamics Q =  U + р V is rewritten as
follows:
QP = U2 -U1 + р(V2 -V1) = U2 - U1 + рV2 -рV1
QP = (U2 + рV2) - (U1 - рV1)
The thermal effect at constant pressure is called the
enthalpy of the system and is denoted by H:
U + рV = H
then:
QP = H2 - H1 = H
Heat spent to increase its enthalpy
The second law of thermodynamics
The heat is not transferred
spontaneously from a cold to a hot
body, ie If any form of energy can be
converted into heat in the case of the
reverse transformation of heat into any
energy, complete conversion can not
be.
Entropy
Entropy is the ratio of the heat of reaction to the
absolute temperature, S = Q \ T
Logarithmic value of the thermodynamic
probability of a system is called entropy:S = k lgW
Here: S - entropy - disorder in the function of the
system;
k - Boltzmann constant
W - thermodynamic probability
Entropy. Standard entropy
The entropy determined at standard
conditions (T = 2980K,
p = 101.3 kPa) is called the absolute value
or the standard entropy and designated
S0 298
(∆S0 298) = ∑( S0 298)product - ∑( S0 298) outgoing
materials
Example calculation of standard entropy
С( ) + СО2 (g) = 2СО(g)
5,7 213,7
197,5
Standard entropy will be:
S0 298 = 2( S0 298) СО – [( S0 298)С + (S0 298)СО2] =
= 2 - 197,5 - ( 5,7 + 213,7) =175,6 joules (mol
K)
Gibbs energy.
1. Free energy - the energy that
can be converted into work
2. Bound energy - an energy that in the
process can not be converted into
job.
G = H - T * S or ΔG = ΔH - TΔS,
G - Gibbs energy
ΔH - enthalpy factor
TΔS - entropy factor
Parameters calculated for the direction and
feasibility of the thermodynamic process:
• ΔG <0 - spontaneous process, a transition of the
system from the initial state to the final
•
ΔG = 0 - the system in balance
•
ΔG> 0 - a transition from the initial to the final
• thermodynamic process: