ME3K Micro Project – Thermal Engineering TEG (313310)-Prepare Report on different laws of thermodynamic

PART
— A

Topic :- “Prepare Report on different laws of
thermodynamic”

AIM/BENEFITS OF THE MICROPROJECT :-

What is Thermodynamics?

The branch which deals with the
movement of energy from one form to the other and the relation between heat and temperature with energy and work done is called as
thermodynamics.
In other terms we can define
thermodynamics as the science stream that deals with the study of the combined
effects of heat and work on the changes of state of matter confined by the laws of
thermodynamics.

Chemical reactions which release
heat energy associated with it are converted into different usable forms based on the laws of
thermodynamics. The fact that energy can only be transformed from one form to the other
forms and its use in different industries is based on energy transformation. We are aware that
chemical reactions have energy associated with it. The laws of thermodynamics deal with
energy changes during a reaction and are not concerned with the rate at which
the reaction is proceeding.

Define Chemical Thermodynamics

Chemical thermodynamics is the
study of relation between work, heat and chemical reactions or with the physical changes of
the state which are confined to the laws of thermodynamics.

Some general
terms like heat, energy, and work were done are often used in thermodynamics. Let us learn a
bit about basic thermodynamics and understand these terms.

Internal Energy

It referred to the energy
content within the system. The energy represents the overall energy of the system and may include
many forms of energy such as potential energy, kinetic energy etc. In a chemical reaction,
we know about energy transformations and basic thermodynamics provides us with information
regarding energy change associated with the particles of the system.

State Functions Affecting Thermodynamics:

·       
Internal energy (U)

·         
Enthalpy (H)

·        
Entropy (S)

·           
Gibbs free energy (G)

There are four laws that govern
the thermodynamic systems’ phenomena, they are: Laws of
Thermodynamics

·            
First law of thermodynamics: When energy moves into or out
of a system, the system’s
internal energy changes in accordance with the law of conservation of mass.

·            
Second law of thermodynamics: The state of the entropy of the
entire universe, as an isolated system, will always increase over time.

·      
Third law of thermodynamics: Entropy of a perfect crystal at
absolute zero is zero. The laws of thermodynamics were the most important
lesson for people to understand the mechanism
behind the phase change of matter.

Frequently Asked Questions – FAQs

What are the basic concepts of thermodynamics?

Thermodynamics, the study of
heat, labor, temperature, and energy relationships. Thermodynamics is in general terms,
concerned with the transition of energy from one position to another and from one form to
another. The basic point is that heat is
an energy form
that corresponds to a specific amount of mechanical activity.

What is the purpose of thermodynamics?

•

The branch of physics concerned
with the interactions between heat and other sources of energy is thermodynamics. It
explains, in particular, how thermal energy is transferred into and from other sources of energy
and how it affects matter.

Who gave laws of thermodynamics?

Rudolf Clausius and William
Thomson (Kelvin) stated both the First Law – which preserves total energy – and the Second Law
of Thermodynamics around 1850. Initially, the second law was conceived in terms of the
fact that heat does not flow from a cooler body to a hotter one naturally.

How is thermodynamics used in everyday life?

The human body obeys
thermodynamic rules. It evaporates from the body as the sweat consumes more and
more heat, getting more disordered and adding
heat to the air, which heats up the room’s air temperature. Many sweaty people
in the “closed system” of a

crowded space will heat it up
fast.

What is the 2nd law of thermodynamics in simple terms?

The Second Law of Thermodynamics
notes that processes requiring heat energy transport or conversion are irreversible. … The
Second Law also notes that every isolated structure has a normal propensity to
degenerate into a more disordered state.

Factors Affecting the Internal Energy

The internal energy of a system may change when:

·                    
Heat passes into or out
of the system,

·     
Work is done on or by the system
or matter enters or leaves the system. Also Check = Internal
energy

Work

Work done by a system is defined as the quantity of
energy exchanged between a system and its
surroundings. Work is completely governed by external factors such as an
external force, pressure or volume or change in temperature etc.

Heat

Heat in thermodynamics is
defined as the kinetic energy of the molecules of the substance. Heat and the thermodynamics together form the basics which helped process designers and engineers to optimize their processes and harness the energy associated
with chemical reactions economically. Heat
energy flows from higher temperatures to lower temperatures.

systems in thermodynamic equilibrium. The laws also use
various parameters for thermodynamic processes, such
as thermodynamic work and heat, and establish relationships between them. They state
empirical facts that form a basis for precluding the possibility of certain
phenomena, such as perpetual motion. In addition to their use in thermodynamics, they
are important

fundamental laws of physics in
general, and are applicable in other natural sciences.
Traditionally,
thermodynamics has recognized three fundamental laws, simply named by an ordinal
identification, the first law, the second law, and the third law.⁰112]13] A more fundamental statement was later labeled as
the zeroth law, after the first three laws had been established.

The zeroth law of thermodynamics
defines thermal equilibrium and forms a basis for the definition of temperature: If two systems are each in thermal
equilibrium with a third
system, then they are in thermal equilibrium with each other.

The first law of thermodynamics
states that, when energy passes into or out of a system (as work, heat, or
matter), the system’s internal energy changes in accord with the law of conservation of
energy.

The second law of thermodynamics
states that in a natural thermodynamic process, the sum of the entropies of the interacting
thermodynamic systems never decreases. Another form of the statement is that heat
does not spontaneously pass from a colder body to a warmer body.

The third law of thermodynamics
states that a system’s entropy approaches a constant value as the temperature approaches
absolute zero. With the exception of non-crystalline solids (glasses) the entropy of a system
at absolute zero is typically

close to zero.’2′

The first and second law prohibit
two kinds of perpetual motion machines, respectively: the perpetual motion machine of
the first kind which produces work with no energy
input, and the perpetual motion machine of the second kind which spontaneously converts thermal
energy into mechanical work.

Contents

·             
1 History

·             
2Zeroth law

·              
3First law

·              
4Second law

·              
5Third law

·              
6Onsager relations

·              
7See also

·              
8References

·              
9Further reading

9.1
Introductory 0
9.2Advanced

·               
10External links

See also: Timeline of
thermodynamics and Philosophy of thermal and statistical physics The history of thermodynamics is
fundamentally interwoven with the history of physics and the history of
chemistry and ultimately dates to theories of heat in

antiquity. The laws of thermodynamics
are the result of progress made in this field over the nineteenth and early twentieth centuries.
The first established thermodynamic principle, which eventually became the
second law of thermodynamics,
was formulated by Sadi Carnot in 1824 in his book Reflections on the Motive Power of Fire. By 1860, as formalized in the works of
scientists such as Rudolf Clausius and William
Thomson, what are now known as the first and second laws were established. Later,
Nernst’s theorem (or Nernst’s postulate), which is now known as the third law, was formulated
by Walther Nernst over the period 1906-12. While the numbering of the laws is universal
today, various textbooks throughout the 20th century have numbered the laws
differently. In some fields, the second law was considered to deal with the efficiency of
heat engines only, whereas what was called the third law dealt with entropy
increases. Gradually, this resolved itself and a zeroth law was
later added to allow for a self-consistent definition of temperature. Additional laws
have been suggested, but have not achieved the  generality of the four accepted
laws, and are generally not discussed in standard

textbooks.

Zeroth law

The zeroth law of
thermodynamics provides for the foundation of temperature as an empirical parameter in thermodynamic systems and establishes the transitive relation between the
temperatures of multiple bodies in thermal equilibrium. The law may be stated in the following
form:

If two systems are both in
thermal equilibrium with a third system, then they are in
thermal
equilibrium with each other.

Though this version of the law is one of the most commonly stated
versions, it is only one of a diversity of statements that are labeled as
“the zeroth law”. Some statements go further,
so as to supply the important physical fact that temperature is and that one can conceptually arrange
bodies in a real number one dimension sequence from colder to hotter. These concepts of temperature and of thermal
equilibrium are fundamental to thermodynamics and were clearly stated in the nineteenth century.
The name zeroth Was invented by Ralph H. Fowler in the 1930s, long after the first, second, and
law

third laws were widely recognized. The law allows
the definition of temperature in a non-circular
way without reference to entropy, its conjugate variable. Such a temperature definition is said to be ’empirical`.

First
law

See also: Thermodynamic
cycle

The first law of thermodynamics is
a version of the law of conservation of energy adapted f_or thermodynamic processes. In general, the conservation law states that the total energy of an isolated
system is constant; energy can be transformed from one form the another but can be neither created nor
destroyed.

 In a closed system (i.e. there is no transfer of matter into or
out of the system), the first law states that the change in internal energy of
the system (AU,,,,e,„) is equal to the difference between the heat supplied to the system (Q) and the work done by the
system on its surroundings. (Note, an alternate sign convention, not used in this article, is to define Was the work
done on the system by its surroundings):

For processes that include
transfer of matter, a further statement is needed.

When two initially isolated
systems are combined into a new system, then the total internal energy of
the new system, will be equal
to the sum of the internal energies of the
two initial systems, U, and U2:

The First Law encompasses
several principles:

The Conservation of energy,
which says that energy can be neither created nor destroyed but can only change form. A
particular consequence of this is that the total energy of an isolated system
does not change.

The concept of internal energy and its relationship
to temperature. If a system has a definite temperature,
then its total energy has three distinguishable components, termed kinetic energy (energy due to the motion of the system as
a whole), potential energy (energy resulting
from an externally imposed force field), and internal energy. The establishment
of the concept of internal energy
distinguishes the first law of thermodynamics from the more general law of conservation of energy.

Work is a process of
transferring energy to or from a system in ways that can be described by macroscopic mechanical
forces acting between the system and its surroundings. The work done by the system can come
from its overall kinetic energy, from its overall potential energy, or from its internal
energy.

For example, when a machine (not
a part of the system) lifts a system upwards, some

energy is transferred from the
machine to the system. The system’s energy increases as work
is done on the system and in this particular case, the energy increase of the
system is manifested as an
increase in the system’s gravitational
potential energy. Work added to the system increases the potential energy of the system:

When
matter is transferred into a
system, that masses’ associated internal energy and potential energy are transferred with it. where u denotes the internal energy per unit mass of the
transferred matter, as measured while in the surroundings; and AM denotes the amount of transferred mass.

The flow of heat is a form of energy transfer. Heating
is the natural process of moving energy to or from a system other
than by work or the transfer of matter. In

a
diathermal system, the internal energy can only be changed by the transfer of
energy as heat:

.

Second
law

        processes
to lead towards spatial homogeneity of
matter and energy, and especially of temperature. It can be formulated in a variety of interesting and important
ways. One of the simplest is the Clausius
statement, that heat does not spontaneously pass from a colder to a hotter

body-

It implies the existence of a quantity called the entropy of a thermodynamic system. In terms of this quantity it
implies that

When two initially isolated systems in separate but
nearby regions
of space, each in thermodynamic equilibrium with itself but not
necessarily with each other, are then allowed to
interact, they will eventually reach a mutual thermodynamic equilibrium.

The
sum of the entropies of the initially isolated systems is less than or equal to the total entropy of the final combination. Equality occurs just
when the two original systems have all their respective intensive variables
(temperature, pressure) equal; then the final system also has
the same values.

The
second law is applicable to a wide variety of processes, both reversible and
irreversible. According to the second law, in a reversible heat transfer, an
element of heat transferred, 5Q, is the product of the temperature (T), both of the system and of the sources or destination of the heat, with the
increment (dS) of the system’s conjugate
variable, its entropy (S):

While reversible processes are a useful and convenient
theoretical limiting case, all natural processes are
irreversible. A prime example of this irreversibility is the transfer
of heat by conduction or radiation. It was known long
before the discovery of the notion of entropy that when two bodies, initially of different
temperatures, come into direct thermal
connection, then heat immediately and spontaneously flows from the
hotter body to the colder one.Entropy may also be viewed as a physical measure
concerning the microscopic details of the motion and
configuration of a system, when only the macroscopic _mates are
known. Such details are often referred to as disorder on a microscopic or macroscopically
scale, and less often as dispersal of
energy. For two givens macroscopically specified
states of a system, there is a mathematically defined how called the ‘difference of information entropy
between them. This defines how much additional microscopic physical information is needed to specify one of e macroscopically specified states, given the macroscopic specification of the other often a conveniently chosen reference state which may be presupposed to exist rather than explicitly stated. A
final condition of a natural process always contains microscopically effects that are not fully and exactly predictable from the macroscopic specification of the initial condition of
the process. why entropy-

  increase s in natural processes the increase tells how much extra microscopic information is needed to distinguish the initial macroscopically
specified state from the final macroscopically specified state Equivalently, in a thermodynamic process, energy spreads.