its about power plants

1. Power Plants
Dr Gordhan Das Valasai
01

2. Power Plants
Contact Hours Hours Credit Hours
Theory 48 Theory 3.0
Teaching Methodology Assessment
1. Lecturing
2. Written Assignments
3. Field Visits
4. Report Writing
1. Mid Exam
2. Final Exam
3. Quizzes
4. Assignments
5. Presentation

3. Power Plants
Objectives:
• To provide knowledge to the students about energy processes
involved in transformation and analysis of power plants.
• To provide knowledge to the students about the efficiencies and
environmental aspects of various processes in different power
plants.
• To provide the knowledge to the students about the steps of the
complete energy production.

4. Power Plants
Course Outcome:
Upon successful completion of the course, the student will be able to:
S. No. CLO Domain Taxonomy
Level
PLO
1. Review different energy resources,
environmental impacts of power generation
and flue gas cleaning techniques
Cognitive 2 7
2. Analyze strengths and weaknesses of
different types of power plants by
performing its thermodynamic calculations
Cognitive 4 2
3. Illustrate the construction and operation of
different components of a power plant.
Cognitive 4 2
4. Design of the major components or
systems of a conventional or alternative Cognitive 5 3

5. Course Contents
Chapter Contents
Introduction Review of mass and energy balances for
steady flow devices, energy sources and
classification; Fossil fuels; composition,
ranking and analysis; combustion
calculations; environmental pollution
Steam
Generators and
Turbines
Combustion equipment and firing
methods, boiler types and their
applications; boiler components, boiler
operation and safety, water treatment.
Impulse and reaction turbines; Pressure
and Velocity Compounding, Turbine
governing and controls
Steam
Powerplants
Rankine Cycle, Superheat, Reheat;
Regenerative Cycle, Open Type Feed
Water Heaters (FWH), Closed Type FWHs
with Drains Cascaded Backwards and
Pumped Forward
Gas Turbine
Powerplants
Gas turbine (Brayton) cycle,
regeneration, intercooling
Chapter Contents
Combined Cycle
Powerplants
Topping and bottoming cycles, combined
cycle efficiency
Cogeneration Cogeneration of power and process heat,
Back Pressure and Extraction Turbines
Diesel Engine
Powerplant
General layout, Site selection criterion,
performance characteristics &
environmental impact consideration
Nuclear Power
Plant
Nuclear fuels, nuclear reaction types,
Components, reactor types, site selection
criterion, safety and environmental
consideration
Renewable Energy
Powerplants
Introduction to Solar, Wind, Hydro and
Geothermal Powerplants
Powerplant
Economics and
Management
Effect of variable load, load curve,
economics of thermal power plants, energy
conservation and management

6. Text and Reference books:
1. El-Wakil, M.M., Power Plant Technology, McGraw-Hill
2. I. Dincer, C. Zamfirescu, Advanced Power generation systems, Elseveir
3. Larry Drbal, Pat Boston, “Powerplant Engineering”, CBS Publishers
4. Black, Veatch, “Power Plant Engineering”, Springer.
5. P.K. Nag, “Power Plant Engineering”, McGraw-Hill.
6. Everett Woodruff, Herbert Lammers, Thomas Lammers, “Steam Plant Operation”,
McGraw-Hill.
7. Thomas Elliott, Kao Chen, Robert Swanekamp, Handbook of Powerplant
Engineering”, McGraw-Hill.
8. Pedersen, E.S., Nuclear Power, Ann Arbor Science

7. • The name thermodynamics is derived from the Greek words therme
(heat) and dynamis (power), which is most descriptive of the early
efforts to convert heat into power.
• Today the same name is broadly interpreted to include all aspects of
energy and energy transformations, including power generation,
refrigeration, and relationships among the properties of matter.
Thermodynamics

8. • One of the most fundamental laws of
nature is the conservation of energy
principle.
• It simply states that during an interaction,
energy can change from one form to
another but the total amount of energy
remains constant.
• That is, energy cannot be created or
destroyed.
Thermodynamics

9. • Heat flows from higher temperature to
lower temperature.
Thermodynamics

10. • A system is defined as a quantity of
matter or a region in space chosen for
study.
• The mass or region outside the
system is called the surroundings.
• The real or imaginary surface that
separates the system from its
surroundings is called the boundary.
• The boundary of a system can be
fixed or movable.
• The boundary is the contact surface
shared by both the system and the
surroundings.
Thermodynamics

11. • Systems may be considered to be
closed or open, depending on whether
a fixed mass or a fixed volume in
space is chosen for study.
• A closed system (also known as a
control mass) consists of a fixed
amount of mass, and no mass can
cross its boundary.
• That is, no mass can enter or leave a
closed system.
Thermodynamics

12. • An open system is one in which matter
flows into or out of the system.
• Most of the engineering systems are
open.
• An open system, or a control volume, as
it is often called, is a properly selected
region in space. It usually encloses a
device that involves mass flow such as a
compressor, turbine, or nozzle.
• Flow through these devices is best
studied by selecting the region within the
device as the control volume.
• Both mass and energy can cross the
boundary of a control volume.
Thermodynamics

13. • Properties: Any characteristic of a system
is called a property. Some familiar
properties are pressure P, temperature T,
volume V, and mass m.
• Properties are considered to be either
intensive or extensive.
• Intensive properties are those that are
independent of the mass of a system,
such as temperature, pressure, and
density.
• Extensive properties are those whose
values depend on the size—or extent—of
the system.
Thermodynamics

14. • Consider a system not undergoing any change. At this point, all the
properties can be measured or calculated throughout the entire
system, which gives us a set of properties that completely describes
the condition, or the state, of the system.
• A system in equilibrium experiences no changes when it is isolated
from its surroundings.
• A system is in thermal equilibrium if the temperature is the same
throughout the entire system.
• Mechanical equilibrium is related to pressure, and a system is in
mechanical equilibrium if there is no change in pressure at any point of
the system with time.
State & Equilibrium

15. • Any change that a system undergoes
from one equilibrium state to another is
called a process, and the series of
states through which a system passes
during a process is called the path of
the process
Processes & Cycles

16. • When a process proceeds in such a
manner that the system remains
infinitesimally close to an equilibrium
state at all times, it is called a quasi-
static, or quasi-equilibrium, process.
• Opposite to above process is called as
nonquasi-equilibrium.
Processes & Cycles

17. • The prefix iso- is often used to designate a process for which a
particular property remains constant.
• An isothermal process, for example, is a process during which the
temperature T remains constant;
• an isobaric process is a process during which the pressure P remains
constant;
• and an isochoric (or isometric) process is a process during which the
specific volume v remains constant.
Processes

18. • Any process or series of processes whose
end states are identical is termed a cycle.
• The processes through which the system
has passed can be shown on a state
diagram, but a complete section of the path
requires in addition a statement of the heat
and work crossing the boundary of the
system.
• A cycle in which a system commencing at
condition ‘1’ changes in pressure and
volume through a path 123 and returns to its
initial condition ‘1’.
Cycle

19. • If A is in thermal equilibrium with B and if B is in thermal equilibrium with C,
then A is in thermal equilibrium with C .
• If two systems are in thermal equilibrium with a third system, then they are in
thermal equilibrium with each other.
Zero’th Law of Thermodynamics

20. • When a system undergoes a thermodynamic cycle then the net heat supplied
to the system from the surroundings is equal to net work done by the system
on its surroundings.
• Heat and work are mutually convertible but since energy can neither be
created nor destroyed, the total energy associated with an energy conversion
remains constant.
• Energy Balance: The net change (increase or decrease) in the total energy of
the system during a process is equal to the difference between the total energy
entering and the total energy leaving the system during that process.
First Law of Thermodynamics
+

21. • Heat can never pass from a colder to a warmer body without some other
change, connected therewith, occurring at the same time or heat can not be
completely and continuously converted to work.
• Aspects of second law of thermodynamics:
Second Law of Thermodynamics

22. • “After your hands become coated with grease, your nose will
begin to itch.”
Law of Mechanical Repair

23. • The ideal gas law, also called the general gas equation, is the
equation of state of a hypothetical ideal gas. It is a good
approximation of the behavior of many gases under many
conditions, although it has several limitations.
• Ideal gas molecules do not attract or repel each other.
• Ideal gas molecules themselves take up no volume.
• Where P is the pressure of the gas, V is the volume taken up by
the gas, T is the temperature of the gas, R is the gas constant,
and n is the number of moles of the gas.
Ideal Gas
PV =nRT

24. • The specific heat capacity of a solid or liquid is usually defined as; the heat
required to raise unit mass through one degree temperature rise.
• Where m is the mass, is the increase in temperature, and c is the specific heat
capacity.
• For a gas there are an infinite number of ways in which heat may be added
between two temperatures, and hence a gas could have an infinite number of
specific heat capacities.
• However, only two specific heat capacities for gases are defined; the specific
heat capacity at constant volume and the specific heat capacity at constant
pressure. We can write above equation
Specific Heat
𝛥Q=mc 𝛥T

25. • For a perfect gas, the values of Cp and Cv are constant for any one gas at all
pressures and temperatures. Hence integrating above equations, we have for a
reversible constant process
• For real gases, Cp and Cv vary with temperature, but for most practical
purposes a suitable average value may be used.
Specific Heat
𝛥Q=m𝑐𝑝 𝛥T 𝛥Q=m𝑐𝑣 𝛥T
- 𝛥Q=m𝑐𝑣(𝑇¿¿2− 𝑇1)¿