Document 6538359

Sample learning out come of the Course
ME-103 Thermodynamics
SECTION-1
Introduction to Thermodynamics
Contents
1.1
Thermodynamics and its applications.
1.2
Closed and open system.
1.3
Forms of energies.
1.4
Properties of a system.
1.5
State and equilibrium.
1.6
Processes and cycles.
1.7
Zeroth law of thermodynamics.
1.8
Absolute temperature scales.
Learning outcomes
Students should be to:
•
appreciate that thermodynamics is a science of energy considering its all aspects and
transformations.
•
understand the microscopic and macroscopic approaches of thermodynamics.
•
understand and define the following terms: thermodynamic system, surrounding,
boundary, closed system, open system, isolated system, control mass, and control
volume.
•
distinguish between static and dynamic forms of energy with examples.
•
understand what is meant by sensible and latent energy.
•
appreciate that internal energy of a system is the sum of all forms of microscopic
energies.
•
distinguish between extensive and intensive properties with examples.
•
understand what is meant by process and path of the process and be able to define
isothermal, isobaric, isochoric processes.
•
understand what is meant by thermodynamic equilibrium and not to be confused with
the thermal equilibrium.
•
understand the quasi-static process.
•
appreciate what is meant by simple compressible system.
•
understand the state postulate according to which the state of a system is completely
specified by two independent intensive properties.
•
appreciate the significance of zeroth law of thermodynamics in temperature
measurement.
•
understand that thermodynamic scale of temperature is independent of the properties of
the system.
•
appreciate that Kelvin and Rankine are the two absolute scales of temperature in SI and
English system of units respectively.
SECTION-2
Properties of pure substances
Contents
2.1
Pure substance.
2.2
Phase change of pure substances.
2.3
Property diagrams for phase change processes.
2.4
Property tables.
Learning outcomes
Students should be able to:
•
define pure substance with examples.
•
understand evaporation and boiling phenomena including the factors effecting and
should appreciate that evaporation causes cooling while boiling depends on the ambient
pressure.
•
explain what is meant by saturated liquid, compressed liquid, saturated vapor and super
heated vapor and be able to identify them on T-v and P-v diagrams.
•
appreciate that during a phase change process the temperature and pressure of a pure
substance are dependent properties.
•
recall what is meant by the term quality of saturated liquid-vapor mixture.
•
appreciate that in the absence of compressed liquid data in a table a general
approximation is to treat compressed liquid as a saturated liquid at given temperature
not pressure.
•
understand what is meant by a critical point and the temperature above the critical point
a phase change process cannot be proceeded by pressure only.
•
understand that at triple point pressure and temperature, a pure substance exist in three
phases in equilibrium.
•
read the steam table.
•
Interpolate the data using linear interpolation.
•
calculate the properties in a saturated mixture using the equation y = y f + xy fg where ‘y’
is any arbitrary property and ‘x’ is its quality in the saturation region.
SECTION-3
First Law of Thermodynamics
Contents
3.1
Heat and work transfer.
3.2
First law of thermodynamics in closed system.
3.3
Conservation of mass principle.
3.4
Conservation of energy principle.
3.5
Steady flow process.
3.6
First law of thermodynamics in open system.
Learning outcomes
Students should be able to:
•
appreciate that the first law of thermodynamics is more than the law of conservation of
energy because it asserts that the total energy is a thermodynamic property.
•
understand that heat and work are energies in transition i.e. a boundary phenomenon.
•
understand that the magnitude of heat and work depend on the path followed by the
process i.e. a path function.
•
understand that the work transfer can change the energy content of an adiabatic
system.
•
understand that the area under the process curve on a P-v diagram represent the
boundary work.
•
calculate the boundary work using Wb = ∫ pdV .
•
understand that for a cyclic process the change in the energy content is zero.
•
understand that mass and energy of the universe is constant.
•
appreciate that first law for closed system in differential form is written as δq - δw = de
i.e. heat and work expressed by inexact differentials.
•
understand the sign convention for heat and work transfer while solving problem using
first law of thermodynamics.
•
understand that during a steady flow processes the fluid flow through the control volume
experiencing no change with time at a fixed position.
•
appreciate that nozzle, diffuser, turbine and compressor are steady flow engineering
devices.
•
solve problems using steady flow energy equation q – w = ∆h + ∆ke + ∆pe .
SECTION-4
Second law of Thermodynamics
Contents
4.1
Thermal energy reservoir.
4.2
Kelvin and Clausius statements of second law of thermodynamics.
4.3
Heat engines.
4.4
Refrigerators.
4.5
Reversible and irreversible processes.
4.6
Carnot cycle.
4.7
Perpetual motion machine.
Learning outcomes
Students should be able to:
•
appreciate that thermal energy reservoirs are the hypothetical bodies having large
thermal energy capacity i.e. can supply or absorb heat without undergoing any change
in temperature.
•
understand the terms source and sink.
•
define the Kelvin and Clausius statements of second law of thermodynamics.
•
appreciate that a process will not occur unless it satisfies both the first and the second
law of thermodynamics.
•
appreciate that heat engines are the devices which convert heat energy into mechanical
work.
•
recognize the difference between refrigerator and heat pump.
•
appreciate that any device, which violate the first or second law of thermodynamics is
called perpetual motion machine.
•
calculate the thermal efficiency and the COP of heat engine and refrigerators.
•
understand the terms internally, externally and totally reversible processes.
•
list the factors causing irreversibility in the process.
•
appreciate that a reversible processes does not occur in nature.
•
describe the four reversible processes of Carnot cycle on a P-v diagram.
•
appreciate that reversed Carnot cycle is known as the Carnot refrigeration cycle.
SECTION-5
Entropy
Content
5.1
Clausius inequality.
5.2
Entropy.
5.3
Increase of entropy principle.
5.4
Property diagrams involving entropy.
5.5
Third law of thermodynamics.
5.6
Entropy as a measure of disorder.
Learning outcomes
Students should be able to:
•
state the Clausius inequality i.e. the cyclic integral of δQ / T is always less than or equal
to zero.
•
appreciate that any process violates clausius inequality will also violate the second law
of thermodynamics or vice versa.
•
appreciate that entropy is a thermodynamic property, which is a consequence of second
law of thermodynamics just like total energy content is a consequence of first law of
thermodynamics.
•
understand that an isentropic process is an adiabatic and a reversible process.
•
understand that on a T-s diagram the area under the process curve represent the heat
transfer for internally reversible process.
•
describe the Mollier chart, which is an h-s diagram.
•
understand that ∆S ≥ ∫ (δQ/T) is a mathematical form of second law of thermodynamics.
•
appreciate that entropy of an isolated system always increases.
•
define the third law of thermodynamics.
SECTION-6
Ideal gas behavior
Contents
6.1
Ideal gas equation of state.
6.2
Specific heats.
6.3
Specific heat of ideal gas.
6.4
Isentropic relationship for ideal gases.
Learning outcomes
Students should be able to:
•
understand what is meant by equation of state.
•
understand that Pv=nRT is one of the equation of state for an ideal gas.
•
appreciate that real gas at low densities, low pressures and high temperature exhibit
ideal gas behavior.
•
understand that vapor and refrigerants cannot be treated as an ideal gas.
•
define heat capacity and specific heat capacity.
•
express specific heats Cv and Cp in terms of thermodynamic properties.
•
recognize that Cv and Cp are the measure of variation in internal energy and enthalpy of
a substance with temperature respectively.
•
recognize that units for specific heats kJ/kg°C and kJ/kgK are identical.
•
appreciate that for ideal gases u, h, Cp and Cv are functions of temperature only.
•
understand the following isentropic relations T2 =  V1 
T1  V2 
k −1
T P 
and 2 =  2 
T1  P1 
k −1
k
where k is the
ratio of specific heats, and appreciate that these relations are only valid for ideal gas,
isentropic process and constant specific heats.
SECTION-7
AVAILABILITY
Contents
7.1
Availability
7.2
Reversible work and Irreversibility.
7.3
Second law efficiency.
Learning outcomes
Students should be able to:
•
define availability or exergy.
•
appreciate that availability is a property of a system-surrounding combination not only of
the system alone.
•
appreciate that energy is a conserved property, what is not conserved is availability.
•
define and understand the terms dead state, surrounding work, useful work, reversible
work and irreversibility.
•
recall that irreversibility for any system closed or open system is the difference between
reversible and useful work.
•
calculate the reversible work, irreversibility and the second law efficiency in simple
problems.
•
appreciate that second law efficiency is the measure of the performance of a device
relative to its performance under reversible conditions.
•
appreciate the aspects of second law of thermodynamics in daily life.
SECTION-8
POWER CYCLES
Contents
8.1
Otto cycle
8.2
Diesel cycle.
8.3
Dual combustion cycle.
8.4
Rankine cycle
Learning outcomes
Students should be able to:
•
state the air-standard assumptions and the cold-air-standard assumptions.
•
know the terms regarding reciprocating engines like TDC, BDC, clearance volume,
compression ratio, and mean effective pressure.
•
understand that mean effective pressure is a parameter used to compare the
performances of reciprocating engines of equal size.
•
classify engines as SI, CI, two stroke and four stroke engines.
•
draw the P-v and T-s diagrams for Otto, diesel, and dual combustion cycles.
•
solve the numericals calculating the thermal efficiency, amount of heat transfer, mean
effective pressure, and the highest temperature and pressure in the cycles (Otto, diesel,
dual) assuming constant specific heats (exclude problems involving the variation of
specific heat with temperature).
•
appreciate that the thermal efficiency of ideal Otto cycle is a function of compression
ratio and specific heat ratios.
•
derive the expressions for thermal efficiency of Otto and Diesel cycle ηth ,otto = 1 −
ηth ,diesel = 1 −
1
r k −1
,
1  rc k − 1 

.
r k −1  k (rc − 1) 
•
sketch the schematic diagram for simple Rankine cycle showing its four main
components i.e. boiler, turbine, condenser, and pump.
•
understand that lowering the condenser pressure; increasing the boiler pressure and
superheating the steam to high temperatures can increase efficiency of the rankine
cycle.
•
sketch the T-s diagram for rankine cycle showing the constant pressure lines.
•
solve the numericals on simple Rankine cycle, calculating the thermal efficiency, quality
of steam, mass flow rate of the steam, heat supplied, heat rejected and pump work.
SECTION-9
Reciprocating Compressors
Contents
9.1
Reciprocating compressors.
9.2
Condition for minimum work.
9.3
Reciprocating compressors including and excluding clearance.
9.4
Multistage compression with intercooling.
9.5
Volumetric efficiency.
9.6
The ideal intermediate pressure.
Learning outcomes
Students should be able to:
•
understand what the function of a compressor is.
•
give differences between rotary and reciprocating compressors regarding their mass
flow and pressure ratio.
•
appreciate that minimum work of compressors is only achieved when compression
process is carried out isothermally.
•
calculate the indicated power of a compressor including and excluding the clearance
volume.
•
appreciate the work saved in intercooling and be able to show it on P-v and T-s
diagrams.
1


n


P
 2 − 1
 P1 



•
V
define volumetric efficiency and to derive the equation ηv = 1 − c
Vs
•
derive that an ideal intermediate pressure for a compressor is Pi = P1 P2 .