Abstract
Sustainable energy systems exhibit a diverse nature and cover a large number of processes such as energy conversion, heating, cooling, and chemical reactions. Sustainable energy engineering is a complex subject because many disciplines such as thermodynamics, fluid mechanics, heat transfer, electromagnetics, and chemical reaction engineering are encountered in its processes and applications.
This is a preview of subscription content, log in via an institution to check access.
Access this chapter
Tax calculation will be finalised at checkout
Purchases are for personal use only
Abbreviations
- a :
-
Acceleration, m/s2
- A :
-
Area, m2
- c :
-
Specific heat, J/kg K
- COP:
-
Coefficient of performance
- d :
-
Displacement, m
- DOF:
-
Degree of freedom
- E :
-
Energy, J
- F :
-
Force, N
- g :
-
Gravitational acceleration, m/s2
- h :
-
Specific enthalpy, J/kg
- H :
-
Enthalpy, J
- k B :
-
Boltzmann constant, J/K
- K :
-
Kinetic energy, J
- KE :
-
Kinetic energy, J
- m :
-
Mass, kg
- M :
-
Molecular mass, kg/kmol
- n :
-
Number of moles, mol or polytropic exponent
- N :
-
Number of molecules
- N A :
-
Number of Avogadro
- p :
-
Momentum, kg m/s
- P :
-
Pressure, Pa
- PE :
-
Potential energy, J
- q :
-
Mass specific heat, J/kg
- Q :
-
Heat, J
- R :
-
Universal gas constant, J/mol K
- Rg :
-
Real gas constant, J/kg K
- s :
-
Specific entropy, J/kg K
- S :
-
Entropy, J/K
- T :
-
Temperature, K
- v :
-
Velocity, m/s, or specific volume, m3/kg
- V :
-
Volume, m3
- u :
-
Specific internal energy, J/kg
- U :
-
Internal energy, J
- W :
-
Work, J
- x :
-
Vapor quality
- Z :
-
Elevation, m or compressibility factor
- α :
-
Peng–Robinson parameter
- γ :
-
Adiabatic exponent
- η :
-
Energy efficiency
- ψ :
-
Exergy efficieny
- ω :
-
Accentric factor
- gen:
-
Generated
- H:
-
High
- liq:
-
Liquid
- L:
-
Low
- n:
-
Value corresponding to 1 mol
- p:
-
Constant pressure
- r:
-
Reduced value
- rev:
-
Reversible
- t:
-
Total
- v:
-
Constant volume
- vap:
-
Vapor
- surr:
-
Surroundings
- sys:
-
System
- _:
-
Average value
- \( \bullet \) :
-
Rate (per unit of time)
References
Callen H.B. 1985. Thermodynamics and an Introduction to Thermostatistics, 2nd edition. Wiley, New York.
Carnot S. 1824. Réflexions sur la Puissance Motrice du Feu et Sur les Machines Propres à Développer Cette Puissance. Bachelier, Paris.
Crosbie S. 1998. The Science of Energy—a Cultural History of Energy Physics in Victorian Britain. The University of Chicago Press, Chicago.
Dincer I. 1998. Thermodynamics, exergy and environmental impact. Proceedings of the ISTP-11, the Eleventh International Symposium on Transport Phenomena, November 29–December 3, Hsinchu, Taiwan, pp.121–125.
Dincer I. 2002. The role of exergy in energy policy making. Energy Policy 30:137–149.
Dincer I., Rosen M.A. 1999. The intimate connection between exergy and the environment, in Thermodynamic Optimization of Complex Energy Systems, A. Bejan and E. Mamut eds., pp. 221–230, Kluwer Academic Publishers, The Netherlands.
Klein S.A. 2010. Engineering Equation Solver (Academic Commercial v.8.629).
Marquand C., Croft D. 1997. Thermofluids—An Integrated Approach to Thermodynamics and Fluid Mechanics Principles. Wiley, New York.
Moran M.J., Shapiro H.N. 1998. Fundamentals of Engineering Thermodynamics, 3rd edition. Wiley, New York.
Stryjek R., Vera J.H. 1986. PRSV, an improved Peng-Robinson equation of state for pure compounds and mixtures. Canadian Journal of Chemical Engineering 64:323.
Szargut J., Morris D.R., Steward F.R. 1988. Exergy Analysis of Thermal, Chemical, and Metallurgical Processes. Hemisphere, New York.
Author information
Authors and Affiliations
Corresponding author
Study Questions/Problems
Study Questions/Problems
-
1.1
Define the notions of force, momentum, and work, and explain the differences among them.
-
1.2
Define the following forms of energy and explain the differences among them: internal energy, work, heat.
-
1.3
Define the following terms: enthalpy, entropy, free energy (Gibbs), exergy.
-
1.4
Give examples of macroscopic forms of energy.
-
1.5
What is a conservative force?
-
1.6
Explain the terms absolute, gauge, and vacuum pressure.
-
1.7
Define the notion of temperature from the prism of kinetic theory of gases. Include relevant formulas in the explanation.
-
1.8
Define the universal gas constant.
-
1.9
Define the Boltzmann constant.
-
1.10
Using appropriate equations, transform the temperature of 100°C in degrees Kelvin, Rankine, and Fahrenheit.
-
1.11
Explain the state-change diagram of a substance.
-
1.12
Define the notion of vapor quality.
-
1.13
Define the following and explain the differences among them: closed system, open system, insulated system.
-
1.14
Does an exergy analysis replace an energy analysis? Describe any advantages of exergy analysis over energy analysis.
-
1.15
Can you perform an exergy analysis without an energy analysis? Explain.
-
1.16
Noting that heat transfer does not occur without a temperature difference and that heat transfer across a finite temperature difference is irreversible, is there such a thing as reversible heat transfer? Explain.
-
1.15
The specific heat of air is 1,005 J/kgK. Express it in kcal/lb°F. Explain the calculations.
-
1.16
Using the ideal gas law, derive an expression for density of atmospheric air as a function of altitude.
-
1.17
Argon is compressed from standard conditions up to a pressure of 5 bar. Assume polytropic compression and calculate the compression work per unit of mass. Do the same calculation for isothermal process. Explain the difference. Argon is assumed to be an ideal gas.
-
1.18
Water is heated from 50 to 90°C. Determine the amount of heat required to do this for 10 kg of water. Determine the relative increase in water volume.
-
1.19
Air at 25°C expands from 300 bar to atmospheric pressure. Determine the work generated assuming adiabatic expansion process.
-
1.20
Using the appropriate lithium bromide–water diagram from Appendix B, determine the temperature and pressure of the vapor when the solution temperature is 100°C and the concentration is 60%.
-
1.21
Calculate the enthalpy needed for unit of mass to heat lithium bromide–water solution from 30°C and 50% concentration to 100°C and 65% concentration.
-
1.22
Ammonia–water vapor at 25 bar and 100°C is cooled (and absorbed) in a process such that eventually it achieves 10°C and 1 bar. Calculate the amount of enthalpy extracted per kilogram.
-
1.23
Based on Tables B.3 and B.4 in Appendix B, calculate the chemical exergy of copper oxychloride, cupric oxide, cupric chloride, and cuprous chloride, and verify the result with the data listed in Table B.4.
-
1.24
Assume that superheated steam at 25 bar and 400°C expands isentropically to 6.22 bar. Determine the temperature after expansion.
-
1.25
Saturated ammonia vapor at −25°C is compressed isentropically to 7.62 bar. Determine the temperature after compression.
-
1.26
Calculate mass, energy, entropy, and exergy balances for the following devices: (a) an adiabatic steam turbine, (b) an air compressor with heat loss from the air to the surroundings, (c) an adiabatic nozzle, and (d) a diffuser with heat loss to the surroundings.
-
1.27
Define each of the following efficiencies for a compressor and explain under what conditions they should be used: (a) isentropic efficiency, (b) isothermal efficiency, and (c) exergy efficiency.
Rights and permissions
Copyright information
© 2011 Springer Science+Business Media, LLC
About this chapter
Cite this chapter
Dinçer, İ., Zamfirescu, C. (2011). Thermodynamic Fundamentals. In: Sustainable Energy Systems and Applications. Springer, Boston, MA. https://doi.org/10.1007/978-0-387-95861-3_1
Download citation
DOI: https://doi.org/10.1007/978-0-387-95861-3_1
Published:
Publisher Name: Springer, Boston, MA
Print ISBN: 978-0-387-95860-6
Online ISBN: 978-0-387-95861-3
eBook Packages: EngineeringEngineering (R0)