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REFERENCE NO: E45 - THERMO 1. COURSE NAME: Thermodynamics 2. COURSE DESCRIPTIONS: The course includes the thermodynamics properties, thermodynamics energy, thermodynamics systems, energy change, heat transfer, vapours, ideal gases, thermodynamics processes and work transfer. 3. NUMBER OF UNITS FOR LECTURE AND LABORATORY: 4 LECTURE, 0 LABORATORY = 4 UNITS 4. NUMBER OF CONTACT HOURS PER WEEK: 4 LECTURE, 0 LABORATORY = 4 HOURS 5. PREREQUISITE: Physics 2 and Integral Calculus 6. COURSE OBJECTIVES: The students shall be able to explain the basic principles for efficient operation of marine heat engine and the relationship between heat and mechanical energy or work, and the conversion of one form into the other FUNCTION: F1 – Marine Engineering at the operational level 7. COURSE OUTLINE: LEARNING OBJECTIVES/OUTCOMES: The students shall be able to . . . . . . 7.1 Thermodynamics Properties 7.1.1 describe the properties used to specify the state, or condition, of a substance, the units which the property is measured and the usual symbol, e.g. 7.1.1.1 pressure 7.1.1.2 temperature 7.1.1.3 volume 7.1.1.4 energy 7.1.2 explain what is meant by: 7.1.2.1 absolute quantities 7.1.2.2 specific quantities 7.1.2.3 intensive values 7.1.2.4 extensive values 7.1.3 explain that a substance can exist in three states, or phases, which are: 7.1.3.1 solid 7.1.3.2 liquid 7.1.3.3 gaseous E-45 THERMO page 1 of 5 7.1.4 describe the energy required to change phase as: 7.1.4.1 enthalpy of fusion (soild-liquid) 7.1.4.2 enthalpy of evaporation (liquid-vapour) 7.1.5 state that a change of phase is constant-temperature process 7.1.6 explain that fluids can have a liquid or a gaseous form 7.2 Thermodynamics Energy 7.2.1 state that “internal” or “intrinsic” energy (U) is related to the motions of the molecules of a substance or a system 7.2.2 state that internal energy is derived only from molecular motions and vibrations, is dependent only on thermodynamic temperature and is energy stored in the molecules 7.2.3 state that the total energy stored in a body, or system, is termed enthalpy (H) 7.2.4 define total stored energy as the some of internal energy and the product of pressure (P) and volume (V), i.e. H = U+PV 7.2.5 define potential energy as energy stored in the molecules by virtue of their vertical position above some datum level 7.2.6 define kinetic energy as energy stored in molecules by virtue of their velocity; kinetic energy has a value of V2 (i.e. 0.5 of velocity squared) per unit mass of substance 7.2.7 state that energy in transition between bodies or systems can only be heat flow (or heat transfer) (Q) and work flow (or work transfer) (W) 7.2.8 define the first law of thermodynamics as “the energy stored in any given thermodynamics system can only be changed by the transition of energies Q and/or W” 7.2.9 solve problems to demonstrate the above objectives 7.3 Thermodynamics Systems 7.3.1 state that systems are identified in terms of mass of substance (i.e. molecules) contained within a system and /or the mass entering and leaving 7.3.2 state that this identification is of importance when evaluating property changes taking place during thermodynamic operations 7.4 Energy Change 7.4.1 explain that the “non-flow” equation derives directly from the first law of thermodynamics and is applicable only to “closed” systems (i.e. no molecules of substance are entering or leaving the system during the thermodynamic operation) 7.4.2 define the general form of the non-flow equations as (U - U1) = ± W ± Q 7.4.3 explain that the mathematical sign associated with the transition energies of Q and W will be governed by “direction”, i.e. whether the energy transfer is “into” or “out of” the closed system 7.4.4 solve simple problems concerning energy changes in practice 7.5 Heat Transfer E-45 THERMO page 2 of 5 7.5.1 state that heat transfer can take place by conduction, convection and radiation and that when substances at different temperatures are placed in contact that will, in time, reach a common temperature through transfer of heat 7.5.2 define specific heat capacity as the heat transfer, per unit mass, per unit of temperature change, for any given body or system 7.5.3 use laboratory equipment to determine: 7.5.3.1 specific heat capacity of substances 7.5.3.2 final temperature of mixtures, and verifies the observed value by calculation 7.5.4 state that the Fourier law for the conduction of heat through a substance as given by Q = λΑθt x 7.5.5 identify the quantities in the Fourier law as Q = heat flow, measured in joules A = surface area, measured in square meters θ = temperature difference between the surface, measured in C t = time interval, measured in seconds x = distance travelled between the surface by the heat, measured in metres λ = the coefficient of thermal conductivity 7.5.6 explain that the units for the coefficient of thermal conductivity are watts per metre per kelvin i.e. joules x metres second x metres² x Kelvin 7.5.7 solve simple numerical problems involving heat transfer between substances when placed in contact with each other; to include mixtures of liquids and solids placed in liquids 7.5.8 solve simple problems on the application of the Fourier law to solid homogenous materials 7.5.9 perform laboratory work to verify the above objective 7.6 Vapours 7.6.1 define the vapour phase as an intermediate stage between the solid and the perfect gas state, and the property values, such as pressure, energy, volume 7.6.2 state that the important fluids in this group are HO (i.e. steam) and the refrigerants 7.6.3 define the following conditions: 7.6.3.1 saturated vapour 7.6.3.2 dry vapour 7.6.3.3 wet vapour 7.6.3.4 dryness fraction 7.6.3.5 superheated vapour 7.6.4 explain and uses the “corresponding” relationship that exists between pressure and temperature for a saturated liquid or saturated vapour 7.6.5 demonstrate the above objective, using laboratory equipment 7.6.6 use tables of thermodynamic properties to determine values for enthalpy, internal energy and volume at any given condition of pressure and/or temperature defined in the above objective E-45 THERMO page 3 of 5 7.7 Ideal Gases 7.7.1 state the “critical temperature” as being the limit of the liquid phase 7.7.2 define an “ideal” gas as one which behaves almost as a perfect gas, whose temperature is above the critical one and whose molecules have a simple monatomic structure 7.7.3 state that an “ideal” gas cannot be liquefied by alteration of pressure alone 7.7.4 state the laws of Boyle and Charles and identifies the following statements with them: P x V = a constant – Boyle V = a constant – Charles T 7.7.5 sketch a P – V curve demonstrating Boyle’s law 7.7.6 sketch a graph of V and T, demonstrating Charle’s law 7.7.7 state that the result of combining the laws of Boyle and Charles is: PV = a constant T 7.7.8 define the specific ideal gas equation as: PV = R, per unit mass of gas T 7.7.9 explain that R will have a different numerical value for each ideal gas or mixture of ideal gases 7.7.10 apply simple numerical calculations involving the elements of the above objectives 7.8 Thermodynamic Processes 7.8.1 define a thermodynamic process as “an operation during which the properties of state, pressure, volume and temperature may change, with energy transfer in the form of work and/or heat flow taking place” 7.8.2 state that the following processes are applicable to ideal gases and vapours: 7.8.2.1 heat transfer: heating and cooling 7.8.2.2 work transfer: compression and expansion 7.8.3 explain in simple terms the second law of thermodynamics\ 7.8.4 explain with the aid of a sketched P-V diagram, where appropriate, the following “standard” processes: 7.8.4.1 pressure remaining constant 7.8.4.2 volume remaining constant 7.8.4.3 temperature remaining constant 7.8.4.4 zero heat transfer 7.8.4.5 polytrophic expansion and compression 7.8.5 describe a process of constant temperature as “isothermal” 7.8.6 describe a process in which there is no heat transfer as “adiabatic” 7.8.7 describe practical applications of the process described in the above objectives 7.8.8 solve simple numerical problems relating to the elements in the above objectives E-45 THERMO page 4 of 5 7.9 Work Transfer 7.9.1 explain that “work” is calculated by force x distance moved by that force 7.9.2 sketch a P-V diagram relating the area of the diagram to the work done when fluid exerts constant pressure on a piston in a cylinder 7.9.3 explain the work transfer for a vapour or an ideal gas terms of pressures and volumes 7.9.4 sketch a P-V diagram, relating the area of the diagram to work done on or by a piston in a cylinder during the polytrophic expansion and compression 7.9.5 state the equation for work transfer, i.e. W = P1V1 – P2V2 n–1 where: W is the work done, in joules P is the pressure at specific points in the process, in newtons/m² V is the volume at the same points as for pressure, in m³ n is a numerical index 7.9.6 state that the numerical index n is derived by experiment, using the equation (P1V1)n = (P2V2)n 7.9.7 state that, for most practical operations, n has numerical values between 1.2 and 1.5 7.9.8 apply simple numerical calculations related to the elements in the above objectives 8. EQUIPMENT, MATERIALS, CHEMICALS, TEACHING AIDS: The equipment, materials, chemicals, teaching aids needed in this course is listed in the attached APPENDIX 1. 9. REFERENCES: 9.1 Longman, R., Harlow, Joel. “Basic Engineering Thermodynamics In S.I Units” 4th Ed., 9.2 Burghart, David M., “Engineering Thermodynamics with Applications”. 9.3 Faires, Virgil M./Simmang, Clifford. “Theory And Problems Of Thermodynamics”. 9.4 Zemansky, Mark W., et.al. “Basic Engineering Thermodynamics”. GMS Publication. 9.5 STCW Code, Table A-III/I 9.6 Osorio-Bea, Cynthia and Amaro, Marcial III. “Marine Thermodynamics 1”. 9.7 Sta. Maria. “Thermodynamics I” 1990. 9.8 Keenan. “Steam Power/Thermodynamics”. 9.9 Holman. “Thermodynamics”. E-45 THERMO page 5 of 5