TE_CO2 bhot acha h ye dekho to aap log.pptx

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1. Diploma in Mechanical Engineering ( M02) 3 rd Semester Thermal Engineering (302)OCBC Name of Subject Teacher Prof. R. K. Hardaha

2. Outcome Based Education (OBE) Outcome Based Curriculum OCBC 2019

3. Solve simple problems based on basic concepts of thermodynamics, and its laws. Course Outcome 2 ( CO2)

4. Explain thermodynamic systems, properties, processes, cycles, gas equation and modes of heat transfer. Learning Outcome 01 Teaching Hrs – 6, Maximum Marks - 7 Method of Assessment Paper-Pen Test (Part of PT-1)

5. Concept of thermodynamic System, definition, classification and applications, State, processes, cycles, Properties, Intensive and Extensive with examples, Point and Path function, Concept of Work and Heat. Definitions: Enthalpy, Internal energy, Entropy, Specific heat at constant pressure (Cp), specific heat at constant volume ( Cv ), relation between Cp & Cv , characteristic gas equation, Universal gas constant, Definition of quasi-static process, flow work, Modes of Heat transfer - definition and types. Contents

6. Solve given problems based on thermodynamic systems, properties and gas equation Learning Outcome 02 Teaching Hrs – 4, Maximum Marks - 10 Method of Assessment : Theory Exam

7. Numerical problems based on Thermodynamic System, Properties, gas equation. Contents

8. Solve given problems based on the laws of thermodynamics. Learning Outcome 3 Teaching Hrs – 8 Maximum Marks - 10 Method of Assessment Theory Exam

9. Laws of thermodynamics- Zeroth law, concept of work and heat, statement of first law- internal energy, enthalpy, relationship between heat transfer, work transfer and change in internal energy, Concept of conservation of mass and control volume, Steady and steady flow energy equation (without proof). Contents

10. Limitation of first law. Second law – Clausius and Kelvin-Planck Statements, concept of heat pump, refrigerator, heat engine, thermal efficiency , COP, reversible process, factors which make a process irreversible, Carnot cycle, its efficiency and limitation, Clausius inequality, entropy Contents

11. 2.1 Concept of thermodynamic System Thermodynamics , science of the relationship between heat, work, temperature, and energy. In broad terms,  thermodynamics  deals with the transfer of energy from one place to another and from one form to another. The key  concept  is that heat is a form of energy corresponding to a definite amount of mechanical work.

12. Thermodynamics ऊष्मागतिकी The branch of Physical Science that deals with the relations between Heat and Work Energy. Heat Engine Heat Pump, Refrigerator

13. Thermal Engineering ऊष्मा अभियांत्रिकी Thermal Engineering is a specialized branch of Mechanical Engineering that deals with the utilization of Heat Energy in to Work and Heat Transfer

14. Steam Engine Steam Turbine Examples of Thermal Engineering Steam Boiler

15. Examples of Thermal Engineering IC Engine Gas Turbine

16. Condencer Examples of Thermal Engineering Heat Exchanger Refrigerator

17. Temperature (ताप) Temperature is a physical property of matter that quantitatively expresses hot and cold. MKS System = ° C SI Unit System =K FPS System = ° F ° C = 273 K = 32 ° F 100 ° C = 373 K = 212 ° F Absolute 0 temprature = K

18. Measurment of Temprature Mercury thermometer Thermo-Couple Resistance Thermometer Radiation Pyrometer

19. Temperature Conversion Formula

20. The condition under which two substances in physical contact with each other exchange no heat energy . Two substances in  thermal equilibrium  are said to be at the same temperature. Thermal Equilibrium

21. Thermal Equilibrium . Thermal Equilibrium .

22. Heat Energy ऊष्मा ऊर्जा (Q) Heat Energy is the result of the movement of tiny particles called atoms, molecules or ions in solids, liquids and gases. At higher temperatures, particles have more energy. Some of this energy can be transmitted to other particles that are at a lower temperature.

23. Heat Energy ऊष्मा ऊर्जा (Q) Unit of Heat (Q) SI System = Joule (J) Unit of Heat (Q) MKS System = Calories

24. Calorie :- The amount of Heat required to raise 1° Celsius temperature of 1 gram of water at Standard atmospheric Pressure. Calorie 1 Calorie = 4.186 Joule (SI Unit) 1 Calorie = 0.427 kgf.m (MKS Unit)

25. Did You Know? A calorie is a unit of energy. In nutrition, calories refer to the energy people get from the food and drink they consume, and the energy they use in physical activity. Below are the calorific values of three main components of food: 1 g of carbohydrates contains 4 kcal 1 g of protein contains 4 kcal 1 g of fat contains 9 kcal

26. What 400 Calories look like in Your Tummy

27. Did You Know? Most people only associate calories with food and drink, but anything that contains energy has calories. 1 kilogram (kg) of coal, for example, contains 7,000,000 calories. There are two types of calorie: A small calorie (cal)  is the amount of energy required to raise the temperature of 1 gram (g) of water by 1º Celsius (º C). A large calorie (kcal)  is the amount of energy required to raise 1 kilogram (kg) of water by 1º C. It is also known as a kilocalorie. 1 kcal is equal to 1,000 cal. The terms “large calorie” and “small calorie” are often used interchangeably. This is misleading. The calorie content described on food labels refers to kilocalories. A 250-calorie chocolate bar actually contains 250,000 calories.

28. The  thermodynamic state  of a system is defined by specifying values of a set of measurable properties sufficient to determine all other properties. For fluid systems, typical properties are pressure, volume and temperature . More complex systems may require the specification of more unusual properties.   Thermodynamic State

29. Within thermodynamics, a physical property is any property that is measurable, and whose value describes a state of a physical system. Our goal here will be to introduce thermodynamic properties , that are used in engineering thermodynamics. Thermodynamic Properties

30. In general,  thermodynamic properties  can be divided into two general classes: 1.Extensive properties 2. Intensive Properties

31.  An  extensive property  is dependent upon the amount of mass  present or upon the  size or extent of a system . For example, the following properties are extensive: Extensive property Enthalpy Entropy Heat Capacity Internal Energy Mass Volume

32.  Density Specific Enthalpy Specific Entropy Specific Heat Capacity Pressure Intensive Property An  intensive property  is  independent of the amount  of mass and may vary from place to place within the system at any moment. For example, the following properties are intensive: Temperature Thermal Conductivity Thermal Expansion Vapor Quality Specific Volume

33. Specific properties  are extensive properties per unit mass and are denoted by lower case letters. For example: Specific Properties Specific volume = v = m 3 /kg Specific Heat = s = J/ kgK Specific Enthalpy = h= J/kg

34. Extensive and Intensive Property

35. One of the most familiar forces is the weight of a body, which is the gravitational force that the earth exerts on the body. In general, gravitation is a natural phenomenon by which all things with mass are brought toward one another. The terms mass and weight are often confused with one another, but it is important to distinguish between them. W=mg Wt.= mass x acceleration due to gravity Mass v/s Weight

36.   Atmospheric pressure is the pressure in the surrounding air at – or “close” to – the surface of the earth. The atmospheric pressure varies with temperature and altitude above sea level. The  Standard Atmospheric Pressure  is defined at sea-level at  273 o K (0 o C)  and is: Atmospheric Pressure 101325 Pa 1.01325 bar 14.696 psi 760 mmHg

37. 2.11 Thermodynamic System A thermodynamic system is a macroscopic region of the universe under study, with a quantity of matter of fixed identity. It is defined by boundaries, which control the transfers between the system and the surroundings (everything which is outside the boundary). The types of transfers that can occur in a thermodynamic process are mass and energy (work and heat).

38. Thermodynamic System

39. 2.12 Classification Of Thermodynamic System A thermodynamic system can be classified as open, closed or isolated, according to the exchanges that can occur with the surroundings. Open system- exchanges of energy and matter. Closed system- exchanges of energy but not of matter. Isolated system- does not exchange energy or matter.

40. Thermodynamic System Open Closed Isolated

41. Thermodynamic System Open System Closed System Isolated System

42. Piston Cylinder Assembly of IC Engine

43. Open System

44. Closed System

45. Closed System

46. Isolated System

47. Heat capacity or thermal capacity is a physical property of matter, defined as the amount of heat to be supplied to a given mass of a material to produce a unit change in its temperature. The SI unit of heat capacity is joule per kelvin . Q= J/K Heat capacity is an extensive property. Heat capacity

48. Specific Heat (विशिस्ट ऊष्मा) (C) The amount of heat required to raise the temperature of the unit mass of a given substance by 1 degree.

49. Their SI units are J/kg K. Two  specific heats  are defined for gases, one for  constant volume  ( Cv ) and one for constant pressure  (Cp). Specific Heat For Gases Specific Heat at Constant Pressure C P Specific Heat at Constant Volume C V

50. The amount of heat required to raise the temperature of the unit mass of a gas by 1 degree in a constant pressure process. Specific Heat at Constant Pressure C P Specific Heat at Constant Volume C V The amount of heat required to raise the temperature of the unit mass of a gas by 1 degree in a constant volume process.

51. In  thermal  engineering and thermodynamics, the  heat capacity ratio , also known as the adiabatic index, the  ratio  of specific heats, or Laplace's coefficient, is the  ratio  of the  heat capacity  at constant pressure (C P ) to  heat capacity  at constant volume (C V ). Adiabatic Index Heat Capacity Ratio ( Adiabatic Index) ( C P ​>C V ​)

52. Why specific heat of a gas at constant pressure is always greater than the specific heat of a gas at constant volume? ANSWER :- ( CP​>CV​) CP​ is greater than CV​ because when a gas is heated at constant volume, no external work is done and so the heat supplied is consumed only in increasing the internal energy of a gas. But if the gas is heated at constant pressure, the gas expands against the external pressure so does some external work. in this case the heat is used up in increasing the internal energy of the gas and in doing some external work. Since the internal energy depends only on temperature, for the same rise of temperature the internal energy of a mass of a gas will increase by the same amount whether the pressure or volume remains constant. But since external work is additionally done for constant pressure than at constant volume to produce the same rise in temperature of the gas. Above is the reason why CP​ is greater than CV​.

53. Latent heat of boiling Latent heat of condensation Latent Heat Of Evaporation (Water)2260 kJ/kg Latent heat of melting Latetent heat of freezing Latent Heat Of Fusion (Water) 334kJ/kg Latent Heat ( गुप्त ऊष्मा) The heat required to convert a solid into a liquid, or a liquid into a vapour , without change of temperature. (Phase Change)

54. Specific Heat, Latent Heat of Ice, Water and Steam

55. Calorific Value (ऊष्मीय मान) The Energy contained in a fuel or food, determined by measuring the heat produced by the complete combution of a unit quantity of it. Unit :- SI kJ/kg or MKS kCal /kg

56. Boyle’s Law Boyle's Law states that the pressure ( P ) of a gas is inversely proportional to the volume ( V ). This law is valid as long as the temperature and the amount of gas are constant. P 1 V 1 = P 2 V 2 (At Constant Temperature)

57. Boyle’s Law Illustrated

58. P 1 V 1 = P 2 V 2 When Temperature T is kept constant. P V Diagram

59. Boyle’s Law

60. Charles law  states that the volume of an ideal gas is directly proportional to the absolute temperature at constant pressure. Charles law V ∝ T

61. Pressure Constant

62. P Constant

63. V ∝ T At Constant Pressure

64. Gay-Lussac’s law is a gas law which states that the pressure exerted by a gas (of a given mass and kept at a constant volume) varies directly with the absolute temperature of the gas. P ∝ T P/T = k Gay-Lussac’s Law

65. Gay-Lussac’s Law At Constant Volume

66. Constant Volume Process At Constant Volume

67. P ∝ T

68. At Constant Volume P ∝ T

69. The combined gas law is also known as a general gas equation is obtained by combining three gas laws which include Charle’s law, Boyle’s Law and Gay-Lussac law. The law shows the relationship between temperature, volume and pressure for a fixed quantity of gas. Combined Gas Law The general equation of combined gas law is given as; PV / T = k If we want to compare the same gas in different cases, the law can be represented as; P 1 V 1  / T 1  = P 2 V 2  / T 2 

70. Combined Gas Equation

71. AB – Constant Volume Process BC – Constant Pressure Process AC – Constant Temperature Process Pressure Volume Diagram

72. Avogadro’s law states that ‘Equal volumes of all gases at conditions of same temperature and pressure have the same number of molecules’, written as: V ∝ n or V/n =K where V=volume of gas; n=Number of moles (1 mole=6.022 x 10 23  molecules). It implies that under similar conditions of pressure, volume and temperatures all gases will have an equal number of molecules, independent of the weight and density of the gas. Avogadro’s Law

73. The specific number of molecules in one gram-mole of a substance, defined as the molecular weight in grams, is 6.02214076 × 10 23 , a quantity called Avogadro’s number, or the Avogadro constant. The volume occupied by one gram-mole of gas is about 22.4 liters at standard temperature and pressure (0 °C, 1 atmosphere) and is the same for all gases, according to Avogadro’s law. Avogadro’s number

74. The  ideal gas law  is derived from empirical relationships among the pressure, the volume, the temperature, and the number of moles of a  gas. It can be used to calculate any of the four properties if the other three are known. Ideal gas equation : PV= nRT Ideal Gas Law

75. The Ideal Gas Equation PV= nRT

76. The  gas constant  (also known as the  molar gas constant ,  universal gas constant , or  ideal gas constant ) is denoted by the symbol R . It is equivalent to the Boltzmann constant, but expressed in units of energy per temperature increment per mole, i.e. the pressure–volume product, rather than energy per temperature increment per particle. The constant is also a combination of the constants from Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law. It is a physical constant that is featured in many fundamental equations in the physical sciences, such as the ideal gas law, the Arrhenius equation, and the Nernst equation. Universal Gas Constant ( R )

77. In  thermal  engineering and thermodynamics, the  heat capacity ratio , also known as the adiabatic index, the  ratio  of specific heats, or Laplace's coefficient, is the  ratio  of the  heat capacity  at constant pressure (C P ) to  heat capacity  at constant volume (C V ). Adiabatic Index Heat Capacity Ratio ( Adiabatic Index) ( C P ​>C V ​)

78. A polytropic process is a thermodynamic process that obeys the relation: where p is the pressure, V is volume, n is the polytropic index, and C is a constant. The polytropic process equation can describe multiple expansion and compression processes which include heat transfer. Polytropic Process A  polytropic process  is a  thermodynamic process  that obeys the relation

79. Polytropic Process

80. Question: How many moles of ‘He’ (Helium) are contained in a 6-litre canister at 101 KPa and 27 ° C. Take R= 8.314 J/mol K Solution: Using the Ideal gas equation, n = PV/RT Therefore, on substituting the values(T = 27 + 273 = 300) we get, = 101 x 6/ 8.314 x 300 = 606/2494.2 = 0.2429 moles Hence, 0.2429 moles of ‘He’ are contained in a 6-litre canister at 101 KPa and 27 ° C Solved Examples for You

81. Sample problems for using the Ideal Gas Law, PV = nRT 1) 2.3 moles of Helium gas are at a pressure of 1.70 atm , and the temperature is 41°C. What is the volume of the gas? 2) At a certain temperature, 3.24 moles of CO 2  gas at 2.15 atm take up a colume of 35.28L. What is this temperature (in Celsius)?

82. Energy ( ऊर्जा) Unit Of Energy (SI unit) = Joule Mechanical Energy Work done Nm = J (Joule) Work done = Force (N) X Displacement (m) = Nm = J Potential Energy = mgh Kinetic Energy = ½ mv Thermal Energy Electrical Energy Chemical Engineering and many more Energy , is the capacity for doing Work. 2

83. Work (Mechanical) Energy (W) कार्य (यांत्रिक) ऊर्जा Work is the product of the magnitudes of the component of a force along the direction of displacement and the displacement. Work is not done on an object unless the object is moved because of the action of a force. The application of a force alone does not constitute work. WD= Force in the direction of Displacement X Displacement = F Cos ϴ X d Joule Unit of force = N (Newton) Unit of Workdone = N.m = J Unit of Energy = J Unit of Heat = J N.m = Joule

84. Law of Conservation of Energy ऊर्जा का अविनाशता का नियम It States that  energy can neither be created nor be destroyed. Although, it may be transformed from one form to another. If you take all forms of energy into account, the total energy of an isolated system always remains constant. 

85. Law of Conservation of Mass द्रव्य का अविनाशता का नियम It states that, in a closed system, mass can neither be created nor destroyed by chemical or physical process. In other words, total mass is always conserved .

86. Defined by change in the system, a thermodynamic process is a passage of a thermodynamic system from an initial to a final state of thermodynamic equilibrium. The initial and final states are the defining elements of the process. Such idealized processes are useful in the theory of thermodynamics Thermodynamic Process

87. Thermodynamic Process 1. Constant Temperature Process or Isothermal Process 2. Constant Volume Process or Isochoric Process 3. Constant Pressure Process or Isobaric Process 4. Constant Entropy Process or adiabatic Process

88. An  isothermal process  is a thermodynamic  process  in which the temperature of a system remains constant. The transfer of heat into or out of the system happens so slowly that thermal equilibrium is maintained.   Isothermal Process

89. An  isochoric process  is a thermodynamic process, in which the  volume  of the closed system remains constant  (V = const). It describes the behavior of gas inside the container, that cannot be deformed. Isochoric Process

90. An isobaric process is a thermodynamic process in which the pressure remains constant. This is usually obtained by allowing the volume to expand or contract in such a way to neutralize any pressure changes that would be caused by heat transfer. Isobaric Process

91. An adiabatic process occur without transferring heat or mass between a thermodynamic system and its surroundings. Unlike an isothermal process an adiabatic process transfers energy to the surroundings only as work. Adiabatic Process

92. P-V Diagram of Various Process (Expansion Process)

93. Enthalpy (H) It is the amount of Heat absorbed or expelled by the system to cause change in the System.

94. Internal Energy आंतरिक ऊर्जा In thermodynamics, the Internal Energy of a system is the energy contained within the system.

95. Entropy (S) Entropy S can be defined as a simple qualitative way to measure the degree of Randomness of the particles, such as molecules in the system. Entroty (S) = ------------------------- Heat Absoebed (Q) Temperature T kJ/K

96. Entropy  is a function of the state of the system, so the  change in entropy  of a system is determined by its initial and final states. In the idealization that a process is reversible, the  entropy  does not  change , while irreversible processes always increase the total  entropy . Change In   Entropy  (ΔS) 

97. Path function : Depends upon the path at which system arrives at a given state. Example :- Work and Heat. Point functions : Which does not depend on path. Example :- temperature, pressure, density, mass, volume, entropy, internal energy. They are the properties of the system. Path and Point functions

98. A  thermodynamic cycle  consists of a linked sequence of  thermodynamic processes  that involve transfer of heat and work into and out of the system, while varying pressure, temperature, and other state variables within the system, and that eventually returns the system to its initial state. Thermodynamic Cycle

99. The Carnot Cycle

100. PV Diagram of Carnot Cycle

101. PV and TS Diagram of Carnot Cycle

102. Ideal Rankine Cycle T S Diagram

103. Processes in Otto Cycle

104. PV and TS Diagram of Otto Cycle

105. 4 Stroke Diesel Engine

106. 4 Stroke Diesel Engine Cycle

107. Diesel Cycle

108. PV and TS Diagram of Diesel Cycle

109. In thermodynamics, a  quasi-static process  (also known as quasi-equilibrium) is a thermodynamic process that happens slowly enough for the system to remain in internal equilibrium. An example of this is quasi-static compression, where the volume of a system changes at a slow rate enough to allow the pressure to remain uniform and constant throughout the system Quasistatic Process

110. First Law of Thermodynamics ऊष्मा गतिकी का प्रथम नियम This means that heat energy cannot be created or destroyed. It can transferred from one body to another and converted to one from to other forms of Energy.  Note:- 1 kCal = 4.186 kJ 1 kCal = 427 kgfm 1 kJ Heat = 1 kJ Work 1 kCal Heat = 427 kgfm Work

111. Second Law of Thermodynamics ऊष्मा गतिकी का द्वितीय नियम Kelvin plank statement Clausius statement

112. Kelvin planck statement It is impossible to construct a device which operates on a cyclic process and convert all the heat supplied to it into equivalent amount of work.

113. Clausius statement It is impossible to construct a device which operates on a cycle and produces no other effect than the transfer of heat from a cooler body to a hotter body.   It is impossible to construct a device which operates on a cyclic process that transfer heat from a cooler body to a hotter body.

114. Heat Engine Heat Pump Refrigerator Heat Engine Heat Pump Refrigerator

115. Third Law of Thermodynamics ऊष्मा गतिकी का तृतीय नियम It states that the Entropy (S) of a perfect crystal at a temperature of zero Kelvin (absolute zero) is equal to zero.

116. There are three modes of heat transfer 1. Conduction 2. Convection 3. Radiation Modes Of Heat Transfer Heat is a form of energy that can be transferred from hot body to cold body or from higher to lower temperature.

117. Conduction :  Conduction refers to the heat transfer that occurs across the medium. Medium can be solid or a fluid. Convection :  Convection refers to the heat transfer that will occur between a surface and a moving fluid when they are at different temperatures.   Radiation : In radiation, in the absence of intervening medium, there is net heat transfer between two surfaces at different temperatures in the form of electromagnetic waves. Conduction, Convection and Radiation

118. Steam Engine A  steam engine  is a heat  engine  that performs mechanical work using  steam  as its working fluid. The  steam engine  uses the force produced by  steam  pressure to push a piston back and forth inside a cylinder. This pushing force is transformed, by a connecting rod and flywheel, into rotational force for work.

119. Steam Engine

120. Internal Combustion Engine An engine which generates motive power by the burning of petrol, oil, or other fuel with air inside the engine, the hot gases produced being used to drive a piston or do other work as they expand.

121. Two Stroke Engine Compression Stroke 2. Power Stroke

122. Suction Compression Power Exhaust Four Stroke Engine

123. Steam Turbine स्टीम टरबाइन Impulse Turbine Reaction Turbine

124. Steam Turbine

125. Enjoy Learning

126. Very Much For Your Kind Attention and Time

127. जय हिन्द जय भारत