introduction of thermodynamics ◦ thermodynamics & energy ◦ closed & open systems ◦...
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INTRODUCTION OF THERMODYNAMICS
◦ Thermodynamics & Energy◦ Closed & Open Systems◦ Properties of a Systems◦ State & Equilibrium◦ Pressure & Temperature◦ Work, Energy & Heat◦ Kinetic & Potential Energy◦ Internal Energy◦ Specific Heat & Lantern Heat
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Objective of this session◦Definition of thermodynamics◦Introduction to energy conversion
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What is “Thermodynamics”?
science of energy
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The name thermodynamics stems from the Greek words therme (heat) and dynamis (power), which is most descriptive of the early efforts to convert heat into power.
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Rub your hands together for 15 seconds.
Are your hands warm?
Thermal energy
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The study of the effects of work, heat flow, and energy on a system
Movement of thermal energy
Engineers use thermodynamics in systems ranging from nuclear power plants to electrical components.
SYSTEM
SURROUNDINGS
BOUNDARY
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Thermal Energy is kinetic energy in transit from one object to another due to temperature difference. (Joules)
Temperature is the average kinetic energy of particles in an object – not the total amount of kinetic energy particles. (Degrees)
Temperature #1 Temperature #2
Heat
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Scale Freezing point of water
Boiling point of water
Celsius 0°C 100°C
Fahrenheit 32°F 212°F
Kelvin 273K 373K
Matter is made up of molecules in motion (kinetic energy)
An increase in temperature increases motion
A decrease in temperature decreases motion
Absolute Zero occurs when all kinetic energy is removed from a object 0 K = -273° C
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Thermal equilibrium is obtained when touching objects within a system reach the same temperature.
When thermal equilibrium is reached, the system loses its ability to do work.
Zeroth Law of Thermodynamics: If two systems are separately found to be in thermal equilibrium with a third system, the first two systems are in thermal equilibrium with each other.
Object #2Object #2 Object #3Object #3
Object #1Object #1(Thermometer)(Thermometer)
Object #1Object #1 Object #2Object #2
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The transfer or movement of thermal energy
Most common types of transfer
Convection
Conduction
Radiation
100% efficiency is unattainable
ALL processes are irreversible
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Power plant
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Rocket
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Air conditioning
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Internal Combustion Engine
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Objective of this session◦Definition of systems◦Familiar with different property definition
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Types of systems1. Closed system (or control mass)
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2. Open system (or control volume)
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Isolated system
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Any characteristic of a system. Some familiar properties are;
# pressure P, # temperature T, # volume V, and # mass m
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Example of extensive and intensive properties
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State: condition of the system characterized by the values of its properties
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Process: any change that a system undergoes from one equilibrium state to another. eg: heating water, student entering classroom….
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Quasistatic (quasiequilibrium) process: is a process which proceeds in such a manner that the system remains infinitesimally close to an equilibrium state at all times
e.g. room heating up uniformly coffee cooling down uniformly
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12 1’1’’System
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Path: the series of states through which a system passes during a process.
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State 1
p
v
State 2
12 1’1’’System
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Cycle: System returns to initial state at the end of process(es)
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p
v
State 2
12System 2
System 1
State 1
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◦Process or cycle efficiency: quality of cycle or process
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