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Chapter 3 The First Law of Thermodynamics: Closed System. 3-1 Introduction To The First Law of Thermodynamics. 3-1-1 Conservation of energy principle Energy can be neither created nor destroyed;it can only change forms.

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chapter 3 the first law of thermodynamics closed system
Chapter 3 The First Law of Thermodynamics: Closed System
3 1 introduction to the first law of thermodynamics
3-1 Introduction To The First Law of Thermodynamics

3-1-1 Conservation of energy principle

Energy can be neither created nor destroyed;it can only change forms

3-1-2 The First Law of Thermodynamics

Neither heat nor work can be destroyed;they can only change from one to another, that is:

slide3

3-1-2 The shortcomings of Q=W

  • Can’t be employed in engineering calculation
  • Can’t show the quality difference between heat and work

In engineering area we would rather use a formula like this:

The net energy transferred from the system

The net energy transferred to the system

-

The net change in the total energy of the system

=

3 2 work
3-2 Work

Work is energy in transition

3-2-1Definition:

work is the energy transfer associated with a force acting through a distance

Denoted by W ----------kJ

work on a unit-mass basis is denoted by w

w----------kJ/kg

work done per unit time is called power

power is denoted as

slide5

3-2-2Positive and negative

Since work is the energy transferred between system and its boundary, then we define that:

work done by a system is positive; and work done on a system is negative

3 3 mechanical forms of work
3-3 Mechanical forms of Work

3-3-1Moving boundary work

slide8

The condition of the formula

Is that:

Reversible Process

A process that not only system itself but also system and surrounding keeps equilibrium

System undergoes a reversible process

3 3 heat transfer
3-3 Heat Transfer

Heat is energy in transition

3-3-1Definition:

Heat is defined as the form of energy that is transferred between two systems due to temperature difference .

denote as Q ----------kJ

heat transferred per unit mass of a system is denoted as q----------kJ/kg

We define heat absorbed by a system is positive

slide12

3-3-2 Historical Background

3-3-3 Modes of Heat Transfer:

Conduction:

slide13

Convection:

Radiation:

slide14

3-3-4 Thermodynamic calculation of Heat

1. Q=mCΔT

2. Consider:

P------the source to do work

dV-----the indication to show if work has been done

the source to lead to heat transfer is T, then there should be:

slide15

What is dx here?

dx-----the indication to show if heat has been transferred

Consider:

We define that x is called entropy and denoted asS

The unit of S is kJ/K

Specific entropy is denoted as s

The unit of s is: kJ/kg.K

slide18

1. The net energy transfer to the system:

Win , Qin

2. The net energy transfer from the system:

Wout , Qout

3. The total Energy ofthe system:

E

slide19

3-4-2 The First-LawRelation

(Qin+Win) - (Qout+Wout) = ΔE

(Qin - Qout) + (Win - Wout) = ΔE

Consider the algebraic value of Q and W

(Qin - ∑Qout) - (∑Wout - ∑Win) =ΔE

Q - W = ΔE

Q = ΔE + W

slide20

3-4-3 Other Forms of the First-LawRelation

1. Differential Form:

δQ = dE + δW

As to a system without macroscopic form energy

δQ = dU + δW

On a unit-mass basis

δq = de + δw

δq = du + δw

slide21

2. Reversible Process

δQ = dE + PdV

or δQ = dU + PdV

On a unit-mass basis

δq = de + pdv

δq = du + pdv

slide22

3. Cycle

δq = du + δw

∮δq = ∮du + ∮δw

since∮du = 0

then∮δ q = ∮δw

if ∮δ q = 0

∮δw =0

This can illustrate that the first kind of perpetual motion machine can’t be produced

slide23

4.Reversible Process under a Constant Pressure

δQ = dU + PdV

Since p=const

δQ = dU + d(pV)

5.Isolated System

dE = 0

3 5 specific heats
3-5 Specific Heats

3-5-1 Definition of specific heat

The energy required to raise the temperature of the unit mass of a substance by one degree

Then q=CT or δq=CdT

3-5-2 Specific heat at constant volume

The specific heat at constant volume Cv can be viewed as the energy required to raise the temperature of unit mass of substance by 1 degree as the volume is maintained constant.

At constant volume , δq = du

CvdT=du

slide25

3-5-3 Specific heat at constant pressure

The specific heat at constant volume Cp can be viewed as the energy required to raise the temperature of unit mass of substance by 1 degree as the volume is maintained constant pressure.

Similarly, at constant pressure

δq = du+ δ w=du+Pdv=du+d(Pv)=dh

CpdT=dh

slide26

3-5-4 Specific Heats of Ideal-Gas

A: Specific heat at constant volume

Since there are no attraction among molecules of ideal-gas,then:

u= f (T )

slide27

B: Specific heat at constant pressure

Since:u= f (T )

h=u+pv

=f (T ) +RT

=f ’( T )

3 6 the internal energy enthalpy of ideal gas
3-6The internal energy, enthalpy of Ideal-Gas

2-7-1 Internal energy and enthalpy

slide29

We define that u =0 while T =0, then:

Obviously, h =0 while T =0, then:

Meanwhile:

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