lecture 5 first law of thermodynamics. you can’t get something for nothing. nothing is for free....
TRANSCRIPT
First Law of ThermodynamicsFirst Law of Thermodynamics
You can’t get something for nothing.
Nothing is for free.
We will discuss these statements later…
Thermodynamic SystemThermodynamic System
Consider a closed system (e.g., a parcel of air).
It has internal energy (“u”) = energy due to molecular kinetic and potential energies.
Suppose some energy (dq) is added to the system.
Example: via radiation from the sun
What happens?
Thermodynamic SystemThermodynamic System
Some of the energy goes into work done (dw) by the system against its surroundings.
Example: expansion
What’s left is a change in internal energy.
du = dq – dw
Conservation of Energy principle
“nothing is for free”
Thermodynamic SystemThermodynamic System
System
EnvironmentHeat
System can exchange energy with environment via heat flow.
Thermodynamic SystemThermodynamic System
In addition, system can do work on environment or vice versa.
Example: expansion
First Law, General FormFirst Law, General Form
dU = dQ – dWdU = dQ – dW
dU = change in internal energy of systemdU = change in internal energy of system
dQ = heat exchanged with environmentdQ = heat exchanged with environment dQ > 0 dQ > 0 heat flowing into system heat flowing into system
dW = work done by or on systemdW = work done by or on system dW > 0 dW > 0 system is doing work system is doing work
Ideal GasIdeal Gas
Consider a system consisting of an ideal Consider a system consisting of an ideal gas in a cylinder.gas in a cylinder.
Cylinder has a piston, which allows Cylinder has a piston, which allows volume to be changed.volume to be changed.
CylinderCylinderweights
more weight, more pressure
Gas
Walls of cylinder:
1) perfect heat conductors
2) perfect insulators
CasesCasesCase 1: Walls of cylinder are perfect Case 1: Walls of cylinder are perfect conductorsconductors heat can freely flow between system and heat can freely flow between system and
environmentenvironment in equilibrium, temperature of system must in equilibrium, temperature of system must
equal temperature of environmentequal temperature of environment
Case 2: Walls of cylinder are perfect Case 2: Walls of cylinder are perfect insulatorsinsulators no heat flow between system and no heat flow between system and
environmentenvironment temperatures of system and environment temperatures of system and environment
need not be equalneed not be equal
Work (Qualitative)Work (Qualitative)
System does work on environment System does work on environment (dW > 0) if gas expands(dW > 0) if gas expands (Piston is pushed upward.)(Piston is pushed upward.)
Work is done on system (dW < 0) if Work is done on system (dW < 0) if gas contractsgas contracts (Piston is pushed downward.)(Piston is pushed downward.)
Work (Quantitative)Work (Quantitative)
Suppose piston is pushed upward a distance dx.Suppose piston is pushed upward a distance dx.
Work (Quantitative)Work (Quantitative)
Suppose piston is pushed upward a distance dx.Suppose piston is pushed upward a distance dx.
dx
Area of piston = A
Pressure force = pA
dW = pAdx
= pdV
First Law, Ideal GasFirst Law, Ideal Gas
dVpdQdU Usually, we are interested in energy per unit mass
Divide both sides by m
Define u = U/m; q = Q/m; = V/m
Internal EnergyInternal Energy
For an ideal gas, For an ideal gas, uu is a function of T only is a function of T only u is an increasing function of Tu is an increasing function of T
Change in internal energy depends only Change in internal energy depends only on change in temperature.on change in temperature. Doesn’t depend on the way in which that Doesn’t depend on the way in which that
temperature change is accomplished.temperature change is accomplished. du = kdu = kdT, where k is a constantdT, where k is a constant (Value of k will be determined shortly.)(Value of k will be determined shortly.)
Heat Capacity, CHeat Capacity, C
dT
dQC
For a gas, C depends on the particular process.
Cv = heat capacity at constant volume (dV = 0)
Cp = heat capacity at constant pressure (dp = 0)
SI units: JK-1
Amount of heat required to change a “body’s” temperature by a given amount
Specific HeatSpecific Heat
Specific heat is heat capacity Specific heat is heat capacity per unit massper unit mass
ccvv (lower case) = specific heat at constant (lower case) = specific heat at constant
volumevolume
ccpp = specific heat at constant pressure = specific heat at constant pressure
Specific heat is the heat energy needed to Specific heat is the heat energy needed to raise the temperature of a unit mass of a raise the temperature of a unit mass of a substance by one degree. substance by one degree.
Specific HeatSpecific Heat
vv dT
dqc
dT
dq
Suppose we add some thermal energy (dq) to a unit mass of a substance like air, water, soil.
We expect T(substance) to increase
How much?
We can define Specific Heat as
Heat added
Temp change
pp dT
dqc
Constant volume Constant pressure
Specific Heat of Dry AirSpecific Heat of Dry Air
ccvv = 717 J = 717 Jkgkg-1-1KK-1-1
ccpp = 1004 J = 1004 Jkgkg-1-1KK-1-1
Note: cNote: cpp – c – cvv = 287 J = 287 Jkgkg-1-1KK-1-1
Look familiar?Look familiar? ccpp – c – cvv = R = Rdd
(Not a coincidence!)(Not a coincidence!)
Internal Energy ChangeInternal Energy Change
The following is The following is alwaysalways true: true:
Tdcdu v (3.40) W&H
Constant-Pressure ProcessesConstant-Pressure Processes
Go back to ideal-gas law:Go back to ideal-gas law:
RTp Take differential of both sides:
dTRpd )(