- There exists for every system a property called energy, . The system energy can be considered as a sum of internal energy, kinetic energy, potential energy, and chemical energy.
- Like the Zeroth Law, which defined a useful property, “temperature,” the First Law defines a useful property called “energy.”
- The two new terms (compared to what you have seen in physics and dynamics, for example) are the internal energy and the chemical energy. For most situations in this class, we will neglect the chemical energy. We will generally not, however, neglect the internal energy, . It arises from the random or disorganized motion of molecules in the system, as shown in Figure 2.1. Since this molecular motion is primarily a function of temperature, the internal energy is sometimes called “thermal energy.”
Figure 2.1: Random motion is the physical basis for internal energy |
Recall that for pure substances the entire state of the system is specified if any two properties are specified. (We will discuss the equations that relate the internal energy to these other variables as the course progresses.)
- The change in energy of a system is equal to the difference between the heat added to the system and the work done by the system,
(2..1) |
- where is the energy of the system,
is the heat input to the system, and
is the work done by the system.
(thermal energy) +- Like the Zeroth Law, the First Law describes the behavior of the new property
- The equation can also be written on a per unit mass basis
- In many situations the potential energy, kinetic energy, and chemical energy of the system are constant or not important. Then
- and
- Sometimes this difference is emphasized by writing the First Law in differential form,
(2..2) |
- where the symbol “ ” is used to denote that these are not exact differentials but rather are dependent on path.
- Note that the signs are important:
- is defined to be positive if it is transferred to the system; thus the numerical value we substitute for will be positive if heat is transferred to the system from the surroundings, and negative if heat is transferred from the system to the surroundings.
- is defined to be positive if it is done by the system (see Section 1.3); thus the numerical value we substitute for will be positive if the system is doing work, and negative if work is being done on the system.
- For quasi-static processes we can substitute ,
- To give an example of where the first law is applied, consider the device shown in Figure 2.2. We heat a gas, it expands against a weight, some force (pressure times area) is applied over a distance, and work is done. The change in energy of the system supplies the connection between the heat added and work done. We will spend most of the course dealing with various applications of the first law — in one form or another.
Figure 2.2: The change in energy of a system relates the heat added to the work done |
The form of the first law we have given here is sometimes called the “control mass” form, because it is well suited to dealing with systems of a fixed mass. We will see in Section 2.5 that this form can be written for a control volume with mass flow in and mass flow out (like a jet engine for example). We will call this the “control volume” form of the first law
The first law in closed system
The equation
E_{in}-E_{out}=ΔE_{system}
Q-W=ΔE_{system}=ΔU
Q=ΔU+W
Per unit mass:
q= Δu+w
dq=du+dw
If the process is reversible, then:
dq=du+pdv
This is the first equation of the first law.
Here q, w, Δu is algebraic.
The only way of the heat change to mechanical energy is expansion of working fluid.
The first law in open system
1. Stead flow
For stead flow, the following conditions are fulfilled:
The matter of system is flowing steadily, so that the flow rate across any section of the flow has the same value;
The state of the matter at any point remains constant;
Q, W flow remains constant;
2. Flow work
W_{flow}=pfΔs=pV
w_{flow}=pv
3.
“ W_{t}” are expansion work and the change of flow work for open system.
4.
“ W_{s}” is “ W_{t}” and the change of kinetic and potential energy of fluid for open system.
5. Enthalpy
for flow fluid energy:
For Per unit mass:
h=u+pv unit: J/kg, kJ/kg
6. Energy equation for steady flow open system
If neglect kinetic energy and potential energy , then:
If the process is reversible, then:
This is the second equation of the first law.
7. Energy equation for the open system
Energy equation for the open system