1. Chapter 7 Energy and Energy Balance
By :Dr Ku Syahidah Ku Ismail

2. Importance of Energy Calculations
You’ve seen that raw materials and products must be moved into and out of various reactors, mixers, and separators. All these operations involve energy.
Eg. How much power (energy/time) is required to pump 1000 L/h of water from storage vessel to a process unit? (This answer determines the size of the required pump motor.)
Eg. How much coal must be burned each day to produce enough energy to generate the steam to run the turbines to produce enough electricity to meet the daily power requirements of a city of 500,000 people?

3. Forms of Energy Three component of total energy of a system
Kinetic energy (Ek)
energy due to the translational motion of the system as a whole relative to some frame of reference (usually the earth’s surface) or to rotation of the system about some axis.
Potential energy (Ep)
energy due to the position of the system in a potential field (such as a gravitational or electromagnetic field).
Internal energy (U)
all energy possessed by a system other than kinetic and potential energy; or
Energy due to translation, rotation, vibration & electromagnetic interactions of the molecules, atom and subatomic particle within the system.

4. Transfer of Energy
In closed system (i.e. no mass is transferred across the system boundaries while the process is taking place), energy may be transferred between such a system and its surroundings in two ways as heat or work.
Heat
Energy that flows as a result of temperature difference between a system and its surroundings.
The direction of flow is always from a higher temperature to a low one.
Heat is defined as positive when its transferred to the system from the surroundings.
Work
energy that flows in response to any driving force other a temperature difference, such as a force, a torque or a voltage
Work is defined as positive when it is done by the system on the surroundings.

5. First Law of Thermodynamics
Law of conservation of energy, which state that energy can neither be created nor destroyed.
General form of first law of thermodynamics
Inlet Energy + Heat - Outlet Energy – Work = Accumulation
Inlet energy and outlet energy is summation/total of all energy such as potential, kinetic and internal energy

6. Kinetic Energy Equation (Ek)
Kinetic energy, Ek (J) of an object of mass m (kg) moving with velocity u (m/s) relative to the surface of the earth is
If the fluid enters a system with a mass flow rate (kg/s) and uniform velocity u (m/s), the rate at which kinetic energy (J/s) is transported into the system is

7. Potential Energy Equation (Ep)
Gravitational potential energy, Ep
if the fluid enters a system with a mass flow rate (kg/s) and an elevation z relative to the potential energy reference plane.
Normally we are interested in the change of potential energy during energy balance calculation

8. Example 7.2-1
Water flows into a process unit through a 2 cm ID pipe at a rate of 2 m3/h. Calculate the kinetic energy transport in this stream in unit J/s.
Solution:
Ek= N.m/s= J/s

9. Class Discussion

10. Energy Balances on Closed System
no mass is transferred across the system boundaries while the process is taking place
Energy balance
Final System Energy – Initial System Energy
= Net Energy Transferred to the System
Initial energy system = Ui + Eki + Epi
Final energy system = Uf + Ekf + Epf
Net energy transfer = Q-W
(Uf-Ui) + (Ekf-Eki) + (Epf-Epi) = Q-W

11. Energy Balances on Closed System
When applying energy balance equation to a given process, you should be aware of the following points;
The internal energy of a system depends almost entirely on the chemical composition, state of aggregation (solid, liquid, or gas), and temperature of the system materials. If no temperature changes, phase changes, or chemical reactions occur in a closed system and if pressure changes are less than a few atmospheres, then ∆U ≈ 0.
If a system is not accelerating, then ∆Ek = 0. If a system is not rising or falling, then ∆Ep = 0.
If a system and its surroundings are at the same temperature or the system is perfectly insulated, then Q = 0. The process is then termed adiabatic.
Work done on or by a closed system is accomplished by movement of the system boundary against a resisting force or the passage of an electrical current or radiation across the system boundary. If there are no moving parts or electrical current at the system boundary, then W = 0.

12. Class Discussion
Example
7.3-1

13. Example 7.3-1
A gas is contained in a cylinder fitted with a movable piston. The initial gas temperature is 25C. The cylinder is placed in boiling water with the piston held in a fixed position. Heat in the amount of 2 kcal is transferred to the gas, which equilibrates at 100C.
The piston is then released, and the gas does 100 J of work in moving the piston to its new equilibrium position. The final gas temperature is 100C.
Write the energy balance equation. Solve the unknown energy term. Express energy in Joules.

14. Energy Balances on Open System
In open system, mass is transferred across the system boundaries while the process is taking place.
Therefore work must be done on open system to push mass in and work is done on the surrounding by mass that emerges from the systems.
Both work terms must be include in the energy balance for open system
The net work done by an open system
and
- shaft work
rate of work done by the process fluid on a moving part within the system such as a pump rotor.
- flow work
rate of work done by the fluid at the system outlet minus rate of work done by the fluid at the system inlet.

15. Energy Balances on Open System
^ symbol is used to denote the specific property (property divided by mass or by mole) such as specific internal energy (Û kJ/kg), specific volume ( m3/kg) and so on.
One important property for energy balance on open system is specific enthalpy (Ĥ kJ/kg).
Sometimes, universal gas law constant can be used as a conversion factor to evaluate specific enthalpy.

16. Class Discussion
Example
7.4-1

17. Example 7.4-1
The specific internal energy of helium at 300K, 1 atm is 3800 J/mol.
The specific molar volume, 300 K, 1 atm is L/mol.
Calculate:
Specific enthalpy of helium at 300K, 1 atm
The rate at which the enthalpy is transported by a stream of helium at 300K, 1 atm with a molar flowrate of 250 kmol/h.

18. Energy Balances Equation for Open System

19. Class Discussion
Example
7.4-2

20. Reference States and State Properties
It is not possible to know the absolute value of Û and Ĥ for a process material, but we can determine the change in ΔÛ and change in ΔĤ corresponding to a specific change of state (temperature, pressure, phase).
A convenient way to tabulate ΔÛ and ΔĤ is to choose a temperature, pressure and state of aggregation (i.e. phase) as a reference state.
Since Ĥ cannot be known absolute, for convenience we may assign a value Ĥo=0 to be reference state. Then ΔĤ1= Ĥ1-0; ΔĤ2= Ĥ2-0 and so on.
Some enthalpy tables give the reference states on which the listed values of Ĥ are based and others do not.
However, we do not have to know the reference state to calculate ΔĤ for the transition from one state to another state since the value are based on the same reference in the table.
Ĥ and Û can be said as state properties
Property whose change of value in any process depend only on it initial and final states and do not depend on the path take to reach the state.

21. Class Discussion
Example
7.5-1

22. Phase Diagram for Water

23. Class Discussion Example 7.5-2
Steam Table
Class Discussion
Example
7.5-2

24. Example 7.5.2
1. Determine the vapor pressure, specific internal energy, and specific enthalpy of saturated steam at 133.5C.
Show that water at 400C and 10 bar is superheated steam and determine its specific volume, specific internal energy and specific enthalpy relative to liquid water at the triple point, and its dew point.

25. Class Discussion
Example
7.5-3

26. Energy Balance Tips
When labeling flowchart, write down together the temperature, pressure and state of aggregation of the process material eg. H2O(s) or H2O(v)
Normally (depend on the process description) for chemical process unit; shaft work, kinetic and potential energy change tend to be negligible compared to heat flows, internal energy and enthalpy changes.
Then simplified energy balance become
Closed System:
Open System:

27. Class Discussion
Example
7.6-1

28. Class Discussion
Example
7.6-3

29. Simultaneous Material and Energy Balance
Saturated steam at 1 atm is discharged from a turbine at a rate of 1150 kg/h. Superheated steam at 300C and 1 atm is needed as a feed to a heat exchanger; to produce it, the turbine discharge stream is mixed with superheated steam available from a second source at 400C and 1 atm. The mixing unit operates adiabatically. Calculate the amount of superheated steam at 300C produced and the required volumetric flow rate of the 400C steam.

30. Mechanical Energy Balance
Important in the operations involve the flow of fluids to, from and between tanks, reservoirs and process unit.
Mechanical energy balance for steady state flow of an incompressible fluid; where F is friction loss
Bernoulli equation
Simplified mechanical energy balance for frictionless process (F=0) in which no shaft work is performed (Ws=0).

31. Class Discussion
Example
7.7-1

32. Class Discussion
Example
7.7-2

33. Class Discussion
Example
7.7-3