Energy is the lifeblood of chemical processes. The governs how energy flows and changes forms in steady-state systems, where conditions remain constant over time.
In non-reactive processes, energy transfers occur through heat, work, and changes in kinetic and potential energy. Understanding these transfers is crucial for analyzing and optimizing various industrial equipment and operations.
Thermodynamic Principles and Energy Transfers
First law in steady-state systems
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First law of thermodynamics asserts energy conservation principle stating energy cannot be created or destroyed, only converted between forms (heat, work, internal energy)
Steady-state operation maintains constant system conditions over time with no accumulation of mass or energy within system boundaries (input rates equal output rates)
equation ΔE=Q−W quantifies energy changes where ΔE represents internal energy change, Q denotes heat added to system, and W signifies work done by system
System boundaries define scope of analysis:
Closed systems allow only energy transfer, no mass exchange (steam turbine)
Open systems permit both mass and energy transfer across boundaries ()
Energy transfers in non-reactive processes
Heat transfer occurs through:
in solid materials (heat flow through metal pot)
in fluids (hot air rising in a room)
via electromagnetic waves (solar energy reaching Earth)
Work manifests as:
Shaft work in rotating machinery (turbines, pumps)
Flow work from fluid movement (compressed air systems)
Electrical work due to current flow (electric motors)
Kinetic energy relates to velocity of moving objects or fluids, calculated as KE=21mv2 (flowing water in pipes)
Potential energy exists as:
Gravitational potential PE=mgh (water in elevated tanks)
Elastic potential stored in compressed springs or gases (pneumatic systems)
Internal energy encompasses all microscopic energy forms within a system (molecular vibrations, rotations)
H=U+PV proves useful for processes (steam power plants)
Energy balances for non-reactive systems
General energy balance equation states Ein+Egenerated=Eout+Eaccumulated
Steady-state simplification reduces to Ein=Eout
Process equipment energy balances:
Heat exchangers: Q=mcpΔT (shell and tube heat exchangers)
Pumps and compressors: W=m(hout−hin) (centrifugal pumps)
Turbines: W=m(hin−hout) (gas turbines)
Reference states establish baselines for energy calculations (standard temperature and pressure)
Psychrometric charts aid in analyzing air-water vapor mixtures (HVAC systems)
Steam tables provide water and steam properties at various conditions (boiler operations)
Efficiency of non-reactive processes
Energy efficiency defined as ratio of useful output energy to input energy η=EinEout×100%
Carnot efficiency represents maximum theoretical efficiency for heat engines ηCarnot=1−THTC
Identifying energy losses helps improve efficiency:
Friction in moving parts (bearings, seals)
Heat leakage through (furnaces, reactors)
Irreversibilities in real processes (throttling valves)
Process integration techniques enhance overall efficiency:
Heat integration through pinch analysis optimizes heat exchanger networks
Cogeneration combines heat and power production (combined cycle power plants)