2nd Law of Thermodynamics
Entropy and disorder.
Two classical statements of the Second Law of Thermodynamics:
| Kelvin & Planck "No (heat) engine whose working fluid undergoes a cycle can absorb heat from a single reservoir, deliver an equivalent amount of work, and deliver no other effect" |
| Clausius "No machine whose working fluid undergoes a cycle can absorb heat from one system, reject heat to another system and produce no other effect" |
Both statements of the Second Law constrains the First Law of Thermodynamics by identifying that energy goes downhill. The Second Law is concerned with Entropy (S) which is produced by all processes and associated with the loss of ability to do work. The Second Law states that the entropy of the universe increases.
For energy to be available there must be a region with high energy level and a region with low energy level. Useful work must be derived from the energy that flows from the high level to the low level.
- 100% energy can not be transformed to work
- entropy can be produced but never destroyed
Efficiency of a heat machine
The thermodynamic efficiency of a heat machine working between two energy levels is defined in terms of absolute temperature and can be expressed as
η = (Th - Tc) / Th = 1 - Tc / Th (1)
where
η = efficiency
Th = temperature high level (K)
Tc = temperature low level (K)
As a consequence, to attain maximum efficiency - Tc has to be as cold as possible. For 100% efficiency Tc should equals to 0 K. This is in real life impossible so the efficiency will always be less than 1 (100%).
| Change in entropy > 0 irreversible process |
Change in entropy = 0 reversible process |
Change in entropy < 0 impossible process |
Entropy is used to define the unavailable energy in a system and entropy defines the relative ability of one system to act on an other. As energy moves toward lower energy levels where one is less able to act upon the surroundings, the entropy is said to increase.
- For the universe as a whole - the entropy is increasing
- Entropy is not conserved like energy
Go to Thermodyamics key values internationally agreed, Standard state and enthalpy of formation, Gibbs free energy of formation, entropy and heat capacity and Standard enthalpy of formation, Gibbs energy of formation, entropy and molar heat capacity of organic substances for listing of values for a lot of inorganic and organic substances.
Thermodynamic Entropy
Change of entropy in a thermodynamic system can be expressed as
dS = d H / Ta (2)
where
dS = change in entropy (kJ/kg K)
dH = change in enthalpy or internal energy (kJ/kg K)
Ta = average temperature (K)
|
Carnot Heat Cycle The sum of (dH / T) values for each step in the Carnot cycle equals 0. This only happens because for every positive H there is a countering negative H, overall. |
Example - Entropy Heating Water
A process raises 1 kg of water from 0 to 100oC (273 to 373 K) under atmospheric conditions.
Specific enthalpy at 0oC (hf) = 0 kJ/kg (from steam tables) (Specific - per unit mass)
Specific enthalpy of water at 100oC (hf) = 419 kJ/kg (from steam tables)
Change in specific entropy:
dS = dH / Ta
= [(419 kJ/kg) - (0 kJ/kg)] / [((273 K) + (373 K)) / 2]= 1.297 kJ/kgK
Example - Entropy Evaporation Water to Steam
A process changes 1 kg of water at 100oC (373 K) to saturated steam at 100oC (373 K) under atmospheric conditions.
Specific enthalpy of steam at 100oC (373 K) before evaporating = 418 kJ/kg (from steam tables)
Specific enthalpy of steam at 100oC (373 K) after evaporating = 2675 kJ/kg (from steam tables)
Change in specific entropy:
dS = dH / Ta
= [(2675 kJ/kg) - (418 kJ/kg)] / [((373 K) + (373 K)) / 2]
= 6.054 kJ/kgK
The total change in specific entropy from water at 100oC to saturated steam at 100oC is the sum of the change in specific entropy for the water, plus the change of specific entropy for the steam.
Example - Entropy Superheated Steam
A process superheats 1 kg of saturated steam at atmospheric pressure to 150oC (423 K).
Specific total enthalpy of steam at 100oC (373 K) = 2675 kJ/kg (from steam tables)
Specific total enthalpy of superheated steam at 150oC (423 K) = 2777 kJ/kg (from steam tables)
Change in specific entropy:
dS = dH / Ta
= [(2777 kJ/kg) - (2675 kJ/kg)] / [((423 K) + (373 K)) / 2]
= 0.256 kJ/kgK
Related Topics
-
Thermodynamics
Work, heat and energy systems.
Related Documents
-
1st Law of Thermodynamics
The First Law of Thermodynamics simply states that energy can be neither created nor destroyed (conservation of energy). Thus power generation processes and energy sources actually involve conversion of energy from one form to another, rather than creation of energy from nothing. -
Adiabatic Flame Temperatures
Adiabatic flame temperatures for hydrogen, methane, propane and octane - in Kelvin. -
Carnot Efficiency
The efficiency of the Carnot cycle. -
Combustion Heat
Heat of combustion (energy content) for som common substances - with examples how to calculate heat of combustion. -
Compressible Gas Flow - Entropy
Calculating the entropy in a compressible gas flow. -
Efficiency
Efficiency is the ratio useful energy output to energy input. -
Equilibrium
The mechanical, thermal, electrostatic, phase or chemical states of equilibrium. -
Standard State and Enthalpy of Formation, Gibbs Free Energy of Formation, Entropy and Heat Capacity
Definition and explanation of the terms standard state and standard enthalpy of formation, with listing of values for standard enthalpy and Gibbs free energy of formation, as well as standard entropy and molar heat capacity, of 370 inorganic compounds. -
Standardized Enthalpies and Entropies
Standardized enthalpies and entropies for some common substances. -
Steam Entropy
Basic steam thermodynamics - entropy diagram. -
Superheated Steam - Enthalpy
Enthalpy of steam superheated to temperatures above it's boiling point. -
Superheated Steam - Entropy
The entropy of steam superheated to temperatures above saturation points. -
Symbols Used to Denote a Chemical Reactions and Process or Condition
Explanation of symbols used as subscripts or superscripts to tell more about the type of chemical reaction, process or condition. -
Thermodynamic Key Values Internationally Agreed
Internationally agreed, internally consistent, values for the thermodynamic properties (standard enthalpy of formation, entropy and [H°(298)-H°(0)]) of key chemical substances. -
Thermodynamic Terms - Functions and Relations
Common thermodynamic terms and functions - potential energy, kinetic energy, thermal or internal energy, chemical energy, nuclear energy and more. -
Third Law of Thermodynamics
The entropy of a substance is zero if the absolute temperature is zero. -
WABT - Weighted Average Bed Temperature
Definition and examples of calculation of weighted average bed temperature in adiabatic reactors. -
Water-Steam Mollier Diagram
Enthalpy-entropy diagram for water and steam. -
Wet Steam - Enthalpy
Wet steam, dryness fraction and enthalpy. -
Zeroth Law of Temperature
The direction of heat flow.
