This document provides an overview of thermodynamics concepts including:
- The various forms of energy and definitions of key terms like system, surroundings, and boundary.
- The three laws of thermodynamics - the zero law states thermal equilibrium is transitive, the first law concerns conservation of energy, and the second law involves entropy and the spontaneity of processes.
- Other concepts like heat, work, internal energy, and free energy are discussed in relation to the first and second laws. Examples are provided to illustrate applications of the principles.
State of matter and properties of matter (Part-2) (Latent Heat, Vapour pressu...Ms. Pooja Bhandare
Latent Heat, Vapour pressure, Factor affecting vapour pressure, Surface area, Types of molecule, Temperature and Intermolecular forces, Sublimation Critical point
States of matter and properties of matterJILSHA123
States of matter and properties of matter, latent heat, vapour pressure, aerosols - inhalers, sublimation critical point, eutectic mixtures, gas laws, Gibbs phase rule, crystalline structures, 3rd b.pharmacy, sanjo college of pharmaceutical studies, palakkad, kerala
Solubility of drugs: Solubility expressions, mechanisms of solute solvent interactions, ideal solubility parameters, solvation & association, quantitative approach to the factors
influencing solubility of drugs, diffusion principles in biological systems. Solubility
of gas in liquids, solubility of liquids in liquids, (Binary solutions, ideal solutions)
Raoult’s law, real solutions. Partially miscible liquids, Critical solution temperature . Distribution law, its limitations and applications
State of matter and properties of matter (Part-4)(Gases, Ideal gas law)Ms. Pooja Bhandare
Gases, Properties of gases, Kinetic Molecular Theory of Ideal Gases, The Gas laws:1.Boyle’s Law ( The Pressure – Volume relationship), 2.Charles’s law( The Temperature- Volume relationship), 3. Gay- Lussac’s law( The Pressure- Temperature relationship), 4. Avogadro’s Law ( The Volume – Amount relationship), Ideal Gas Law:
State of matter and properties of matter (Part-2) (Latent Heat, Vapour pressu...Ms. Pooja Bhandare
Latent Heat, Vapour pressure, Factor affecting vapour pressure, Surface area, Types of molecule, Temperature and Intermolecular forces, Sublimation Critical point
States of matter and properties of matterJILSHA123
States of matter and properties of matter, latent heat, vapour pressure, aerosols - inhalers, sublimation critical point, eutectic mixtures, gas laws, Gibbs phase rule, crystalline structures, 3rd b.pharmacy, sanjo college of pharmaceutical studies, palakkad, kerala
Solubility of drugs: Solubility expressions, mechanisms of solute solvent interactions, ideal solubility parameters, solvation & association, quantitative approach to the factors
influencing solubility of drugs, diffusion principles in biological systems. Solubility
of gas in liquids, solubility of liquids in liquids, (Binary solutions, ideal solutions)
Raoult’s law, real solutions. Partially miscible liquids, Critical solution temperature . Distribution law, its limitations and applications
State of matter and properties of matter (Part-4)(Gases, Ideal gas law)Ms. Pooja Bhandare
Gases, Properties of gases, Kinetic Molecular Theory of Ideal Gases, The Gas laws:1.Boyle’s Law ( The Pressure – Volume relationship), 2.Charles’s law( The Temperature- Volume relationship), 3. Gay- Lussac’s law( The Pressure- Temperature relationship), 4. Avogadro’s Law ( The Volume – Amount relationship), Ideal Gas Law:
Solubility of Drugs (PHYSICAL PHARMACEUTICS-I)Rakesh Mishra
Solubility expressions, mechanisms of solute solvent interactions,solubility parameters, factors influencing
solubility of drugs, diffusion principles in biological systems, Raoult’s law, real solutions. Partially miscible
liquids(Phase equilibria, Phase rule, One , two and three component systems, ternary phase
diagram, Critical solution temperature and applications). Distribution law, its limitations and
applications
Solubility of liquids in liquids, The term miscibility refers to the mutual solubility of the component of liquid - liquid system, Raoult’s Law, Raoult’s law may be mathematically expressed as: Ideal solution, Real solution
State of matter and properties of matter (Part-6)(Relative humidity, Liquid ...Ms. Pooja Bhandare
RELATIVE HUMIDITY, Humidity, Wet and Dry Hygrometer, LIQUID COMPLEX, LIQUID CRYSTALS, Types of liquid crystals, GLASSY STATES, Characteristics glassy state, Types of glassy state, What is the Glass Transition Temperature?
State of matter, Properties of various state of matter, Volume, Diffusion, Compressibility, Rigidity or Fluidity, Density, Shape, Kinetic energy of particles at a given temperature, Intermolecular space, Intermolecular Force of attraction, Arrangement of molecules, Changes in the state of matter, Enthalpy, Entropy, Triple point, Freezing, Melting, Deposition, Sublimation, Vaporization and Condensation
Solubility of Drugs (PHYSICAL PHARMACEUTICS-I)Rakesh Mishra
Solubility expressions, mechanisms of solute solvent interactions,solubility parameters, factors influencing
solubility of drugs, diffusion principles in biological systems, Raoult’s law, real solutions. Partially miscible
liquids(Phase equilibria, Phase rule, One , two and three component systems, ternary phase
diagram, Critical solution temperature and applications). Distribution law, its limitations and
applications
Solubility of liquids in liquids, The term miscibility refers to the mutual solubility of the component of liquid - liquid system, Raoult’s Law, Raoult’s law may be mathematically expressed as: Ideal solution, Real solution
State of matter and properties of matter (Part-6)(Relative humidity, Liquid ...Ms. Pooja Bhandare
RELATIVE HUMIDITY, Humidity, Wet and Dry Hygrometer, LIQUID COMPLEX, LIQUID CRYSTALS, Types of liquid crystals, GLASSY STATES, Characteristics glassy state, Types of glassy state, What is the Glass Transition Temperature?
State of matter, Properties of various state of matter, Volume, Diffusion, Compressibility, Rigidity or Fluidity, Density, Shape, Kinetic energy of particles at a given temperature, Intermolecular space, Intermolecular Force of attraction, Arrangement of molecules, Changes in the state of matter, Enthalpy, Entropy, Triple point, Freezing, Melting, Deposition, Sublimation, Vaporization and Condensation
thermodynamics. in physical world outside and inside the living body. important factor for heat and energy for the living.
different forms of energy, kinetic energy and pottential energy.
different forms of system, open and closed. laws of thermodynamics and gibbs free energy. entrophy and enthalphy
in this module all the relevant topics of thermodynamics and kinetics has been covered according to the engineering chemistry syllabus and also you can practice questions of thermodynamics and kinetics from this given module. this module is very easy to understand
as everything given is in simple language with figures
The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic systems. The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but cannot be created or destroyed.
General Summary of Thermodynamics
FIRST LAW OF
THERMODYNAMICS:
The total amount of energy (and
mass) in the universe is constant.
That is, in any process energy can
be changed from one form to
another; but, it can never be
created nor destroyed.
“ You can’t get something for
nothing”
SECOND LAW OF
THERMODYNAMICS:
In any spontaneous process the
entropy of the universe increases:
Suniverse = Ssystem + Ssurroundings
or
Suniverse -Ssurroundings = Ssystem
(Variant)In trying to do work, you
always lose energy to the
surroundings.
“You can’t even break even!”
THIRD LAW OF
THERMODYNAMICS:
Any pure crystalline substance at
a temperature of absolute zero
(0.0K) has an entropy of zero
(S = 0.0 J/K-mol).
Terminology:
Energy = capacity to do work
System = portion of the universe we are considering
Open system = energy and matter can transfer
Closed system = energy transfers
Isolated system = no transfers
Surroundings = everything else besides the system
Isothermal = system at constant temperature
Heat capacity = amt. of heat required to raise the temperature of a
certain amt. of material by 1C or 1K.
Calorie = amt. of heat required to raise the temperature of 1g of water
by 1ºC.
Signs:
H >0 or (+) heat absorbed (endo)
H <0 or (-) heat released (exo)
S >0 or (+) entropy increasing (becoming disordered)
S <0 or (-) entropy decreasing (becoming ordered)
G >0 or (+) nonspontaneous Kc <1
G = 0, Kc = 1
G < 0 or (-) spontaneous Kc >1
Rules about Entropy: (Entropy increases)
1. w/ increasing temperature*
2. as one goes from s -> l -> aq ->g*
3. if a solid or liquid is dissolved in a solvent*
4. number of particles increases*
5. mass of the molecule increases
6. Entropy is higher for weakly bonded materials than for strong
covalent materials
7. As complexity of a molecule increases.
FORMULA’S:
G = H- TS (T in K = 273 + C)
T = H/S (assume G = 0 or when Kc = 1, like fusion/vaporization)
Hrxn = (#mol.) *(Hf(products)) - (#mol.) *(Hf(reactants)) = kJ
Srxn = (#mol.) *(S(products)) - (#mol.) *(S(reactants) ) = J/K (Watch Out -> J to kJ)
Grxn = (#mol.) *(Gf(products)) - (#mol.) *(Gf(reactants)) = kJ
G = -RTlnKc or Kc = e
-(G/RT)
Remember: e
x
is 2
nd
function natural log (ln) on calculator and work inside-out
H S G
+ + (+/-) (Spont. Only at High Temp. when TS > H)
- + - (Spontaneous at ALL Temperatures)
- - (+/-) (Spont. Only at Low Temp. when TS < H)
+ - + (Non-spontaneous at ALL Temperatures)
G = H- TS when G is – gives a spontaneous
reaction
Enthalpy (H): The Energy of motion or transition.
q is the heat measured from a reaction. If rxn is at constant pressure q = H
.
Richard's aventures in two entangled wonderlandsRichard Gill
Since the loophole-free Bell experiments of 2020 and the Nobel prizes in physics of 2022, critics of Bell's work have retreated to the fortress of super-determinism. Now, super-determinism is a derogatory word - it just means "determinism". Palmer, Hance and Hossenfelder argue that quantum mechanics and determinism are not incompatible, using a sophisticated mathematical construction based on a subtle thinning of allowed states and measurements in quantum mechanics, such that what is left appears to make Bell's argument fail, without altering the empirical predictions of quantum mechanics. I think however that it is a smoke screen, and the slogan "lost in math" comes to my mind. I will discuss some other recent disproofs of Bell's theorem using the language of causality based on causal graphs. Causal thinking is also central to law and justice. I will mention surprising connections to my work on serial killer nurse cases, in particular the Dutch case of Lucia de Berk and the current UK case of Lucy Letby.
THE IMPORTANCE OF MARTIAN ATMOSPHERE SAMPLE RETURN.Sérgio Sacani
The return of a sample of near-surface atmosphere from Mars would facilitate answers to several first-order science questions surrounding the formation and evolution of the planet. One of the important aspects of terrestrial planet formation in general is the role that primary atmospheres played in influencing the chemistry and structure of the planets and their antecedents. Studies of the martian atmosphere can be used to investigate the role of a primary atmosphere in its history. Atmosphere samples would also inform our understanding of the near-surface chemistry of the planet, and ultimately the prospects for life. High-precision isotopic analyses of constituent gases are needed to address these questions, requiring that the analyses are made on returned samples rather than in situ.
Richard's entangled aventures in wonderlandRichard Gill
Since the loophole-free Bell experiments of 2020 and the Nobel prizes in physics of 2022, critics of Bell's work have retreated to the fortress of super-determinism. Now, super-determinism is a derogatory word - it just means "determinism". Palmer, Hance and Hossenfelder argue that quantum mechanics and determinism are not incompatible, using a sophisticated mathematical construction based on a subtle thinning of allowed states and measurements in quantum mechanics, such that what is left appears to make Bell's argument fail, without altering the empirical predictions of quantum mechanics. I think however that it is a smoke screen, and the slogan "lost in math" comes to my mind. I will discuss some other recent disproofs of Bell's theorem using the language of causality based on causal graphs. Causal thinking is also central to law and justice. I will mention surprising connections to my work on serial killer nurse cases, in particular the Dutch case of Lucia de Berk and the current UK case of Lucy Letby.
Seminar of U.V. Spectroscopy by SAMIR PANDASAMIR PANDA
Spectroscopy is a branch of science dealing the study of interaction of electromagnetic radiation with matter.
Ultraviolet-visible spectroscopy refers to absorption spectroscopy or reflect spectroscopy in the UV-VIS spectral region.
Ultraviolet-visible spectroscopy is an analytical method that can measure the amount of light received by the analyte.
Nutraceutical market, scope and growth: Herbal drug technologyLokesh Patil
As consumer awareness of health and wellness rises, the nutraceutical market—which includes goods like functional meals, drinks, and dietary supplements that provide health advantages beyond basic nutrition—is growing significantly. As healthcare expenses rise, the population ages, and people want natural and preventative health solutions more and more, this industry is increasing quickly. Further driving market expansion are product formulation innovations and the use of cutting-edge technology for customized nutrition. With its worldwide reach, the nutraceutical industry is expected to keep growing and provide significant chances for research and investment in a number of categories, including vitamins, minerals, probiotics, and herbal supplements.
The increased availability of biomedical data, particularly in the public domain, offers the opportunity to better understand human health and to develop effective therapeutics for a wide range of unmet medical needs. However, data scientists remain stymied by the fact that data remain hard to find and to productively reuse because data and their metadata i) are wholly inaccessible, ii) are in non-standard or incompatible representations, iii) do not conform to community standards, and iv) have unclear or highly restricted terms and conditions that preclude legitimate reuse. These limitations require a rethink on data can be made machine and AI-ready - the key motivation behind the FAIR Guiding Principles. Concurrently, while recent efforts have explored the use of deep learning to fuse disparate data into predictive models for a wide range of biomedical applications, these models often fail even when the correct answer is already known, and fail to explain individual predictions in terms that data scientists can appreciate. These limitations suggest that new methods to produce practical artificial intelligence are still needed.
In this talk, I will discuss our work in (1) building an integrative knowledge infrastructure to prepare FAIR and "AI-ready" data and services along with (2) neurosymbolic AI methods to improve the quality of predictions and to generate plausible explanations. Attention is given to standards, platforms, and methods to wrangle knowledge into simple, but effective semantic and latent representations, and to make these available into standards-compliant and discoverable interfaces that can be used in model building, validation, and explanation. Our work, and those of others in the field, creates a baseline for building trustworthy and easy to deploy AI models in biomedicine.
Bio
Dr. Michel Dumontier is the Distinguished Professor of Data Science at Maastricht University, founder and executive director of the Institute of Data Science, and co-founder of the FAIR (Findable, Accessible, Interoperable and Reusable) data principles. His research explores socio-technological approaches for responsible discovery science, which includes collaborative multi-modal knowledge graphs, privacy-preserving distributed data mining, and AI methods for drug discovery and personalized medicine. His work is supported through the Dutch National Research Agenda, the Netherlands Organisation for Scientific Research, Horizon Europe, the European Open Science Cloud, the US National Institutes of Health, and a Marie-Curie Innovative Training Network. He is the editor-in-chief for the journal Data Science and is internationally recognized for his contributions in bioinformatics, biomedical informatics, and semantic technologies including ontologies and linked data.
4. Forms of energy
4
The INTERNAL ENERGY, E of a system is the sum of the kinetic and
potential energies of all the particles that compose the system or the total
energy of a system.
5. Definitions
5
System: A region of the universe that we direct our
attention to.
Surroundings: Everything outside a system is
called surroundings.
Boundary: The
boundary or wall
separates a system
from its surroundings.
9. Energy Transfer: Heat and
Work
9
Both work and heat together allow systems to exchange
energy
Heat is the transfer of thermal energy between two bodies that
are at different temperatures
Work is the force used to transfer energy between a system
and its surroundings, and is needed to create heat and the
transfer of thermal energy.
System
Heat (q)
Work (w)
Surroundings
11. Work =(Force)x(distance)
=Fd
Force=(Presssure)x(Area)
W=P(Ad)
=PV
PV work is also called expansion
work. There other types of work
that are not discussed here.
Work
12. 12
• Energy may enter the system as heat or work.
• The energy is stored as potential energy (PE) and kinetic energy
(KE).
• This energy can be withdrawn as work or heat from the system.
Energy Transfer: Heat and
Work
13. Zero law of thermodynamics
13
The Zero Law of Thermodynamics states that if two
systems are in thermodynamic equilibrium with a
third system, the two original systems are in thermal
equilibrium with each other.
System A
System C
System B
14. First law of thermodynamics
There Is No Free Lunch!!
14
Energy can not be created or destroyed only
transformed
ΔEuniv=ΔEsys+ΔEsurr=0
ΔEsys=−ΔEsurr
The First Law of Thermodynamics states that energy
can be converted from one form to another with the
interaction of heat, work and internal energy, but it
cannot be created nor destroyed, under any
circumstances.
ΔE=Q+W
15. 1st law of Thermodynamics is about
Conservation of Energy
15
As heat is applied to a closed system, the system
does work by increasing its volume.
w=PΔV
The sum of heat and work is the change in internal energy, ΔE.
In an isolated system, Q=−W. Therefore, ΔE=0.
16. Second law of thermodynamics
16
Second law of thermodynamics is about spontaneity
of processes.
Heat does not go from a colder body to a hotter
body.
flow of heat is always from a hotter body to a colder
body.
The entropy of the universe will increase during any
spontaneous change.
17. Entropy is the measure of disorder
Qtr ∝ T
ΔS ∝ Qtr
Entropy increases with softer, less rigid solids, solids
that contain larger atoms, and solids with complex
molecular structures.
Entropy
17
(Qtr)=The quantity of heat transferred
18. Entropy
18
The Second Law of Thermodynamics states that the
state of entropy of the entire universe, as a closed
isolated system, will always increase over time. The
second law also states that the changes in the
entropy in the universe can never be negative.
19. Free energy
19
ΔG=ΔH−TΔS
ΔH refers to the heat change for a reaction. A positive ΔH means that heat
is taken from the environment (endothermic). A negative ΔH means that
heat is emitted or given to the environment (exothermic).
ΔG is a measure for the change of a system's free energy.
20. 20
If ΔG < 0, the process occurs spontaneously.
If ΔG = 0, the system is at equilibrium.
If ΔG > 0, the process is not spontaneous as written
but occurs spontaneously in the reverse direction.
21. ΔG=ΔH−TΔS
21
Case ΔH ΔS ΔG Reaction
1. high temperature - + - Spontaneous
2. low temperature - + - Spontaneous
3. high temperature - - + Nonspontaneous
4. low temperature - - - Spontaneous
5. high temperature + + - Spontaneous
6. low temperature + + + Nonspontaneous
7. high temperature + - + Nonspontaneous
8. low temperature + - + Nonspontaneous
22. Example:
22
O2 2 O
occurs spontaneously under what temperature
conditions?
Answer:
By simply viewing the reaction one can determine that the
reaction increases in the number of moles, so the entropy
increases.
The enthalpy is positive, because covalent bonds are
broken. When covalent bonds are broken energy is
absorbed, which means that the enthalpy of the reaction is
positive. So, if the temperature is low it is probable
that ΔH is more than T∗ΔS, which means the reaction is not
spontaneous. If the temperature is large then T∗ΔS will be
larger than the enthalpy, which means the reaction is
23. 23
For more examples related to second law of
thermodynamics refer to the appendix sheet file named
ThermoEg(1) at:
bit.ly/physicalpharmacy
24. 3rd Law of Thermodynamics
24
It says that however it is impossible to reach absolute
zero, but at which (0 Kelvin), there will be no entropy
(S) and a pure crystalline structure of matter will form.