1) The document discusses the kinetic molecular theory and gas laws, which describe the behavior of ideal gases.
2) It explains that ideal gases are made of small, hard spheres that move rapidly in random motion and exert pressure through collisions with container walls.
3) The gas laws described are Boyle's law (inverse relationship between pressure and volume at constant temperature), Charles's law (direct relationship between volume and temperature at constant pressure), and Gay-Lussac's law (direct relationship between pressure and temperature at constant volume).
Properties of gases: gas laws, ideal gas equation, dalton’s law of partial pressure, diffusion of gases, kinetic theory of gases, mean free path, deviation from ideal gas behavior, vander wails equation, critical constants, liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity
I made this presentation for my own college assignment and i had referred contents from websites and other presentations and made it presentable and reasonable hope you will like it!!!
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Presents the gas laws and the factors upon which they are based. Includes Boyles', Charles', Gay Lussac's, Avogadro's and Dalton's Laws as well as the Combined Gas Law and the Universal Gas Law.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Properties of gases: gas laws, ideal gas equation, dalton’s law of partial pressure, diffusion of gases, kinetic theory of gases, mean free path, deviation from ideal gas behavior, vander wails equation, critical constants, liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity
I made this presentation for my own college assignment and i had referred contents from websites and other presentations and made it presentable and reasonable hope you will like it!!!
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Presents the gas laws and the factors upon which they are based. Includes Boyles', Charles', Gay Lussac's, Avogadro's and Dalton's Laws as well as the Combined Gas Law and the Universal Gas Law.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Kinetic Gas Theory including Ideal Gas Equation. Temperature, Volume, Applications
Boyle's Law, Charles' Law and Avogadro's Law. Ideal Gas Theory, Dalton's Partial Pressure
2 main factors determine state:
The forces (inter/intramolecular) holding particles together
The kinetic energy present (the energy an object possesses due to its motion of the particles)
KE tends to ‘pull’ particles apart
Ethanol (CH3CH2OH), or beverage alcohol, is a two-carbon alcohol
that is rapidly distributed in the body and brain. Ethanol alters many
neurochemical systems and has rewarding and addictive properties. It
is the oldest recreational drug and likely contributes to more morbidity,
mortality, and public health costs than all illicit drugs combined. The
5th edition of the Diagnostic and Statistical Manual of Mental Disorders
(DSM-5) integrates alcohol abuse and alcohol dependence into a single
disorder called alcohol use disorder (AUD), with mild, moderate,
and severe subclassifications (American Psychiatric Association, 2013).
In the DSM-5, all types of substance abuse and dependence have been
combined into a single substance use disorder (SUD) on a continuum
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comorbidities, fetal alcohol spectrum disorders, genetic risk factors, and
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micro teaching on communication m.sc nursing.pdfAnurag Sharma
Microteaching is a unique model of practice teaching. It is a viable instrument for the. desired change in the teaching behavior or the behavior potential which, in specified types of real. classroom situations, tends to facilitate the achievement of specified types of objectives.
Basavarajeeyam is an important text for ayurvedic physician belonging to andhra pradehs. It is a popular compendium in various parts of our country as well as in andhra pradesh. The content of the text was presented in sanskrit and telugu language (Bilingual). One of the most famous book in ayurvedic pharmaceutics and therapeutics. This book contains 25 chapters called as prakaranas. Many rasaoushadis were explained, pioneer of dhatu druti, nadi pareeksha, mutra pareeksha etc. Belongs to the period of 15-16 century. New diseases like upadamsha, phiranga rogas are explained.
Explore natural remedies for syphilis treatment in Singapore. Discover alternative therapies, herbal remedies, and lifestyle changes that may complement conventional treatments. Learn about holistic approaches to managing syphilis symptoms and supporting overall health.
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Tom Selleck Health: A Comprehensive Look at the Iconic Actor’s Wellness Journeygreendigital
Tom Selleck, an enduring figure in Hollywood. has captivated audiences for decades with his rugged charm, iconic moustache. and memorable roles in television and film. From his breakout role as Thomas Magnum in Magnum P.I. to his current portrayal of Frank Reagan in Blue Bloods. Selleck's career has spanned over 50 years. But beyond his professional achievements. fans have often been curious about Tom Selleck Health. especially as he has aged in the public eye.
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Introduction
Many have been interested in Tom Selleck health. not only because of his enduring presence on screen but also because of the challenges. and lifestyle choices he has faced and made over the years. This article delves into the various aspects of Tom Selleck health. exploring his fitness regimen, diet, mental health. and the challenges he has encountered as he ages. We'll look at how he maintains his well-being. the health issues he has faced, and his approach to ageing .
Early Life and Career
Childhood and Athletic Beginnings
Tom Selleck was born on January 29, 1945, in Detroit, Michigan, and grew up in Sherman Oaks, California. From an early age, he was involved in sports, particularly basketball. which played a significant role in his physical development. His athletic pursuits continued into college. where he attended the University of Southern California (USC) on a basketball scholarship. This early involvement in sports laid a strong foundation for his physical health and disciplined lifestyle.
Transition to Acting
Selleck's transition from an athlete to an actor came with its physical demands. His first significant role in "Magnum P.I." required him to perform various stunts and maintain a fit appearance. This role, which he played from 1980 to 1988. necessitated a rigorous fitness routine to meet the show's demands. setting the stage for his long-term commitment to health and wellness.
Fitness Regimen
Workout Routine
Tom Selleck health and fitness regimen has evolved. adapting to his changing roles and age. During his "Magnum, P.I." days. Selleck's workouts were intense and focused on building and maintaining muscle mass. His routine included weightlifting, cardiovascular exercises. and specific training for the stunts he performed on the show.
Selleck adjusted his fitness routine as he aged to suit his body's needs. Today, his workouts focus on maintaining flexibility, strength, and cardiovascular health. He incorporates low-impact exercises such as swimming, walking, and light weightlifting. This balanced approach helps him stay fit without putting undue strain on his joints and muscles.
Importance of Flexibility and Mobility
In recent years, Selleck has emphasized the importance of flexibility and mobility in his fitness regimen. Understanding the natural decline in muscle mass and joint flexibility with age. he includes stretching and yoga in his routine. These practices help prevent injuries, improve posture, and maintain mobilit
Title: Sense of Smell
Presenter: Dr. Faiza, Assistant Professor of Physiology
Qualifications:
MBBS (Best Graduate, AIMC Lahore)
FCPS Physiology
ICMT, CHPE, DHPE (STMU)
MPH (GC University, Faisalabad)
MBA (Virtual University of Pakistan)
Learning Objectives:
Describe the primary categories of smells and the concept of odor blindness.
Explain the structure and location of the olfactory membrane and mucosa, including the types and roles of cells involved in olfaction.
Describe the pathway and mechanisms of olfactory signal transmission from the olfactory receptors to the brain.
Illustrate the biochemical cascade triggered by odorant binding to olfactory receptors, including the role of G-proteins and second messengers in generating an action potential.
Identify different types of olfactory disorders such as anosmia, hyposmia, hyperosmia, and dysosmia, including their potential causes.
Key Topics:
Olfactory Genes:
3% of the human genome accounts for olfactory genes.
400 genes for odorant receptors.
Olfactory Membrane:
Located in the superior part of the nasal cavity.
Medially: Folds downward along the superior septum.
Laterally: Folds over the superior turbinate and upper surface of the middle turbinate.
Total surface area: 5-10 square centimeters.
Olfactory Mucosa:
Olfactory Cells: Bipolar nerve cells derived from the CNS (100 million), with 4-25 olfactory cilia per cell.
Sustentacular Cells: Produce mucus and maintain ionic and molecular environment.
Basal Cells: Replace worn-out olfactory cells with an average lifespan of 1-2 months.
Bowman’s Gland: Secretes mucus.
Stimulation of Olfactory Cells:
Odorant dissolves in mucus and attaches to receptors on olfactory cilia.
Involves a cascade effect through G-proteins and second messengers, leading to depolarization and action potential generation in the olfactory nerve.
Quality of a Good Odorant:
Small (3-20 Carbon atoms), volatile, water-soluble, and lipid-soluble.
Facilitated by odorant-binding proteins in mucus.
Membrane Potential and Action Potential:
Resting membrane potential: -55mV.
Action potential frequency in the olfactory nerve increases with odorant strength.
Adaptation Towards the Sense of Smell:
Rapid adaptation within the first second, with further slow adaptation.
Psychological adaptation greater than receptor adaptation, involving feedback inhibition from the central nervous system.
Primary Sensations of Smell:
Camphoraceous, Musky, Floral, Pepperminty, Ethereal, Pungent, Putrid.
Odor Detection Threshold:
Examples: Hydrogen sulfide (0.0005 ppm), Methyl-mercaptan (0.002 ppm).
Some toxic substances are odorless at lethal concentrations.
Characteristics of Smell:
Odor blindness for single substances due to lack of appropriate receptor protein.
Behavioral and emotional influences of smell.
Transmission of Olfactory Signals:
From olfactory cells to glomeruli in the olfactory bulb, involving lateral inhibition.
Primitive, less old, and new olfactory systems with different path
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Gases
1. Gases
By Dr Zahid khan
Senior Lecturer king faisal university,
Kingdom of Saudi Arabia.
2. Kinetic-Molecular Theory
• KMT – based on idea that particles of matter are always in motion.
• The kinetic theory of gases makes several basic assumptions.
• It assumes that gases consist of hard, spherical particles, usually
atoms or molecules, that have the following properties.
• First, the gas particles are so small in relation to the distances
between them that their individual volumes can be assumed to be
insignificant.
• The large relative distances between the particles means that there is
considerable empty space between the particles.
2
3. This assumption that gas particles are far apart explains
the important property of gas compressibility: A gas is
easily compressed because of the space between the
particles.
The second property of gas particles assumed by the
kinetic theory is that no attractive or repulsive forces
exist between the particles.
As a result, gases are free to move inside their
containers. In fact, a gas expands until it takes the
shape and volume of its container.
4. The third assumption is that gas particles move
rapidly in constant random motion.
The particles travel in straight paths and move
independently of each other.
Only when a particle collides with another
particle or object does theory assumes further
that these collisions between gas particles are
perfectly elastic, which means that during a
collision the total amount of kinetic energy
remains constant and that the kinetic energy is
transferred without loss from one particle to
another.
5. Four variables are generally used to describe a gas. The variables
and their common units are pressure (P) in kilopascals, volume (V)
in liters, temperature (T) in kelvins, and number of moles (n).
The gas laws will enable you to predict gas behavior at specific
conditions. Understanding the gas laws will help you understand
everyday applications of gases in automobile airbags, scuba-diving
equipment, and hot-air balloons, among many others.
6. Amount of Gas
Using the kinetic theory, you can predict and explain how gases
will respond to a change of conditions, specifically the pressure.
When you pump up a tire, you should expect the pressure inside
it to increase. Collisions of gas particles with the inside walls of
the tire result in the pressure that is exerted by the enclosed gas.
By adding gas, you increase the number of gas particles, thus
increasing the number of collisions, which explains why the gas
pressure increases.
7. As long as gas temperature does not change,
doubling the number of gas particles doubles
the pressure. Tripling the number of gas
particles triples the pressure, and so forth.
Once the pressure exceeds the strength of the
container, however, the container will rupture.
8. In a similar way, letting the air out of a tire decreases the pressure
inside the tire. The fewer particles inside exert less pressure.
When a sealed container of gas under pressure is opened, gas inside
moves from the region of higher pressure to the region of lower
pressure outside. This is the principle used in aerosol cans.
9. There are other ways to increase gas pressure.
You can raise the pressure exerted by a contained gas by reducing its
volume. The more the gas is compressed, the greater is the pressure it
exerts inside the container. Reducing the volume of a contained gas by half
doubles the pressure.
Doubling the volume of the container will halve the gas pressure because
the same number of gas particles occupy a volume twice the original size.
10. Raising the temperature of an enclosed gas provides yet another way to
increase gas pressure.
If the average kinetic energy of a gas doubles, the Kelvin temperature doubles
and the pressure of the enclosed gas also doubles.
By contrast, as the temperature of an enclosed gas decreases, the particles
move more slowly and have less kinetic energy. They strike the container
walls with less force. Halving the Kelvin temperature of a gas in a rigid
container decreases the gas pressure by half.
11. Boyle,s Law
When the pressure goes up, the volume goes down.
Similarly, when the pressure goes down, the volume goes
up.
Boyle’s law states that for a given mass of gas at constant
temperature, the volume of the gas varies inversely with
pressure. In an inverse relationship, the product of the two
variables quantities is constant.
P1 x V1 = P 2 x V2
if T is constant.
12. Charle,s Law
Charles’s law summarizes Charles’s observations and the findings of Kelvin.
Charles’s law states that the volume of a fixed mass of gas is directly proportional to
it Kelvin temperature if the pressure is kept constant.
The ratio of volume to Kelvin temperature for a gas sample at any two set of
conditions is constant. Thus you can write Charles’s law as follows:
V1
T1
=
V2
T2
13. William Thompson (Lord Kelvin) realized the significance of this
temperature value.
He identified -273.15°C as absolute zero, the lowest possible
temperature. On the Kelvin temperature scale, 0 K corresponds to
-273.15°C.
14. Gay-Lussac’s law
Gay-Lussac’s law states that the pressure of a gas is directly proportional to the
Kelvin temperature if the volume remains constant.
On a hot summer day, the pressure in a car tire increases. This increase
illustrates a relationship that was discovered in 1802 by Joseph Gay-Lussac
(1778-1850), a French chemist.
Therefore assuming that the volume remains constant, you can write GayLussac’s law as follows:
P1
T1
=
P2
T2
15. Real vs. Ideal Gases
An ideal gas is one that follows all of the assumptions of the kinetic theory. Its particles
could have no volume, and there could be no attraction between particles in the gas.
Unfortunately, there is no gas where this holds true.
At many conditions of temperature and pressure, however, real gases do behave like
ideal gases.
In a real gas the particles do have volume, and there are attractions between the
particles. Because of these attractions, gases can condense, or even solidify, when it is
compressed and cooled.
16. Suppose you want to calculate the number of moles (n) of a gas in a fixed volume at a
known temperature and pressure. The calculation of moles is possible by modifying
the combined gas law.
The number of moles of gas is directly proportional to the number of particles.
Hence, moles must be directly proportional to volume as well.
Therefore, you can introduce moles in to the combined gas law by dividing
each side of the equation by n.
P1 x V1
T 1 x n1
=
P2 x V2
T 2 x n2
This equation shows that (P x V)/(T x n) is a constant. This constancy holds for what are
called ideal gases. A gas behaves ideally if it conforms to the gas laws.
17. If you could evaluate the constant (P x V)/(T x n), you could then calculate the
number of moles of gas at any specified value of P, V, and T. This constant is
symbolized as R.
You can find the actual value of R, given an important fact about gases: 1 mol of
every gas occupies 22.4 L at STP. Inserting the values of P, V, T, and n into the
equation:
R=
PxV
Txn
=
101.3 kPa x 22.4 L
= 8.31 L x kPa/K x mol
273 K x 1 mol
The ideal gas constant (R) has the value 8.31 L x kPa/K x mol. Rearranging
the equation for R, you obtain the usual form of the ideal gas law:
18. P x V = n x R x T; or, PV = nRT
An advantage of the ideal gas law over the combined gas law is that it
permits you to solve for the number of moles of a combined gas when P, V,
and T are known.
P is the pressure
V is the volume
n is the amount of gas (moles)
R is the Real Gas constant, with units appropriate for the units of pressure,
volume, temperature, and amount of gas.
T is the temperature (in Kelvin because an absolute scale is necessary.)