This document discusses colligative properties, which are physical properties of solutions that depend only on the ratio of solute to solvent particles and not the identity of the solute. It describes four colligative properties: boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure. It explains how adding a nonvolatile solute affects the phase diagram by shifting the freezing point downward and boiling point upward. Formulas are provided to calculate changes in boiling point and freezing point based on molality. Raoult's Law is introduced to explain how vapor pressure of a solution depends on the mole fraction of the solvent. Osmotic pressure is defined as the pressure required to prevent solvent flow across a semiperme
Definite Volume
Not Definite Shape
Molecules Are Much Closer Than Gases
Intermolecular Forces In Between Solids And Gases
properties of liquids
Evaporation
Process Of Changing A Liquid Into A Gas Phase
For example, liquid water conversion into vapor form
Cooling Process
Definite Volume
Not Definite Shape
Molecules Are Much Closer Than Gases
Intermolecular Forces In Between Solids And Gases
properties of liquids
Evaporation
Process Of Changing A Liquid Into A Gas Phase
For example, liquid water conversion into vapor form
Cooling Process
RAOULT'S LAW ( Physical & Analytical Chemistry)Hasnaın Sheıkh
Name; Hasnain Nawaz
Surname : Shaikh
ROLL NO: 16 CH 42
B.E: Chemical Engineering (In Progress).
Mehran University of Engineering and Technology
Jamshore, ISO 9001 Certified.
Colligative properties of dilute solutions Manik Imran Nur Manik
lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
a solution is a homogeneous mixture composed of two or more substances. In such a mixture, a solute is a substance dissolved in another substance, known as a solvent.
Colligative properties of dilute solutions: lowering of vapour pressure, elevation of
boiling point, depression of freezing point and osmotic pressure including necessary
thermodynamic derivations.
T. Y. B. Sc. Unit II, Chemical Thermodynamics.pptxKusumBaser1
This power point is based on the syllabus of TYBSc SEM V, unit 2, Paper 1, Mumbai university. This covers colligative properties, relative lowering of vapour pressure, elevation in boiling point, depressure in freezing point, Osmotic pressure, Chemical kinetics, various methods to find out these colligative properties, reverse osmosis, vant hoff factor, some numerical.
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.
Professional air quality monitoring systems provide immediate, on-site data for analysis, compliance, and decision-making.
Monitor common gases, weather parameters, particulates.
This pdf is about the Schizophrenia.
For more details visit on YouTube; @SELF-EXPLANATORY;
https://www.youtube.com/channel/UCAiarMZDNhe1A3Rnpr_WkzA/videos
Thanks...!
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.
Observation of Io’s Resurfacing via Plume Deposition Using Ground-based Adapt...Sérgio Sacani
Since volcanic activity was first discovered on Io from Voyager images in 1979, changes
on Io’s surface have been monitored from both spacecraft and ground-based telescopes.
Here, we present the highest spatial resolution images of Io ever obtained from a groundbased telescope. These images, acquired by the SHARK-VIS instrument on the Large
Binocular Telescope, show evidence of a major resurfacing event on Io’s trailing hemisphere. When compared to the most recent spacecraft images, the SHARK-VIS images
show that a plume deposit from a powerful eruption at Pillan Patera has covered part
of the long-lived Pele plume deposit. Although this type of resurfacing event may be common on Io, few have been detected due to the rarity of spacecraft visits and the previously low spatial resolution available from Earth-based telescopes. The SHARK-VIS instrument ushers in a new era of high resolution imaging of Io’s surface using adaptive
optics at visible wavelengths.
Cancer cell metabolism: special Reference to Lactate PathwayAADYARAJPANDEY1
Normal Cell Metabolism:
Cellular respiration describes the series of steps that cells use to break down sugar and other chemicals to get the energy we need to function.
Energy is stored in the bonds of glucose and when glucose is broken down, much of that energy is released.
Cell utilize energy in the form of ATP.
The first step of respiration is called glycolysis. In a series of steps, glycolysis breaks glucose into two smaller molecules - a chemical called pyruvate. A small amount of ATP is formed during this process.
Most healthy cells continue the breakdown in a second process, called the Kreb's cycle. The Kreb's cycle allows cells to “burn” the pyruvates made in glycolysis to get more ATP.
The last step in the breakdown of glucose is called oxidative phosphorylation (Ox-Phos).
It takes place in specialized cell structures called mitochondria. This process produces a large amount of ATP. Importantly, cells need oxygen to complete oxidative phosphorylation.
If a cell completes only glycolysis, only 2 molecules of ATP are made per glucose. However, if the cell completes the entire respiration process (glycolysis - Kreb's - oxidative phosphorylation), about 36 molecules of ATP are created, giving it much more energy to use.
IN CANCER CELL:
Unlike healthy cells that "burn" the entire molecule of sugar to capture a large amount of energy as ATP, cancer cells are wasteful.
Cancer cells only partially break down sugar molecules. They overuse the first step of respiration, glycolysis. They frequently do not complete the second step, oxidative phosphorylation.
This results in only 2 molecules of ATP per each glucose molecule instead of the 36 or so ATPs healthy cells gain. As a result, cancer cells need to use a lot more sugar molecules to get enough energy to survive.
Unlike healthy cells that "burn" the entire molecule of sugar to capture a large amount of energy as ATP, cancer cells are wasteful.
Cancer cells only partially break down sugar molecules. They overuse the first step of respiration, glycolysis. They frequently do not complete the second step, oxidative phosphorylation.
This results in only 2 molecules of ATP per each glucose molecule instead of the 36 or so ATPs healthy cells gain. As a result, cancer cells need to use a lot more sugar molecules to get enough energy to survive.
introduction to WARBERG PHENOMENA:
WARBURG EFFECT Usually, cancer cells are highly glycolytic (glucose addiction) and take up more glucose than do normal cells from outside.
Otto Heinrich Warburg (; 8 October 1883 – 1 August 1970) In 1931 was awarded the Nobel Prize in Physiology for his "discovery of the nature and mode of action of the respiratory enzyme.
WARNBURG EFFECT : cancer cells under aerobic (well-oxygenated) conditions to metabolize glucose to lactate (aerobic glycolysis) is known as the Warburg effect. Warburg made the observation that tumor slices consume glucose and secrete lactate at a higher rate than normal tissues.
The ASGCT Annual Meeting was packed with exciting progress in the field advan...
Colligative Properties III
1. Colligative Properties
Pt. 3
By Shawn P. Shields, Ph.D.
This work is licensed by Shawn P. Shields-Maxwell under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0
International License.
2. Colligative Properties
A physical property of a solution that
depends only on the ratio of the number
of particles of solute to solvent in the
solution, not the identity of the solute.
Describes a nonvolatile solute dissolved
in a solvent.
3. Four Colligative Properties
Boiling point elevation
Freezing point depression
Vapor pressure lowering
Osmotic pressure
How can we explain these?
5. Effect of Colligative Properties on the Phase Diagram
T (C)
P
(atm)
1 atm
Dotted lines
indicate the new
phase boundaries
for the solution.
The solid-liquid
coexistence line is
now shifted to
lower temperatures.
The liquid-vapor line
shifts to higher
temperatures.
6. Effect of Colligative Properties on the Phase Diagram
T (C)
P
(atm)
1 atm
new mp
X
new bp
X
Boiling point
elevation
Melting point
depression
Vapor pressure
lowering (come
back to this)
7. Boiling Point Elevation
Recall: The boiling point of a substance is the
temperature where the vapor pressure equals the
external (usually atmospheric) pressure.
The external pressure doesn’t change, but the
temperature required to attain that vapor pressure is
increased!
Tb = kbm
Tb is the increase in boiling
temperature
kbis the molal boiling point elevation
constant (look it up for a given
solvent)
m is the molality of the solute
molality =
moles solute
kg of solvent
8. Freezing Point Depression
When the freezing point is depressed, this means the
temperature must be lower before a given substance
freezes.
Tf = kfm
Tf is the decrease in freezing
temperature
kfis the molal freezing point
depression constant (look it up
for a given solvent)
m is the molality of the solute
molality (m) =
moles solute
kg of solvent
9. Calculating Solvent Mass
Use the volume of the solvent and its density to
find the mass of solvent for molality (m).
𝐦𝐨𝐥𝐚𝐥𝐢𝐭𝐲 (𝐦) =
𝐦𝐨𝐥𝐞𝐬 𝐬𝐨𝐥𝐮𝐭𝐞
𝐤𝐠 𝐨𝐟 𝐬𝐨𝐥𝐯𝐞𝐧𝐭
𝐝𝐞𝐧𝐬𝐢𝐭𝐲
𝐠
𝐦𝐋
=
𝐦𝐚𝐬𝐬
𝐯𝐨𝐥𝐮𝐦𝐞
10. Recall: Equilibrium Vapor Pressure
Molecules in the liquid phase
continuously vaporize and condense
in a closed container.
rate of evaporation = rate of condensation
The partial pressure of the gas is constant
at equilibrium.
Liquid molecule
11. Vapor Pressure Lowering
The vapor
pressure of the
solution is
lower than the
pure solvent.
T (C)
P
(atm)
1 atm
Normal bp of
pure solvent
VP at bp of
pure solvent
X VP of solution
12. Raoult’s Law
The vapor pressure of the solution depends on the
mole fraction of the solvent.
Psoln = χsolventPsolvent
ο
Psoln is the vapor pressure of the solution
is the mole fraction of the solvent
Psolvent
ο
is the vapor pressure of the pure solvent
13. Raoult’s Law
The vapor pressure of the solution
depends on the mole fraction of
the solvent.
χ 𝐬𝐨𝐥𝐯𝐞𝐧𝐭 =
moles 𝐬𝐨𝐥𝐯𝐞𝐧𝐭
moles solute + moles solvent
Liquid molecule
Nonvolatile solute
14. Osmosis
The two regions are
separated by a
semipermeable membrane
that allows solvent to pass,
but not solute particles.
Osmosis By OpenStax College [CC BY 3.0
(http://creativecommons.org/licenses/by/3.0)], via Wikimedia Commons
The net movement of solvent molecules from a
region of lower solute concentration to one with a
higher concentration.
15. Osmotic Pressure ()
Osmotic pressure is the amount of pressure required to
stop the flow of solvent.
A similar equation to the Ideal Gas law can be written for
the osmotic pressure:
Π V = nRT
Where is the osmotic pressure (in the same units as
the gas constant, R)
V is the volume in L, n is moles of solute, and
T is temperature in K
16. Osmotic Pressure ()
We can rearrange this equation to a more
useful form
Π V = nRT
Π =
n
V
RT = CRT
Where C is the concentration (M, molarity)