This document provides an overview of key concepts related to gases, including:
- The properties of ideal gases and units of pressure like pascals and atmospheres.
- Gas laws including Boyle's, Charles', Gay-Lussac's, Avogadro's, and the ideal gas law.
- Conditions of STP and using gas laws to perform stoichiometric calculations.
- The kinetic molecular theory which explains gas properties in terms of particle motion.
- How real gases differ from ideal gases due to intermolecular forces.
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
Includes the principles of the KMT and their application to molecular behavior.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
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.
Organic chemistry involves the study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds, which include not only hydrocarbons but also compounds with any number of other elements, including hydrogen (most compounds contain at least one carbon–hydrogen bond), nitrogen, oxygen, halogens, phosphorus, silicon, and sulfur.
This branch of chemistry was originally limited to compounds produced by living organisms but has been broadened to include human-made substances such as plastics. The range of application of organic compounds is enormous and also includes, but is not limited to, pharmaceuticals, petrochemicals, food, explosives, paints, and cosmetics.
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
Includes the principles of the KMT and their application to molecular behavior.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
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.
Organic chemistry involves the study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds, which include not only hydrocarbons but also compounds with any number of other elements, including hydrogen (most compounds contain at least one carbon–hydrogen bond), nitrogen, oxygen, halogens, phosphorus, silicon, and sulfur.
This branch of chemistry was originally limited to compounds produced by living organisms but has been broadened to include human-made substances such as plastics. The range of application of organic compounds is enormous and also includes, but is not limited to, pharmaceuticals, petrochemicals, food, explosives, paints, and cosmetics.
A conceptual description of the van der Waals equation for real gases. Discussion of van der Waals constants a and b, plus conceptual example. Does not assume that intermolcular forces have been learned previously. General Chemistry
This showcases the basics of the laws governing behavior of gases which includes:
1. Boyle's Law
2. Charles's Law
3. Gay - Lussac's Law
4. Combined Gas Law
5. Avogadro's Law
6. Ideal Gas Law
7. Dalton's Law on Partial Pressures
8. Graham's Law of Diffusion
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
Palestine last event orientationfvgnh .pptxRaedMohamed3
An EFL lesson about the current events in Palestine. It is intended to be for intermediate students who wish to increase their listening skills through a short lesson in power point.
The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
Operation “Blue Star” is the only event in the history of Independent India where the state went into war with its own people. Even after about 40 years it is not clear if it was culmination of states anger over people of the region, a political game of power or start of dictatorial chapter in the democratic setup.
The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
The Indian economy is classified into different sectors to simplify the analysis and understanding of economic activities. For Class 10, it's essential to grasp the sectors of the Indian economy, understand their characteristics, and recognize their importance. This guide will provide detailed notes on the Sectors of the Indian Economy Class 10, using specific long-tail keywords to enhance comprehension.
For more information, visit-www.vavaclasses.com
2. Objectives
O Discuss the properties of gases (especially in terms
of SI units).
O Define and identify the gas laws.
O Perform calculations using the ideal gas law.
O Define conditions of STP (Standard Temperature and
Pressure).
O Apply the gas laws to stoichiometric calculations.
O Calculate the molar mass of a gas using laboratory
data and the ideal gas law.
O Explain the properties of ideal gases as defined by
the Kinetic Molecular Theory.
O Define effusion and diffusion.
O Explain how real gases differ from ideal gases.
3. Outline
I. Properties of Gases
A. Properties of Ideal Gases
B. SI Units of Pressure
1. Barometer
II> The Gas Laws
A. Relationships Between Properties
B. Boyle’s Law
C. Charles’ Law
D. Gay Lussac’s Law
E. Avogadro’s Law
F. Ideal Gas Law
G. The Combined Gas Law
H. Dalton’s Law of Partial Pressures
III. Gas Stoichiometry
IV. Kinetic Molecular Theory
A. Ideal Gases
B. Gas Diffusion and Effusion
V. Real Gases
A. Properties of Real Gases
B. Intermolecular Forces
C. Van der Waals Equation
D. Examples of Real Gases
4. An Introduction to Gases
O Remember from Unit 1 that gases:
O Take up the shape AND volume of a container.
O Are in constant, rapid, and random motion.
O Are easily compressed
O Exert force on their surroundings
Smoke Texture by Caleb CC-BY https://flic.kr/p/5RZseH
Gas – colliding particles w/o gravity force by numerical physics. http://youtu.be/iC3bfyP6Wuk Standard YouTube License
5. An Introduction to Gases
O Gases provide instant observations.
O Provide a way to evaluate real world
issues.
7. Units of Pressure
O SI Units: Pascal (Pa) contains units
𝑁𝑒𝑤𝑡𝑜𝑛
𝑀𝑒𝑡𝑒𝑟2
O More commonly used
O Atmosphere (atm)
O Millimeter Mercury (mmHg)
O Torr
101,325 𝑃𝑎 = 1 𝑎𝑡𝑚
1 𝑎𝑡𝑚 = 760 𝑚𝑚𝐻𝑔
1 𝑎𝑡𝑚 = 760 𝑡𝑜𝑟𝑟
8. Barometers
O Barometers are used to
measure atmospheric pressure
O Tube with a vacuum inverted in
a petri dish of Hg. Height of
Hg rises until the pressure from
atmosphere and Hg in tube are
equal.
O Height measured in mmHg.
"Prinzip Torricelli" by Volker Sperlich - Quelle: Volker Sperlich: "Übungsaufgaben zur Thermodynamik mit Mathcad" (2002)
Fachbuchverlag Leipzig. Licensed under CC BY-SA 2.0 de via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Prinzip_Torricelli.jpg#/media/File:Prinzip_Torricelli.jpg
9. Other Pressure Gauges
O Same concept used on
O Tire gauges
O Blood pressure cuffs
O Etc.
"Tire pressure gauge" by (U.S. Air Force photo by Airman Frank Snider) - USAF photo archive. Licensed under Public Domain via
Wikimedia Commons - http://commons.wikimedia.org/wiki/File:Tire_pressure_gauge.jpg#/media/File:Tire_pressure_gauge.jpg
"Sphygmomanometer" by Original uploader was ML5 at en.wikipedia - Transferred from en.wikipedia; transferred to Commons by
10. Concept Check
O The local weather station reports the
pressure as 30.59 inHg. Convert to
mmHg, torr and atm.
777.0 mmHg
1.022 atm
11. The Gas Laws
O Gas behavior allows us to observe:
O What happens in a situation.
O We want to convert that to WHY
something happens.
O Scientists developed the gas laws.
12. The Gas Laws
O Relate the properties of gases to one
another.
O Boyle’s Law
O Charles’ Law
O Gay Lussac’s Law
O Avogadro’s Law
O Ideal Gas Law
O Combined Gas Law
O Dalton’s Law of Partial Pressures.
13. Boyle’s Law
O Pressure is inversely proportional to
volume (if temperature and mol are held
constant).
𝑃1 𝑉1 = 𝑃2 𝑉2
O Graph of P vs
1
𝑉
will give a
straight line.
"Boyles Law animated" by NASA's Glenn Research Center - http://www.grc.nasa.gov/WWW/K-12/airplane/aboyle.html. Licensed
under Public Domain via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Boyles_Law_animated.gif#/media/File:Boyles_Law_animated.gif
14. Boyle’s Law
Boyle’s Law Demonstrations. NCSSMDistanceEd. 2011. CC-BY https://youtu.be/N5xft2fIqQU
15. Concept Check
O A balloon occupies 5.4 L and has a
pressure of 1.04 atm. If the pressure
drops to 0.856 atm, what will the new
volume be? Assume temperature and mol
are held constant.
6.12 L
16. Concept Check
O A gas inside a balloon occupies 325 mL
and exerts a pressure of 4.56 atm. If the
pressure drops to 2.26 atm, what will the
new volume be? (Assume temperature
and mol are held constant.)
655 mL
17. Charles’ Law
O Temperature (in Kelvin) is directly proportional
to volume (if pressure and mol are held
constant).
𝑇1
𝑉1
=
𝑇2
𝑉2
O Graph of T (K) vs V will give a
straight line.
"Charles and Gay-Lussac's Law animated" by NASA's Glenn Research Center - http://www.grc.nasa.gov/WWW/K-
12/airplane/aglussac.html. Licensed under Public Domain via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Charles_and_Gay-Lussac%27s_Law_animated.gif#/media/File:Charles_and_Gay-
Lussac%27s_Law_animated.gif
18. Charles’ Law
55 Gallon steel drum can crush. Thechemman. 2010. Standard YouTube License. https://youtu.be/JsoE4F2Pb20
Gharles’ Law Demonstartion. Fostythesnowman. 2012. Standard YouTube License. https://youtu.be/GcCmalmLTiU
19. Concept Check
O A balloon occupies 15.4 L at 25◦C. What
volume would the gas occupy at 35◦C.
Assume pressure and mol are held
constant.
16 L
20. Gay-Lussac’s Law
O Temperature (in Kelvin) is directly related to
pressure (if volume and mol are held
constant).
𝑃1
𝑇1
=
𝑃2
𝑇2
O Graph of P vs T will give a
straight line.
"Temperature Pressure law" by Evan Mason - Own work. Licensed under CC BY-SA 3.0 via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Temperature_Pressure_law.svg#/media/File:Temperature_Pressure_law.svg
22. Concept Check
O A gas in a closed container (fixed volume
and mol) exerts a pressure of 8.64 atm at
50 ◦C. What would the temperature be (in
◦C) if the pressure was suddenly raised to
17.2 atm?
370 ◦C
23. Avogadro’s Law
O Volume is directly proportional to mol (if
pressure and temperature are held
constant).
O Graph of n vs V will give a
straight line.
𝑛1
𝑉1
=
𝑛2
𝑉2
24. Concept Check
O 4.15 mol of He occupy a 75 L balloon.
What volume will 3.75 mol occupy (at the
same temperature and pressure.
68 L
25. Ideal Gas Law
O We can combine the gas laws into one
equation:
𝑃𝑉 = 𝑛𝑅𝑇
P = pressure (atm)
V = volume (L)
n = amount (mol)
R = Constant 0.08206
𝐿 𝑎𝑡𝑚
𝑚𝑜𝑙 𝐾
T = temperature (K)
26. Concept Check
O What volume will a 82.6 g sample of N2
exerting 7.25 atm at 62.1 °C fill?
11.19 L
27. Combined Gas Law
O Ideal Gas law can be rearranged to give
O R and n are left out because they cancel.
28. Concept Check
O A sample of He at 37 °C exerts 15.1 atm
in a 2425 mL container. If the temperature
suddenly cools to 20.1 °C and the volume
adjusts to 1815 mL, what will the new
pressure be?
19.1 L
29. Dalton’s Law of Partial
Pressures
O The pressure of a mixture of gases is
equal to the partial pressure of all the
individual components.
O A gas exerts the same pressure whether
alone or in a mixture.
“"Dalton's law of partial pressures" by Max Dodge - Own work. Licensed under CC BY-SA 4.0 via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Dalton%27s_law_of_partial_pressures.png#/media/File:Dalton%27s_law_of_partial_pressure
s.png
30. Real World Application
O Scuba divers use various mixtures of
gases depending on the depth of their
dive.
O Mixtures may be Nitrox, Trimix, Oxygne or
Heliox
O For very deep dives, they use a mixture
called Heliox which contains He and O2.
31. Concept Check
O 22.1 L of oxygen gas originally at 25°C and 1.75 atm
and 9.20 L of He gas originally at 25 °C and 17.84 atm
are pumped into a single scuba tank with a volume of
10.0 L.
O Calculate the partial pressure oxygen:
O Calculate the partial pressure of helium:
O Calculate the pressure in the scuba tank. 3.87 atm Oxygen
16.41 atm He
20.28 atm total
36. Concept Check
O At STP, a balloon containing 4.92 mol of
gas has a volume of 15.1 L. If the balloon
has a leak and eventually contained only
3.14 mol, what volume would the balloon
occupy?
9.64 L
37. Molar Mass of a Gas
O Can use the ideal gas law to solve for n
(mol)
O If you also know the mass of the gas, can
solve for molar mass.
38. Concept Check
O A laboratory group measures an excess of a
volatile liquid. They add this to an empty flask
with a volume of 257.6 mL. They heat the
sample to 76.8 degrees C until all the liquid is
vaporized. The pressure in the lab is 0.924
atm. How many mol of gas are present?
O If the volatile liquid had a mass of 0.142 g,
what was the molar mass of the unknown
liquid?
8.29 x 10-3 mol
17.1 g/mol
39. Kinetic Molecular Theory
O Explains the properties of gases and why
the gas laws are accurate.
O Contains 4 postulates.
"Translational motion" by Greg L at the English language Wikipedia. Licensed under CC BY-SA 3.0 via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Translational_motion.gif#/media/File:Translational_motion.gif
40. Kinetic Molecular Theory
O 1. The volume of gas particles is
negligible compared to the volume which
they occupy.
42. Kinetic Molecular Theory
O 3. Gas particles have no (attractive or
repulsive) intermolecular interactions.
O All collisions between gas particles are
elastic so that all kinetic energy is
conserved during collisions.
43. Kinetic Molecular Theory
O 4. The kinetic energy of a gas is directly
proportional to the K temperature.
44. Concept Check
Kristin_ A . Mergingue Bakeshop. Bit Balloons. 2012. https://flic.kr/p/bzbZkW
O Using the Kinetic
Molecular Theory,
consider two
balloons…
45. Concept Check
Kristin_ A . Mergingue Bakeshop. Bit Balloons. 2012. https://flic.kr/p/bzbZkW
O If you had two balloons
of exactly the same
volume. One contains
H2, the other Ne…
O Do the balloons have
the same or different
pressure?
46. Concept Check
Kristin_ A . Mergingue Bakeshop. Bit Balloons. 2012. https://flic.kr/p/bzbZkW
O If you had two balloons
of exactly the same
volume. One contains
H2, the other Ne…
O Do the balloons have
the same or different
temperature?
47. Concept Check
Kristin_ A . Mergingue Bakeshop. Bit Balloons. 2012. https://flic.kr/p/bzbZkW
O If you had two balloons
of exactly the same
volume. One contains
H2, the other Ne…
O Do the balloons have
the same or different
mol?
48. Concept Check
Kristin_ A . Mergingue Bakeshop. Bit Balloons. 2012. https://flic.kr/p/bzbZkW
O If you had two balloons
of exactly the same
volume. One contains
H2, the other Ne…
O Do the balloons have
the same or different
grams?
49. Gas Diffusion and Effusion
O Diffusion:
O The movement of particles from an area of
high concentration to an area of low
concentration… spreading out until the
concentration is consistent throughout.
"Diffusion" by JrPol - Own work. Licensed under CC BY 3.0 via Wikimedia Commons -
http://commons.wikimedia.org/wiki/File:Diffusion.svg#/media/File:Diffusion.svg
50. Gas Diffusion and Effusion
O Effusion:
O The process where a gas escapes through
a small hole from one chamber to another.
"Effusion" by Astrang13 - Own work. Licensed under CC BY-SA 3.0 via Wikimedia
Commons -
51. Gas Diffusion and Effusion
O Root Mean Square Velocity
O Graham’s Law of Effusion:
"Effusion" by Astrang13 - Own work. Licensed under CC BY-SA 3.0 via Wikimedia
Commons -
52. Real Gases
O The Kinetic Molecular Theory assumes
ideal behavior.
O Only holds at high temperature and low
pressure. Under these conditions gas
particles are moving rapidly and very far
apart so intermolecular forces are
negligible.
53. Real Gases
O Have Intermolecular forces that reduce
observed pressure.
O Small for Noble Gases and nonpolar
molecules.
O Large for ionic and polar compounds.
O Include
O London Dispersion Forces
O Dipole-Dipole Interactions
O Hydrogen Bonding
O Ionic Interactions
54. Real Gases
O Take up volume.
O Increases with molecular mass.
O Observed volume will be too low since
molecules take up some of the volume
measured.
55. Real Gases
O Graph shows how increasing pressure
affects the PV/nRT value.
Real Gases. 2015. CC-BY-SA.
56. Van der Waals Equation
O Ideal gas law can be corrected for volume and pressure using
the van der waals equation. Observed pressure is always
lower, observed volume is always higher than actual.
O The higher the value of a the greater the attraction between
molecules and the more easily the gas will compress.
O The b term represents the volume occupied by the gas particles.
•Source: Boundless. “Van der Waals Equation.” Boundless Chemistry. Boundless, 12 Nov. 2014. Retrieved 29 Mar. 2015 from
HTTPS://WWW.BOUNDLESS.COM/CHEMISTRY/TEXTBOOKS/BOUNDLESS-CHEMISTRY-TEXTBOOK/GASES-5/DEVIATION-
57. Air Pollution
O One of the best places to observe gases.
O Primary sources emitted directly into the
atmosphere.
O NOx
O SOx
O VOCs
O Particulates
O Free Radicals
59. Ozone Depletion
O Depleted through free radicals.
O Some reactions include:
O + O3 → 2 O2
Cl−+O3→ClO − + O2
ClO−+O3→Cl − + 2O2
O A single Cl froma CFCs can regenerate
and continue reacting with ozone for ~ 2
years.
Source: Boundless. “Ozone Depletion.” Boundless Chemistry. Boundless, 12 Nov. 2014. Retrieved 29 Mar. 2015 from
https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/gases-5/deviation-of-gas-from-ideal-behavior-
56/ozone-depletion-272-8710/
60. Unit 5 Review Activity
O This is NOT meant to replace homework
questions or studying.
O Unit 5 Review Problems
Oxygen = (22.1 L x 1.75 atm) / 10.0 L = 3.87 atm
Helium = (17.84 atm x 9.20L) / 10.0 L = 16.41 atm
3.87 + 16.41 = 20.28 atm
15.1 L x 3.14 mol / 4.92 mol = 9.64 L
(0.924 atm x 0.2576 L) / (0.08206 x 350) =0.00829 mol
0.142/0.00829 = 17.1 g/mol
Same: Boyle’s Law
Same: Boyle’s Law
Same: Charles’ Law
Same: Avogadros Law
Different: Molar Masses differ.
Pressure read is always lower than what it should be due to intermolecular forces. Correcting it means that we must add in a factor to account for those forces.
Correcting volume means we must subtract the volume the particles actually occupy.
Primary causes of air pollution are combustion engines (nitrogen oxides) (NO2 CO and CO2 produced, NO2 breaks into O and NO. O is a free radical).
and burning of coal for electricity (sulfur oxides). (SO2 produced, Oxidized to SO3, combines with water to make sulfuric acid—acid rain).
Scrubbers used to improve coal burning---CaO, combines with SO2 to make CaSO3. This is not a very soluble compound and is modified for use in many industrial applications including fertilizer (gypsum), drywall, desicants etc.
~ 9000 deaths a year in Ontario are linked to smog exposure. US and other countries issue health advisories via media when levels reach certain levels deemed unhealthy.
~Asthma and other respiratory conditions increase significantly in areas containing high levels. Also linked to birth defects. Worse in developing countries and countries with fewer regulations.