gases & atmospheric chemistry
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Gases & Atmospheric Chemistry. Unit 5. States of Matter. Solid, Liquid & Gas. Forces Holding Solids Together. The forces that are holding a solid together are very strong Forces: Ionic Covalent Some intermolecular forces in some substances. Forces Holding Solids Together. - PowerPoint PPT PresentationTRANSCRIPT
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Gases & Atmospheric Chemistry
Unit 5
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States of MatterState PropertiesSolid •Definite shape and volume
•Are virtually incompressible•Do not flow easily
Liquid •Assume the shape of the container but have a definite volume•Are virtually incompressible•Flow readily
Gas •Assume the shape and volume of the container•Are highly compressible•Flow readily
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Solid, Liquid & Gas
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Forces Holding Solids Together The forces that are holding a solid
together are very strong
Forces: Ionic Covalent Some intermolecular forces in some
substances
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Forces Holding Solids TogetherExplains why solids: Have a definite shape
Strong bonds holding molecules together (rigid)
Do not flow readily In order to be able to flow particles have to
slip past one another, strong bonds do not allow this
Cannot be compressed Strong bonds mean that there are few
empty spaces between the particles
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Forces Holding Liquids Together The forces that are holding a liquid
together are not as strong as ionic or covalent bonds
Forces: intermolecular
Bonds hold molecules closely together but do not lock them into place
Liquids can spread out and take the shape of the container while keeping a constant volume
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Because gases have NO definite shape or volume there appears to be an absence of forces between the molecules in a gas
No limit to the diffusion of gas molecules into the atmosphere (a very large container)
Gases – Lack of Forces
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The Kinetic Molecular Theory Kinetic Molecular Theory = the idea
that all substances contain particles that are in constant, random motion
Particles are continually moving & colliding
Explains:1. Diffusion2. Evaporation
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Diffusion Example: food colouring is added to
water will slowly spread out
Explanation from Kinetic Molecular Theory: molecules of food colouring and molecules of water are moving and colliding with each other which causes them to mix
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Evaporation Example: water in an open container
slowly decreases as some of the water evaporates
Explanation from Kinetic Molecular Theory : some water molecules in the open container obtain sufficient energy from collision to escape from the liquid
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3 Types of Motion A particle an exhibit 3 type of motion:
1. Vibrational = back-and-forth motion of atoms within a molecule
2. Rotational = spinning
3. Translational = straight line
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3 Types of Motion
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Motion in Relation to State Solid – mainly vibration due to
restriction of the strong bonds Particles stay together in a relatively
ordered state Liquid – some of all 3 types of motion
Less orderly state than solid Gas – rotate and vibrate but
translational (straight-line) motion is the most significant Most disordered state with no organization
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Properties of Gases1. Gases are compressible: When pressure is
increased, the volume of a gas decreases. When pressure is decreased, the volume of a gas increases. The volume of a liquid and a solid remain constant during changes in temperature because their particles cannot move independently of one another like the gas particles can.
2. Gases expand as the temperature increases (much more than water and solid).
3. Gases have very low viscosity (they flow fast). 4. Gases have much lower densities than solids or
liquids. 5. ALL Gases are miscible (some liquids are miscible
yet some are immiscible).
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Earth’s Leaky Atmosphere? Many of the gases that make up Earth’s
atmosphere and those of the other planets are slowly leaking into space.
Hot gases, especially light ones, evaporate away
chemical reactions and particle collisions eject atoms and molecules
and asteroids and comets occasionally blast out chunks of atmosphere
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The Atmosphere
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Measurement of Gas Pressure Pressure = force
exerted on an object per unit of surface area Unit = Pa (pascal)
Atmospheric Pressure = the force per unit area exerted by air on all objects Standard Atmospheric
Pressure: 101.3 kPa or 760 mm
Hg or 760 torr one standard atmosphere
(1atm)
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Units of PressureUnit of pressure Symbo
lInstruments that use the unit
1) Millimetres of Mercury: mm of Hg.
mmHg Blood pressure meters
2) 1 Torr torr Vacuum pumps
3) Pascal (Pa) the SI unit of pressure. 1 kPa = 1000 Pa
Pa Pressure sensors in pipelines
4) Bars: 1 bar bar Pressure sensors in scooba gear
5) Atmospheres (atm) atm Gas compressors
6) Pounds per square inch Psi Hydraulic pumps
Conversion: 1 atm = 760 mm of Hg = 101.325 kPa = 1.01325 bar = 760 torr = 14.7 psi
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Pressure Conversions
A. What is 475 mm Hg expressed in atm?
760 mm Hg = 1 atm
475 mm Hg = x
x = 475/760 = 0.625 atm
B. The pressure of a tire is measured as 10 kPa. What is this pressure in mm Hg?
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Pressure Conversions
A. What is 2 atm expressed in torr?
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STP & SATP STP = Standard Temperature &
Pressure Exactly 0°C (273K) 1atm or101.325kPa
SATP = Standard Ambient Temperature and Pressure exactly 25°C (298K) 100kPa
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Gases Moving Gases naturally move from areas of
high pressure to low pressure, because there is empty space to move into
Examples of Spray Cans: whipped cream, hair spray, paint
a propellant forces the product out
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Gas Law – Boyle’s LawRelationship: Pressure & Volume
As pressure on a gas increases, the volume of the gas decreases
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Pressure and Volume Relationship As pressure increases volume decreases
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Gas Law – Boyle’s LawRelationship: Pressure & Volume
Boyle’s Law = as the pressure on a gas increase, the volume of the gas decreases proportionally
p1v1 = p2v2
Provided that the temperature and amount of gas are constant
The volume and pressure of a gas are inversely proportional
Graphically: P 1 (inverse relationship) V
Robert Boyle (1627-1691). Son of Early of Cork, Ireland.
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Boyle’s LawSample Problems: 1. A 350 mL sample of air at 125 kPa is reduced to a
volume of 250 mL. Calculate the new pressure.(ans: 180 kPa)
2. A 55 mL sample of helium at 525 torr is compressed to a certain volume at 2.5 atm. What is the new volume, in litres?(ans: 0.015 L)
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