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Behavior of Gases

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Title: Behavior of Gases


1
Behavior of Gases
  • Ch 12 Prentice Hall

2
Kinetic Theory
  • ? Gases are composed of SMALL, SEPARATE particles
    called MOLECULES.
  • ? Gas molecules are in CONSTANT MOTION
  • ? All COLLISIONS between particles are PERFECTLY
    ELEASTIC
  • ? The MOLECULES of a gas display no ATTRACTION or
    REPULSION for one another.

3
Kinetic Theory
  • ? The AVERAGE KINETIC ENERGY of the molecules is
    DIRECTLY PROPORTIONAL to the KELVIN temperature
    of the gas.

4
Ideal Gas
  • ? Gas whose BEHAVIOR conforms to the KINETIC
    THEORY -it is THEORETICAL.

5
  • Gas Pressure
  • Pressure FORCE AREA ____ atm
  • Atmospheric Pressure - the PRESSURE the earths
    ATMOSPHERE exerts due to its WEIGHT.
  • Barometer
  • ? Instrument used to measure ATMOSPHERIC
    PRESSURE
  • ? Invented by TORRICALLI

6
The Combined Gas LawCombines the following laws
and equations together
7
Charles law
Variation of gas volume with temperature while
pressure is kept constant
V1/T1 V2/T2
T (K) t (0C) 273.15
8
Boyles Law
P1V1 P2V2
Pressure and volume units can be any variant of
pressure and volume HOWEVER the units MUST agree
for both pressures and both volumes!
9
Combined Gas Law
  • ? Expresses the relationship between the
    PRESSURE, VOLUME and TEMPERATURE of a FIXED
    amount of GAS.
  • Equation P1V1 P2V2
  • T1 T2

10
STANDARD TEMPERATURE AND PRESSURE
  • STP CONDITIONS
  • 273 K
  • 1 atm 760 mmHg

11
Combined Gas Law
  • Ex A sample of gas has a volume of 201 L when
    its temperature is 293 K and its pressure is 224
    mmHg. What volume will the gas occupy at STP?
  • V1 201 L V2 ?
  • T1 293 K T2 273 K
  • P1 224 mmHg P2 760 mmHg
  • (224) (201) (760) x
  • (293) (273)
  • (224) (201) (273) (293) (760) x
  • X 55 L

12
Diffusion
  • ? The RAPID spreading of a GAS
  • Grahams Law of Diffusion
  • ? Under the same conditions of TEMPERATURE and
    PRESSURE, gases DIFFUSE at a rate INVERSLEY
    proportional to the SQUARE ROOT of their
    DENSITIES (or MOLAR MASS)
  • Equation

13
Ideal Gas Equation
  • Equation PV nRT
  • ? New variables
  • n AMOUNT of gas in MOLES
  • R UNIVERSAL GAS CONSTANT
  • PROPORTIONALLY constant
  • value depends on UNITS used for PRESSURE and
    VOLUME
  • value of R when using kPa and L
  • R 8.314 L . kPa / Mol . K

14
  • Ex The average lung capacity for a female
    student is 3.9 L. At normal body temperature,
    37oC, and 110 kPa, how many moles of air could
    her lungs hold?
  • P 110 kPa V 3.9 L T 310 K (273
    37)
  • n X R 8.314 L . kPa / Mol . K
  • (110)(3.9) x (310)(8.314)
  • (110)(3.9) 0.17 mol
  • (310)(8.314)

15
Avogadros Law
  • ? Equal VOLUMES of different GASES under the SAME
    conditions have the SAME number of PARTICLES.
  • ? Conversely, if samples of DIFFERENT GASES at
    the same TEMPERATURE and PRESSURE contain the
    SAME number of PARTICLES, then the VOLUMES of all
    the SAMPLES must be EQUAL.
  • ? At STP, one MOLE of any gas occupies a VOLUME
    of 22.4 L.
  • ? 22.4 L is the MOLAR VOLUME of a gas.

16
Daltons Law of Partial Pressures
Equation PT P1 P2 P3
  • ? The PRESSURE of a gas MIXTURE is the SUM of the
    INDIVIDUAL PRESSURES of each gas ALONE.

17
  • ? Ex Oxygen gas has been collected over water at
    a total pressure of 95.0 kPa and a temperature of
    25oC. What is the pressure of the dry oxygen gas?

PT 95 kPa P vapor 3.17 kPa P oxygen
X 95 3.17 x 91.83 kPa x
18
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