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5 properties of gasas
- Gases have an indefinite shape
- Gases can expand
- Gases can compress
- Gases have low densities
- Gases diffuse uniformly throughout their containers
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All temp. calculations must be in?
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The result of constantly moving molecules striking the inside wall of the container
Gas pressure
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collide with wall less frequently and less energy, results in a lower pressure
molecules that move more slowly
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collide more often, so the gas pressure increases
Molecules move more rapidly
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Measured by an instrument called a barometer
Atmospheric pressure
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Standard pressure of Atmosphere?
1 ATM
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Standard pressure of millimeters of Hg?
760 mm Hg
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Standard pressure of torr
760 torr (exactly)
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Equal standard pressure?
1 ATM= 760 mHg= 760 torr
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Volume and pressure are?
inversely proportional. as pressure goes up, volume goes down.
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Boyle's law is written?
P1V1=P2V2
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As pressure goes up, temp?
Goes up!
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Charles Law is written?
V1/T1 = V2/T2
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n (mol) and P (pressure): As one goes up, ?
so does the other
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At constant pressure, the volume, V, occupied by a gas sample is directly proportional to ?
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At constant vlume, the pressure, P, exerted by a gas sample is directly proportional to ?
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3 gas laws can be combined to represent the relationship between the three variables when they all change simultaneously
The combined gas law
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molecules of water in constant motion
some strike the surface with enough energy to escape the gas phase
when in a closed container, the vapor is collected in the space above the liquid
Vapor pressure
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vapor pressure of water is dependent on?
- the temp but not the volume of water.
- increases as temp increases
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Ptotal = P1+P2+P3+.......
- Daltons Law of partial pressures
- (587torr N + 158torr O + 7 torr Ar = 752 torr)
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a gas that always behaves in a predictable and consistent manner
an Ideal gas
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behave very much like the ideal gas model except at low T and high P
Real gases
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Always use what Conversions for..
P (pressure)=
V (volume)=
N (mole)=
T (temp)=
- P= ATM
- V= Liter
- N= mol
- T= Kelvin
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demonstrate rapid motion, move in straight lines, and travel in random directions
gas molecules
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the average kinetic energy of gas particles is proportional to the ?
Kelvin temp
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have no attraction for one another. After colliding they simply bounce away in a different direction
Gas molecules
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An ideal gas at absolute zero has?
No kinetic energy and therefore no motion
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in a collision between gas particles, there is no net loss of kinetic energy
elastic collisions
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referred to as the Ideal Gas constant, R
.0821 L atm/mol K
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PV = nRT
Ideal gas constant, R
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