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Expansion
gas particles move in all directions and fill the container
Fluidity
gas particles have no attractive forces so particles flow past each other
Low Density
gas particles are far apart
Compressibility
the volume of particles are negligible compared to the container and the particles are far apart
Diffusion
spontaneous (no energy required) mixing of two gases caused by random motion
Effusion
gas particles pass through a small opening
Pressure
is the result of large numbers of rapidly moving gas particles simultaneously colliding with an object
Factors affecting gas pressure
amount of gas (moles) volume and temperature
Pressure
Force/Area
Pressure Units
1 atm = 760mmHg = 760 torr = 101.3 kPa
Standard Temperature and Pressure (STP)
Temperature: 0C or 273K
Convert ot kelvin
Pressure: 1 atm or 760mmHg or 101.3kPa
Ideal Gas
follows gas laws at all conditions of pressure and temperature and would conform to the postulates of the KMT. Particles would have no volume & no attraction b/w the particles.
Real Gases
due to attractive forced it can condense to a liquid when it is compressed or cooled. Water vapor at 100C condenses to a liquid when it cools. Polar molecules attracted to each other.
no gas conforms to all the KMT
ideal gas doesn’t exist
Particles of real gases
have volume and there are attractions b/w particles
High temperatures and Low Pressure
Real Gas behaves like an ideal gas.
At high temps: particles have enough energy (KMT) to overcome attractive forces
At low pressure: particles are far apart
Real gases at High Pressure
Deviate from an ideal gas because the attractive forces reduce the distance b/w the particles and the gas occupies a smaller volume than expected
Most ideal gas Behavior
Nonpolar molecule: weakest attractive force
A gas consists of a large #s of particles with an insignificant ___ that are in constant ____
volume, motion
Each particle travels in a ____ ____ until it collides with another particle or object. The particle exerts a ____ as a result of that collision.
straight line, force
All collisions of gas particles are perfectly ___ (total kinetic energy constant).
elastic
There are no ____ forces b/w molecules of an ideal gas.
attractive
absolute temp (kelvin) is a measure of the ____
average kinetic energy
Gases at the same temp have
the same average kinetic energy
Kinetic energy: 1/2mv²
1/2(mass)(velocity)²
Ideal gas conditions
High temp
low pressure
particle size small compared to space b/w particle
Interactions b/w particles are insignificant
Nonideal gas condition
Low temp
high pressure
particle size significant compared to space b/w particles
Interactions b/w particles are significant
Constant Volume
Temp, Kinteric Energy, Pressure are all direct
Cool gas: fewer and less energetic collisions
Hot gas: more and more energetic collisions
Constant temp
Volume and Pressure are Inverse
Gas Laws
Apply to IDEAL Gases
Boyle’s Law
Pressure-Volume Relationship (constant Temp) P1V1=P2V2
Volume and Pressure are inverse
When volume increases the collision rate decreases causing pressure to decrease with constant temperature
Charles’ Law
Temperature-Volume Relationship (constant Pressure) V1/T1 = V2/T2
Temp and Volume are direct
At constant pressure and an increase in temp the collision rate increases and are the collisions are more energetic. To maintain constant gas pressure, the volume increases.
Gay-Lussac’s Law
Pressure-Temperature Relationship (constant Volume) P1/T1 = P2/T2
Temp and pressure are direct
Ina. container that has a fixed volume, an increase in temp causes the collisions to be more frequent and with more energy. Since the volume is constant the gas pressure increases.
Combined Gas Law
(P1*V1)/T1 = (P2*V2)/T2
Avogadro’s Principal
At the SAME TEMPERATURE and PRESSURE, equal VOLUMES of gases contain the SAME # of particles.
As the # of particles increases, the frequency of collisions with the walls of the container increases which leads to an increase in the pressure of the gas
Flexible container will expand until the pressure of the gas inside the container once again balances the pressure of the gas outside
Thus, Volume of the gas is proportional to the # of gas particles
Gas mixtures: Dalton’s Law of Partial Pressures
Ptotal = Pa + Pb + Pc + …
Partial Pressure is the pressure that an individual gas would exert if it were alone in the container.
Gases collected by WATER DISPLACEMENT
The KMT predicts that the pressure rises as the temp of a gas increases because___
both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall
Higher Molecular speed
the lighter the molecule
The KMT does not work well for real gases at low temps because the gas molecules
have the opportunity for intermolecular attraction
T
T or F: The average kinetic energy of an ideal gas particle is proportional to the temp in Kelvin
T
T or F: The volume of ideal gas particles is negligible compared to the volume of the container
T
T or F: The ideal gas particles exert no attractive force upon each other
F
T or or F: The mass of an ideal gas is negligible
T
T or F: An ideal gas will not condense when compressed or cooled
F
T or F: The pressure decreases as the temp of a gas increases
T
T or F: Real gases deviate from ideal gas behavior because the attractions b/w gas molecules exists
F
T or F: Real gas are more like ideal gases with increasing pressure
T
T or F: Real gases are more like ideal gases with increasing temp
F
T or F: Real gas are more like idea gases with decreasing volume of the gas container
T
T or F: Ideal gas behavior is best achieved at low pressure and high temp with real gases