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20 Cards in this Set
- Front
- Back
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What is the kinetic-molecualar theory based on?
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The idea that particles of matter are always in motion
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What is an ideal gas?
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An imaginary gas that perfectly fits all the assumptons of the kinetic-molecular theory.
No real gas fits all the points perfectly but the noble gases are the closest. |
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What are the 5 assumptions in the Kinetic-Molecular theory of gases?
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1. Gases consist of large numbers of tiny particles that are far apart realative to their size.
2. Collisions are elastic between particles and the container. 3. Particles are always in motion. No attractive forces between them except near condensation point. 4. No forces of attraction or repulsion between particles. 5. The average kinetic energy of gas particles depends on the temperature of the gas. |
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What is an elastic collision?
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a collision in which there is no net loss of kinetic energy.
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What is "Expansion"?
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no definite shape or volume; take shape/volume of container
-move in all directions (3) -no significant attraction or repultion (4) |
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What is "Fluidity"?
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has particles glide easily past eachother
-no significant attraction or repultion (4) |
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What is "Low Density"?
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Density in gaseous state is about 1/1000 of the substance in liquid or solid state
-gases are farther apart (1) |
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What is "Compressibility"?
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gas particles can be forced in to a smaller area, (with a higher density)
-gases "chose" to be farther apart (1) |
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What is "Difusion"?
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Gases spread out and mix together without being stirred
-gases spread out(1) -gases are always randomly moving (3) Rate Depends on: speed, diameters, attractive forces |
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What is "Effussion"?
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The process by which gas particles pass through a tiny opening
-gases spread out(1) -gases are always randomly moving (3) Rate is proportional to velocities |
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What is "Pressure"?
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Pressure = force/area
lower area > force up or lower force > area down |
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What is "Newton"?
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SI unit for Pressure
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What is a barometer?
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A device used to measure atmospheric pressure
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What are the units of Pressure?
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-millimeters of mercury, Hg, based on a mercury barometer
-1 mm Hg = 1 toor -atmosphere of pressure, atm -pascal, Pa, one newton of force exerted on 1 square meter |
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What is the standard temperature and pressure (STP)?
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1 atm pressure
0 degrees Celcius |
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What is Boyle's Law?
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P1V1/P2V2
as the pressure increases the volume decreases -there is more space for the molecules to move so there is less pressure forcing them together |
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What is Charles's Law?
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V1=V2
T1 T2 gases expand when heated -the heat excites the molecules so they move faster and farther |
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What is important to remember when calculating Charles's Law?
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USE KELVIN!!!!!
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What is Gay-Lussac's Law?
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P1=P2
T1 T2 as temperature is increased the pressure is increased -increase in temperature excites the molecules so they hit the container and eachother more frequently and with greater force thereby increasing the pressure |
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What is the Combined Gas Law?
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P1V1=P2V2
T1 T2 The relationship between pressure, volume and temperature When one variable is kept constant it is removed from the equation |
