42 terms

Gas Laws, Gas Laws

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Boyle's Law (graph and relationship)
Inverse
Charles Law (graph and relationship)
Direct
Gay-Lussac's Law (graph and relationship)
Direct
Boyle's Law (define in words)
For a fixed amount of gas at a constant temperature, the volume of the gas increases as the pressure decreases.
Charles Law (define in words)
For a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature increases.
Gay-Lussac's Law (define in words)
For a fixed amount of gas at a constant volume, the pressure of the gas increases as the temperature increases.
Boyle's Law (equation)
P1V1 = P2V2
Charles Law (equation)
V1/T1 = V2/T2
Gay-Lussac's Law (Equation)
P1/T1 = P2 /T2
Combined Gas Law (Equation)
P1V1/T1= P2V2/T2
Kinetic Molecular Theory
1) mass no volume 2) no forces exerted 3) constant, random motion 4) elastic collisions 5) kinetic energy based on temperature regardless of gas
Increases
As the volume of confined gas decreases at constant temperature, the pressure exerted by the gas___________.
Boyle's Law example
Which gas law is involved when a balloon pops after being sat on?
Kelvin
unit of measurement used for temperature
atmosphere
a unit of measurement used to describe pressure
liters
unit of measurement used to describe volume in Ideal Gas Law
zero degrees C
Standard temperature
1 atmosphere
Standard pressure
Where would there be more air pressure - sitting at your desk, Boulder City Colorado or on top of a mountain?
Faster
Heating up the molecules of a gas allow the particles to move......
MORE pressure
If MORE gas molecules created MORE collisions with the sides of a container, then there will be_____
Burst because increased altitude will decrease external pressure allowing the internal pressure of the balloon to expand the balloon beyond its capacity.
A fly away balloon will eventually ......
diffusion
spontaneous mixing of particles through continuous, rapid, random motion
Charles' Law
the volume of a given mass of gas at a constant pressure varies directly as its absolute temperature; V1T2 = V2T1
Kinetic Molecular Theory
collection of rules that describe the behavior of gases
STP
the temperature of 0°C and pressure of 1 atm
equal volumes of all gases, at the same temperature and pressure, have the same number of molecules; the volume and amount (moles) of the gas are directly proportional; V1n2=V2n1
Dalton's Law of Partial Pressure
in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases; P-total = P1 + P2 + P3 . . .
elastic collision
an encounter between two bodies in which the total kinetic energy of the two bodies after the encounter is equal to their total kinetic energy before the encounter
ideal gas
a theoretical gas composed of many randomly moving point particles that do not interact except when they collide elastically
Boyle's Law
For a fixed amount of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional; P1V1 = P2V2
temperature
A measure of the average kinetic energy of a substance
pressure
a force exerted by the substance per unit area on another substance
ideal gas constant
"R" the universal constant in the gas equation: PV = nRT
mole
the SI unit of amount of substance
kinetic energy
energy that a particle possesses by virtue of being in motion
Combined Gas Law
combines Charles' Law, Boyle's Law, Amonton's Law, and Avogadro's Law; P1V1n2T2 = P2V2n1T1
Ideal Gas Law
the equation of state of a hypothetical ideal gas; PV = nRT
real gas
as opposed to a perfect or ideal gas - exhibit properties that cannot be explained entirely using the ideal gas law
FLEECE
Fluid, Low Density, Expand to Fill Container, Effuse/Diffuse, Compressible, Exert Pressure
Effusion
Gas particles pushing or leaking out through small openings in the container
Ideal Gas Law (equation)
PV=nRT