42 terms

CoachTonerTEACHER

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

sitting at your desk

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

Avogadro's Law

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