gas law flipbook

gas

law

flipbook

INDEX

combined gas laws

properties of gases

practice problems

ideal gas law & molar volume

experimental gas laws

properties of gases

what are they?

Kinetic Molecular Theory assumptions of the model: -all particles are in constant, random, motion -all collisions between particles are perfectly elastic (even exchange of energy) -the volume of the particles in a gas is negligible -the average kinetic energy of the molecules is its Kelvin temp. This theory neglects any intermolecular forces as well. Gases expand to fill their container while solids/liquids don't. Gases are also compressible unlike solids/liquids.

Volume, Temperature, and Pressure 4 quantities to define the state of gas: -quantity of gas, n (moles) -temperature of gas, T (Kelvins) -volume of gas, V (liters) -pressure of gas, P (atmospheres) Gas Pressure: a measure of the force that a gas exerts on its container- force/unit area: N/m^2 (1.0 Pascal)Gas Volume: Gas is a state of matter that has no fixed shape and no fixed volume. Gas Temp.: a measure of the average translational kinetic energy of the molecules

conversions: 1.00 atm = 760.00 mmHg = 760.00 torr = 29.92 Hg = 14.7 psi = 101.325 kPa = 10^5 Pa

methods to convert are using dimensional analysis

ideal gas law

avogadro's principle/molar volume

ideal gas law

molar volume- this is the volume that one mole of gas occupies at STP. It is 22.4 L. avogadro’s law, a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules.

-a description of gas behavior that permits you to solve for the number of moles of a contained gas when given only ONE VALUE EACH for P, V, and T.

Equation: PV = nRT- ideal gas constant(R):-0.0821 L x atm/mol K -62.4 L x mmHg/mol K -8.314 L x KPa/mol K

STP- standard temperature (273 K and standard pressure (101.3 kPa) new conversion factor: - 22.4 L = 1 mol at STP

V = must be LT = must be in Kelvin

boyle's, charle's, gay-lussac's

laws

of combined volumes: volume of gases always combine with one another in the ratio of small whole numbers, as long as volumes are measured at the same T and P

"father of chemistry"-the volume of a confined gas is inversely proportional to the pressure exerted on the gas. -all gases behave in this manner

if a given quantity of gas is held at a constant pressure, then its volume is directly proportional to the absolute temperature

-at constant volume, pressure and temperature of gases are directly related-if the pressure increases ( and the container is not expandable) the temp. increases

-p a i/v : pressure & volume inversely proportional-volume: high, pressure: low at constant temp. -holds true only at low pressures

-V a T-temp. a volume at constant pressure

equation: p1t2=p2t1

equation: v1t2=v2t1

equation: p1v1=p2v2

charle's

boyle's

gay-lussac's

Índice

Sección

Versus

Texto

Timeline

Frase

Mapa

10

Imagen

Datos

11

Vídeo

Equipo

12

Procesos

Gracias

combined gas law

P V T Relationshipwhat happens to one variable if two of the other variables change?

this law combines the laws of boyle, charles, and gay-lussac-you can use this law to find the equations for all of the other laws

practice problems

*i wrote the laws they are on the paper*

THANKS!