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Chemistry

Gases Vocabulary

TermDefinition
Ideal Gas Law Pv=nRT
P(Ideal Gas Law) pressure in atmospheres
v(Ideal Gas Law) volume in liters
n(Ideal Gas Law) number of moles of gas
R(Ideal Gas Law) universal gas constant 0.0821 L x atm/mol x K
T(Ideal Gas Law) kelvin temperature
Combined Gas Law P1V1 / T1 = P2V2 / T2 or P1V1T2=P2V2T1
1 atm= 760mmHg
1 atm=760mmHg= 101.3kPa
Grahams's Law Of Effusion says that a gas will effuse at a rate that is inversely proportional to the square root of its molecular mass, MM
Dalton's Law Of Partial Pressures says that the sum of the individual pressures of all the gasses that make up a mixture is equal to the total pressure or the partial pressure of each gas is equal to the mole fraction of each gas x total pressure
Boyle's Law P1V1=P2V2
Gay-Lusaac's Law P1/T1=P2/T2
Dalton's Law Pt=P1+P2+P3................
Charle's Law States That the volume of a gas is directly proportional to its temperature in kelvins @ constant mass and pressure
When the pressure and number of particles of a gas are constant, which of the following is also constant? the ratio of the volume and temperature in kelvins
As the temperature of a fixed volume of a gas increases, the pressure will increase
Under what conditions do real gases deviate most from ideal behavior? low temperature and high pressures
Characteristics Of Gases ~expand to fill any container ~are fluids(like liquids ~no volume ~have very low densities (1/1000) ~are compressible, also they effuse and diffuse
Kinetic-Molecular Theory (KMT) based on the idea that particles of matter are always in motion
How many assumptions are there of KMT? 5
First Assumption gases consist of large number of tiny particles that are far apart relative to their size
Second Assumption collisions between gas particles and between particles and container walls are elastic collisions
Third Assumption gas particles are in continuous, rapid, and random motion, they therefore possess kinetic energy, the energy of motion
Fourth Assumption there are no forces of attraction or repulsion between gas particles
Fifth Assumption The average K.E. of gas particles depends on the temperature of the gas not the identity of the particle
Temperature the measure of kinetic energy
SI Unit For Pressure Pascal (Pa)
Boyle's Law States That the pressure and volume of a gas are inversely related @constant mass and temperature
Avogadro's Law States That the volume is directly proportional to the number of moles
Gay-Lusaac's Law States That the pressure and absolute temperature of a gas are directly related @ constant mass and volume
Ideal Gas Law Definition an ideal gas law is one whose particles take up no space and have no attractive forces for each other
Density Formula Pm=dRT
Diffusion the tendency of molecules and ions to move form areas of high concentration to areas of low concentration
Effusion the diffusion of a gas through a small opening in an otherwise closed container
Charle's Law V1/T1=V2/T2
Created by: jordinlevy