Term | Definition |
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 |