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Chemistry
Gases Vocabulary
| 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 |
Created by:
jordinlevy
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