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| 15430131267 | manometer | instrument to measure pressure of gas in a container |  | 0 |
| 15430134755 | barometer | an instrument used to measure atmospheric pressure |  | 1 |
| 15430143159 | average height of barometer | 760 mmHg | 2 | |
| 15430146753 | atmospheric pressure | mass of air being pulled toward the center of the Earth by gravity | 3 | |
| 15430166540 | standard atmosphere (atm) | a unit of pressure; it is the pressure required to support 760 mm of mercury in a mercury barometer at 25°C 1 atm = 760 mmHg (torr) = 101325 Pa = 14.7 psi | 4 | |
| 15430781873 | kelvin scale of temperature | an absolute scale of temperature in which 0 K is the absolute zero of temperature |  | 5 |
| 15430186499 | Boyle's Law | a principle that describes the relationship between the pressure and volume of a gas at constant temperature P₁V₁ = P₂V₂ inverse relationship between pressure and volume |  | 6 |
| 15430206435 | Charles's Law | a principle that describes the relationship between the temperature and volume of a gas at constant pressure V₁/T₁ = V₂/T₂ volume of each gas is directly proportional to temperature |  | 7 |
| 15430230346 | Avogadro's Law (Avogadro's Hypothesis) | equal volumes of gases at the same temperature and pressure contain equal numbers of molecules P₁/n₁ = V₂/n₂ for a gas at a constant temperature and pressure, the volume is directly proportional to the number of moles of gas |  | 8 |
| 15430599382 | root mean square velocity | the square root of the average of the squares of the individual velocities of gas particles u (average speed of gas particle (m/s)) = √3RT/M (molar mass) R = 8.31 J/mol·K (8.31x10³ g·m²/s²·mol·K) M = molar mass of gas |  | 9 |
| 15430291544 | Ideal Gas Law | PV=nRT (n is equal to the number of moles of the substance and R is the gas constant 0.0821) |  | 10 |
| 15430306152 | Combined Gas Law | the relationship between the pressure, volume, and temperature of a fixed amount of gas |  | 11 |
| 15430322506 | volume of 1 mole of gas at STP | 22.4 L/mol |  | 12 |
| 15430331408 | standard temperature and pressure (STP) | a temperature of 273 K and a pressure of 1.00 atm | 13 | |
| 15430345138 | Dalton's Law of Partial Pressures | for a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone |  | 14 |
| 15430350864 | partial pressure | the pressure that a particular gas would exert if it were alone in the container |  | 15 |
| 15430374764 | mole fraction and partial pressure | The partial pressure of a component in a gaseous mixture is its mole fraction of gas multiplied by the total pressure For gases, the mole fraction of a component is equivalent to its percent by volume divided by 100% |  | 16 |
| 15430411421 | collecting gas over water | gas in bottle is a mixture of water vapor and oxygen collected when the rate of escape equals the rate of return (equilibrium), the number of water molecules in vapor state remains constant, thus pressure of the water vapor remains constant |  | 17 |
| 15430498164 | vapor pressure of water | pressure exerted by water vapor in equilibrium with liquid water in a closed container at a specific temperature | 18 | |
| 15430504512 | Kinetic Molecular Theory of Gases | 1. the particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be negligible (zero) 2. the particles are in constant motion. the collisions of particles with the walls of the container are the cause of the pressure exerted by the gas 3. the particles are assumed to exert no forces on each other; they are assumed neither to attract nor repel each other 4. the average kinetic energy of a collision of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas |  | 19 |
| 15430582262 | average kinetic energy | directly proportional to the absolute temperature |  | 20 |
| 15428057073 | diffusion | the process by which molecules move from an area of higher concentration to an area of lower concentration smaller gas particles diffuse faster than larger ones the rate of the mixing of gases |  | 21 |
| 15430683476 | effusion | the passage of a gas through a tiny orifice into an evacuated chamber | | 22 |
| 15430700648 | Graham's Law of Effusion | states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass |  | 23 |
| 15428050309 | rate of effusion | measures the speed at which the gas is transferred into the chamber |  | 24 |
| 15430902108 | rate of effusion using density | the rate of effusion of a gas is inversely proportional to the square root of the density of the gas r₁/r₂ = √D₂ /√D₁ |  | 25 |
| 15430958318 | time of effusion | the time it takes a gas to effuse if directly proportional to the square root of the molar mass of the gas t₂/t₁ = √MM₂/√MM₁ |  | 26 |
| 15430712027 | Van der Waals Equation | a mathematical expression for describing the behavior of real gases |  | 27 |
| 15430736458 | intermolecular forces | relatively weak interactions that occur between molecules | 28 | |
| 15430740283 | dipole-dipole attraction | attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other |  | 29 |
| 15430745783 | london dispersion forces | forces, existing among noble gas atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor |  | 30 |
| 15479413098 | when does a gas behave most ideally | low pressure, high temperature, low number of moles | 31 | |
| 15479416327 | when does a gas behave less ideally | high pressure, low temperature, high number of moles | 32 |
