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unit 8

gases

TermDefinition
Pressure continuous physical force exerted on or against an object by something in contact with it.
Newton the SI unit of force. It is equal to the force that would give a mass of one kilogram an acceleration of one meter per second per second, and is equivalent to 100,000 dynes.
Barometer an instrument measuring atmospheric pressure, used especially in forecasting the weather and determining altitude.
Millimeters of Mercury a manometric unit of pressure, formerly defined as the extra pressure generated by a column of mercury one millimetre high, and currently defined as exactly 133.322387415 pascals.
Atmosphere of Pressure the pressure within the atmosphere of Earth.
Pascal the unit of pressure or stress in the International System of Units (SI).
Partial Pressure the pressure that would be exerted by one of the gases in a mixture if it occupied the same volume on its own.
Dalton's law of partial pressure that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Boyles Law Boyle's law states that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature P1V1 = P2V2
Absolute Zero the lowest temperature that is theoretically possible, at which the motion of particles that constitutes heat would be minimal.
Charle's law a statement that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature
Gay-Lussac's law a law stating that the volumes of gases undergoing a reaction at constant pressure and temperature are in a simple ratio to each other and to that of the product.
Combined gas law expresses the relationship between the pressure, volume, and absolute temperature of a fixed amount of gas
Avogadro's law a law stating that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
Standard molar volume of a gas the volume of one mole of a gas at STP
ideal gas law relation between the pressure P, volume V, and temperature T of a gas in the limit of low
ideal gas constant the proportionality constant in the ideal gas equation
Graham's law of effusion the ratio of the rates of diffusion or effusion of two gases is the square root of the inverse ratio of their molar masses
Created by: ea386057
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