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Ch 10 Chem Vocab

Chemistry

QuestionAnswer
diffusion spontaneous mixing of the particles of two substances caused by their random motion.
effusion a process by which gas particles pass through a tiny opening.
elastic collision a collision between gas particles and between gas particles and container walls in which there is no net loss of kinetic energy.
fluid a substance that can flow and therefore take the shape of its container; a liquid or a gas.
ideal gas an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory.
kinetic-molecular theory a theory based on the idea that particles of mater are always in motion
real gas a gas that does not behave completely according to the assumptions of the kinetic molecular theory
atmosphere of pressure (atm) exactly equivalent to 760 mm Hg
barometer a device used to measure atmospheric pressure
millimeter of mercury (mm of Hg) a common unit of pressure
newton the si unit for force that will increase the speed of a kilogram mass by one meter per second it is applied
pascal the pressure exerted by a force of one newton acting on an area of one square meter
kilopascal
pressure the force per unit area in a surface
standard temperature and pressure (STP) the agreed upon standard conditions of exactly one atm pressure and 0 degress celcius
standard ambient temperature and pressure (SATP)
torr
absolute zero the tempature given a value of zero on the kelvin scale
Kelvin
Boyle’s Law the volume fixed mass of gas varies inversely with pressure at constant tempature
Charles’s Law the volume of a fixed mass of gas at constant pressure varies directly with the kelvin temppature
Combined gas law the relationship between the pressure volume and tempature of a fixed amount of gas
Dalton’s Law of partial pressure the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Gay-Lusscac’s Law the pressure of a fixed mass of gas at constant volume varies directly with the kelvin tempature
Ideal gas law the mathematical relationship of pressure volume tempature and the number of moles of a gas
Partial pressure the pressure of each gas in a mixture
Avogadro’s Law equal volumes of gases at the same tempature and pressure contain equal numbers of molecules
van der Waals equation
bar
Gas Constant
diffusion Spontaneous mixing of the particles of two substances caused by their random motion
effusion The rate at which a gas escapes
elastic collision A collision between gas particles and between gas particles and container walls in which there is no net loss of kinetic energy
fluid A substance that can flow and therefore take the shape of its container; a liquid or a gas.
ideal gas An imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory.
kinetic-molecular theory A theory based on the idea that particles of mater are always in motion
real gas A gas that does not behave completely according to the assumptions of the kinetic molecular theory
atmosphere of pressure (atm) 760 mm Hg
barometer A device used to measure atmospheric pressure
millimeter of mercury (mm of Hg) A common unit of pressure
newton The si unit for force that will increase the speed of a kilogram mass by one meter per second it is applied
pascal Unit of measurement for pressure
kilopascal 1000 pascals
pressure The force per unit area in a surface
standard temperature and pressure (STP) The standard conditions of exactly one atm of pressure and 0 degress celcius
standard ambient temperature and pressure (SATP)
torr
absolute zero The temperature given a value of zero on the kelvin scale
Kelvin The temperature at which all thermal motion ceases
Boyle’s Law The volume fixed mass of gas varies inversely with pressure at constant tempature
Charles’s Law The volume of a fixed mass of gas at constant pressure varies directly with the kelvin temperature
Combined gas law The relationship between the pressure volume and temperature of a fixed amount of gas
Dalton’s Law of partial pressure The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Gay-Lusscac’s Law the pressure of a fixed mass of gas at constant volume varies directly with the kelvin temperature
Ideal gas law the mathematical relationship of pressure volume temperature and the number of moles of a gas
Partial pressure the pressure of each gas in a mixture
Avogadro’s Law equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
van der Waals equation Relates equation of real gas to that of the ideal
bar
Gas Constant R equals 0.082 liter-atmospheres per mole-degree
Created by: j.millsdar4