Question | Answer |
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 matter are always in motion |
real gas | a gas that does not behave completely according to the assumption of the kinetic-molecular theory |
atmosphere of pressure (atm) | exactly equivalent to 760mm 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; the force that will increase the speed of a one 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 | more convenient way to express pressure; 1 atm is equal to 101.325 kPa |
pressure | the force per unit area on a surface |
standard temperature and pressure (STP) | the agreed-upon standard conditions of exactly 1 atm pressure and 0 C |
standard ambient temperature and pressure (SATP) | 1 bar; 1 atm and 25 C |
torr | a pressure of 1 mm Hg; 1 torr |
absolute zero | the temperature -237.15 C, given a value of zero in the Kelvin scale |
Kelvin | a scale that starts at a temperature corresponding to -273.15 C |
Boyle’s Law | the volume of a fixed mass of gas varies inversely with pressure at constant temperature |
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 | an equation of state that extends the ideal gas law to real dases by inclusion of two empirically determined parameters, which are different for different gases |
bar | 100 kPa |
Gas Constant | R equals 0.082 liter-atmospheres per mole-degree |