Chapter 5 - gases Flashcards
barometer
a device for measuring atmospheric pressure.
manometer
a device for measuring the pressure of a gas in a container.
torr
another name for millimeter of mercury (mm Hg)
standard atmosphere
a unit of pressure equal to 760 mm Hg.
pascal
the SI unit of pressure; equal to newtons per meter squared.
Boyle’s law
the volume of a given sample of gas at constant temperature varies inversely with the pressure.
ideal gas
a hypothetical gas that strictly obeys the ideal gas law.
Charle’s law
the volume of a given sample of gas at constant pressure is directly proportional to the temperature in kelvins.
Avogadro’s law
equal volumes of gases at the same temperature and pressure contain the same number of particles.
ideal gas law
an equation of state for a gas, where the state of the gas is its condition at a given time; expressed by PV=nRT, where P=pressure, V=volume, n=moles of the gas, R=the universal gas constant, and T=absolute temperature. This equation expresses behavior approached by real gases at high and low .
molar volume
the volume of one mole of an ideal gas; equal to 22.42 liters at STP.
standard temperature and pressure (STP)
the condition 0 degrees celsius and 1 atmosphere of pressure.
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.
partial pressure
the independent pressures exerted by different gases in a mixture.
mole fraction
the ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture.
kinetic molecular theory (KMT)
a model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion.
root mean square velocity
the square root of the average of the squares of the individual velocities of gas particles.
joule
the SI unit for energy, defined as Kg* m2/s2
effusion
the passage of a gas through a tiny orifice into an evacuated chamber.
diffusion
the mixing of gases.
Graham’s law of effusion
the rate of effusion of a gas is inversely proportional to the square root of the mass of its particles.
van der Waals equation
a mathematical expression for describing the behavior of real gases.
atmosphere
the mixture of gases that surrounds the earth’s surface.
air pollution
contamination of the atmosphere, mainly by the gaseous products of transportation and production of electricity.
