effusion: the process by which a gas escapes from its container through a tiny hole into a region with low pressure
grahamās law of effusion: effusion rate of gas is inversely proportional to the square root of its molar mass and its density
law of effusion and law of diffusion are interchangeable
kinetic molecular theory: behavior of gases is directly related to the basis of motion of the particles that make up the gas
individual gas molecules treated as point masses
gas is mostly empty space
gas molecules are constantly and randomly moving throughout its occupied space and continually collide with each other and the container walls
intermolecular forces are negligible, assuming particles donāt interact at all
average kinetic energy of particles is proportional to absolute temperature of the gas - all populations of gas molecules at the same temperature have same average kinetic energy
universal gas constant: R=8.314 (kg*m^2)/(s^2mol**K)
diffusion: spread of one substance through another - occurs when there are differences in composition of the mixture of gases within occupied space
mean free path: average distance a particle can travel through air or gas before colliding with another particle, depends on density and pressure
Pressure: P=F/A where F is force and A is surface area
Barometer: instrument that is measured with a barometer
Manometer: measures pressure exerted by a gas, displayed by delta h = P sample - P atm
Boyles Law: Pressure is inversely related to volume at a constant T and n.
Charlesā Law: Volume of a fixed quantity of gas is directly proportional to the temperature (in K) when pressure and n are constant
Avogadroās Law: Pressure is proportional to moles of gas when temperature and volume are constant
Amontonsā Law: Volume is proportional to its temperature at constant pressure and volume; pressure is directly proportional to temperature if volume is held constant
Combined Gas Law: (P1V1)/T1 = (P2V2)/T2
Ideal Gases: gases that behave in accordance with combined gas law; assumed that volumes of individual gas particles are insignificant
Ideal Gas Law: PV=nRT
Standard Temperature and Pressure (STP): 0 degrees C and 1 bar of pressure; one mol of an idea gas will occupy 22.4 L
Density of any gas at STP can be found by dividing its molar mass by the molar volume
we can use the ideal gas law to find n, which is number of moles, which we can then use to perform stoichiometric calculations
Partial Pressure: pressure exerted by each individual gas in a mixture of gases
Atmospheric Pressure: sum of partial pressures of all gases in the air
Daltonās Law of Partial Pressures: total pressure of any mixture of gases is the sum of the partial pressures in the mixture
Mole Fraction: abundance of a specific component i in a mixture of gases
van der Waals Equation: corrects for intermolecular forces and volume taken up by particles
van der Waals Forces: intermolecular forces that contribute to the value of the a constant of a gaseous substance
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