Chem test gases
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21 Terms
kinetic molecular theory
the behavior of matter in terms of particles in motion
particle size KMT assumptions
gases consist of small particles separated from one another
particle motion KMT assumptions
gas particles are in constant and random motion. collisions between gas particles are elastic
elastic collision
a collision in which no kinetic energy is lost
particle energy KMT assumptions
temp is a measure of the average kinetic energy of the particles
temperature
a measure of the average kinetic energy of the particles in a sample of matter
pressure
force per unit area
barometer
an instrument used to measure atmospheric pressure
atmosphere unit of pressure
one atmosphere is equal to 760 mmhg or 760 torr or 101.3 kilopascals
dalton’s law of partial pressure
the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture
boyle’s law
states that the volume of a fixed amount of gas held at a constant temp, varies inversely with the pressure
absolute zero
represents the lowest possible theoretical temp
charle’s law
the volume of a given amount of gas is directly proportional to its kelvin temp at a constant pressure
gas lussac’s law
the pressure of a fixed amount of gas varies directly with the kelvin temp. when the volume remains constant
combined gas law
the relationship among pressure, temp, and volume
avogadro’s principle
equal volumes of gases at the same temp and pressure contain equal numbers of particles
molar volume
of a gas is the volume 1 mol occupies at 0.0 degrees celsius and 1 atm of pressure
standard temp and pressure (STP)
t= 0.0 degrees celsius (273)
p= 1 atm
1 mol of gas = 22.4L
standard room conditions (SRC)
t= 25.0 degrees celsius (298)
p= 1 atm
1 mol of gas= 24.5L
ideal gas law constant (R)
represented by R and is 0.0821 Lxatm/molxk when pressure is in the atmosphere
ideal gas law
describes the physical behavior of an ideal gas in terms of the pressure, volume, temp, and number of moles of gas present