a common unit of pressure
measurement; standard atmospheric pressure at sea level is defined as exactly 760 mm Hg
3 of 28
Define the milimeter of mercurcy (mm Hg)
a common
unit of pressure; the millimeter of mercury, also
called a torr, is based on atmospheric pressure
measurements using a mercury barometer
4 of 28
Define a bar
a unit of pressure
5 of 28
State the ideal gas law
a description of how the
volume of a gas is affected by changes in pressure,
temperature, and amount; PV = nRT
6 of 28
Define the gas constant (R)
he constant in the ideal gas
law PV = nRT
7 of 28
Define the standard temperature and pressure (STP)
T = 273.15 K; P = 1 atm
8 of 28
Define standard molar volume
the volume of 1 mol
of a gas at 0°C and 1 atm pressure; 22.414 L
9 of 28
State the Dalton's law of partial pressures
The total
pressure exerted by a mixture of gases in a container at constant V and T is equal to the sum of the pressures exerted by each individual gas in
the container
10 of 28
Define the kinetic-molecular theory
a theory describing
the quantitative behavior of gases
11 of 28
State Graham's law
The rate of effusion of a gas is
inversely proportional to the square root of its
molar mass
12 of 28
Define effusion
the escape of gas molecules through a
tiny hole in a membrane without molecular
collisions
13 of 28
State Van Der Waals equation
a modification of
the ideal gas law that introduces correction
factors to account for the behavior of real gases
14 of 28
Define a primary pollutant
those that enter the environment directly from a source such as vehicle or
industrial emissions
15 of 28
Define a secondary pollutant
formed by the chemical
reaction of a primary pollutant and are not
directly emitted from a source
16 of 28
State the greeenhouse effect
the trapping of heat emitted
from the Earth by gases that absorb infrared
radiation (greenhouse gases)
17 of 28
Define a greenhouse gas
gases that absorb infrared
(IR) radiation
18 of 28
Define Climate Change
occurs as a result of rising
levels of greenhouse gases from human activities
19 of 28
State Boyle's law
V ∝ 1/P or PV = k at constant n and T
20 of 28
State Charle's law
V ∝ T or V>T = k at constant n and P
21 of 28
State Avogadro's law
V ∝ n or V>n = k at constant T and P
22 of 28
State the Ideal Gas Law
V = nRT/P or PV = nRT
23 of 28
State the equation for Standard temperature and pressure (STP) for gases
T = 0 °C P = 1 atm
24 of 28
State the equation for Gas density
d = m/V = PM/RT
25 of 28
State Dalton’s law of partial pressures
Ptotal = P1 + P2 + P3 +.....
where P1, P2,....are the pressures each individual gas would have if it were alone.
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