Gas and Solution Vocab Flashcards
Acid rain
a result of air pollution by sulfur dioxide
Air pollution
= contamination of the atomosphere, mainly by the gaseous products of transportation and
production of electricity
atmosphere
= the mixture of gases that surrounds the earth’s surface
avagadro’s law
= equal volume of gasses at the same temperature and pressure contain the same
number of particles
Barometer
a device for measuring atmospheric pressure
Boyle’s law
= the volume of a given sample of gas at constant temperature varies inversely with the
pressure
Charl’es Law
= the volume of a given sample of gas at constant pressure is directly proportional to the
temperature in kelvins
Coagulation
= the destruction of a colloid by causing particles to aggregate and settle out
Colligative properties
= properties of a solution that depend only on the number, and not on the
identity, of the solute particles
Colloid
a suspension of particles in a dispersing medium
Dalton’s law of partial pressure
= 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
Desalination
the removal of dissolved salts from an aqueous solution
Dialysis
a phenomenon in which a semipermeable membrane allows transfer of both solvent
molecules and small solute molecules and ions
Diffusion
= the mixing of gases
Effusion
the passage of a gas through a tiny orifice into an evaluated chamber
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
Heat of hydration
= the enthalpy change associated with placing gaseous molecules or ions in water; the
sum of the energy needed to expand the solvent and the energy released from the solvent-solute
interaction
Heat of solution
= the enthalpy change associated with dissolving a solute in a solvent; the sum of the
energies needed to expand both solvent and solute in a solution and the energy release from the
solvent-solute solution
Henry’s law
= the amount of a gas dissolved in a solution is directly proportional to the pressure of the
gas above the solution
Ideal gas law
an equation of state for a gas, where the state of the gas is its condition at a given time;
this equation expresses behavior approached by real gases at high T and low P
Ideal Solution
a solution whose vapor pressure is directly pro-portional to the mole fraction of solvent
present
Ion paring
a phenomenon occurring in solution when oppositely charged ions aggregate and behave as a single particle
Isotonic solutions
solutions having identical osmotic pressure
Kinetic Molecular Theory (KTM)
a model that assumes that an ideal gas is composed of tiny particles
(molecules) in constant motion.
Manometer
A device for measuring the pressure of a gas in a container
Millimeters of mercury
a unit of pressure, also called a torr, 760 mm Hg = 760 torr = 101,325
Pa = 1 standard atmosphere.
Molal boiling point elevation constant
a constant characteristic of a particular solvent that gives the
change in boiling point as a function of solution molality; used in molecular weight determination
Molal freezing point elevation constant
a constant characteristic of a particular solvent that gives the
change in freezing point as a function of solution molality; used in molecular weight determination
Molality
the number of moles of solute per kilogram of solvent in a solution (n/kg)
Molar Volume
the volume of one mole on an ideal gas; equal to 22,4 liters at STP
Mole Fraction
the ration of the number of moles of a given component in a mixture to the total number of moles in the mixture
Normality
The number of equivalents of a substance dissolved in a liter of solution X Molarity
Osmosis
the flow of solvent into a solution through a semipermeable membrane
Osmotic pressure
the pressure that must be applied to a solution to stop osmosis; π = MRT
Partial Pressure
the independent pressures exerted by different gases in a mixture
Pascal
= the SI unit of pressure; equal to newtons per meter squared
Photochemical smog
= air pollution produced by the action of light on oxygen, nitrogen oxides, and
unburned fuel from auto exhaust to form ozone and other pollutants
Raolt’s law
he vapor pressure of a solution is direclty proportional to the mole fraction of solvent present
Reverse Osmosis
the process occurring when the external pressure on a solution causes a net flow of
solvent through a semi-permeable membrane from the solution to the solvent
Root mean square velocity
= the square root of the average of the squares of the individual velocities of
gas particles
Semipermeable membrane
a membrane that allows solvent but non-solute molecules to pass through
Standard atmosphere
a unit of pressure equal to 760 mmHg
Standard temperature and pressure (STP)
= the condition 0°C and 1 atmosphere of pressure
Thermal pollution
= the oxygen-depleting effect on lakes and rivers of using water for industrial cooling
and returning it to its natural source at a higher temperature
Torr
another name for millimeter of mercury (mmHg)
Tyndall effect
the scattering of light by particles in a suspension
Universal gas constant
= the combined proportionality constant in the ideal gas law; 0.08206 L · atm/K ·
mol or 8.3145 J/K · mol
Van der Waals Equation
a mathematical expression for describing the behavior of real gases
Van Hoff factor
the ratio of moles of particles in solution to moles of solute dissolved
