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AP Chem > Gas and Solution Vocab > Flashcards

Gas and Solution Vocab Flashcards

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1
Q

Acid rain

A

a result of air pollution by sulfur dioxide

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2
Q

Air pollution

A

= contamination of the atomosphere, mainly by the gaseous products of transportation and
production of electricity

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3
Q

atmosphere

A

= the mixture of gases that surrounds the earth’s surface

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4
Q

avagadro’s law

A

= equal volume of gasses at the same temperature and pressure contain the same
number of particles

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5
Q

Barometer

A

a device for measuring atmospheric pressure

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6
Q

Boyle’s law

A

= the volume of a given sample of gas at constant temperature varies inversely with the
pressure

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7
Q

Charl’es Law

A

= the volume of a given sample of gas at constant pressure is directly proportional to the
temperature in kelvins

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8
Q

Coagulation

A

= the destruction of a colloid by causing particles to aggregate and settle out

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9
Q

Colligative properties

A

= properties of a solution that depend only on the number, and not on the
identity, of the solute particles

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10
Q

Colloid

A

a suspension of particles in a dispersing medium

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11
Q

Dalton’s law of partial pressure

A

= 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

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12
Q

Desalination

A

the removal of dissolved salts from an aqueous solution

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13
Q

Dialysis

A

a phenomenon in which a semipermeable membrane allows transfer of both solvent
molecules and small solute molecules and ions

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14
Q

Diffusion

A

= the mixing of gases

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15
Q

Effusion

A

the passage of a gas through a tiny orifice into an evaluated chamber

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16
Q

Graham’s Law of Effusion

A

the rate of effusion of a gas is inversely proportional to the square root of the
mass of its particles

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17
Q

Heat of hydration

A

= 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

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18
Q

Heat of solution

A

= 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

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19
Q

Henry’s law

A

= the amount of a gas dissolved in a solution is directly proportional to the pressure of the
gas above the solution

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20
Q

Ideal gas law

A

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

21
Q

Ideal Solution

A

a solution whose vapor pressure is directly pro-portional to the mole fraction of solvent
present

22
Q

Ion paring

A

a phenomenon occurring in solution when oppositely charged ions aggregate and behave as a single particle

23
Q

Isotonic solutions

A

solutions having identical osmotic pressure

24
Q

Kinetic Molecular Theory (KTM)

A

a model that assumes that an ideal gas is composed of tiny particles
(molecules) in constant motion.

25
Q

Manometer

A

A device for measuring the pressure of a gas in a container

26
Q

Millimeters of mercury

A

a unit of pressure, also called a torr, 760 mm Hg = 760 torr = 101,325
Pa = 1 standard atmosphere.

27
Q

Molal boiling point elevation constant

A

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

28
Q

Molal freezing point elevation constant

A

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

29
Q

Molality

A

the number of moles of solute per kilogram of solvent in a solution (n/kg)

30
Q

Molar Volume

A

the volume of one mole on an ideal gas; equal to 22,4 liters at STP

31
Q

Mole Fraction

A

the ration of the number of moles of a given component in a mixture to the total number of moles in the mixture

32
Q

Normality

A

The number of equivalents of a substance dissolved in a liter of solution X Molarity

33
Q

Osmosis

A

the flow of solvent into a solution through a semipermeable membrane

34
Q

Osmotic pressure

A

the pressure that must be applied to a solution to stop osmosis; π = MRT

35
Q

Partial Pressure

A

the independent pressures exerted by different gases in a mixture

36
Q

Pascal

A

= the SI unit of pressure; equal to newtons per meter squared

37
Q

Photochemical smog

A

= air pollution produced by the action of light on oxygen, nitrogen oxides, and
unburned fuel from auto exhaust to form ozone and other pollutants

38
Q

Raolt’s law

A

he vapor pressure of a solution is direclty proportional to the mole fraction of solvent present

39
Q

Reverse Osmosis

A

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

40
Q

Root mean square velocity

A

= the square root of the average of the squares of the individual velocities of
gas particles

41
Q

Semipermeable membrane

A

a membrane that allows solvent but non-solute molecules to pass through

42
Q

Standard atmosphere

A

a unit of pressure equal to 760 mmHg

43
Q

Standard temperature and pressure (STP)

A

= the condition 0°C and 1 atmosphere of pressure

44
Q

Thermal pollution

A

= 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

45
Q

Torr

A

another name for millimeter of mercury (mmHg)

46
Q

Tyndall effect

A

the scattering of light by particles in a suspension

47
Q

Universal gas constant

A

= the combined proportionality constant in the ideal gas law; 0.08206 L · atm/K ·
mol or 8.3145 J/K · mol

48
Q

Van der Waals Equation

A

a mathematical expression for describing the behavior of real gases

49
Q

Van Hoff factor

A

the ratio of moles of particles in solution to moles of solute dissolved

AP Chem (10 decks)

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