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Chem 101 > Chapter 12 > Flashcards

Chapter 12 Flashcards

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1
Q

Absolute zero

A

The zero point on the absolute temperature scale; -273.15ºC or 0ºK; theoretically, the temperature at which molecular motion is a minimum

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2
Q

Atmosphere (atm)

A

A unit of pressure; the pressure that will support a column of mercury 760 mm high at 0ºC; 760 torr

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3
Q

Avogadro’s Law

A

At the same temperature and pressure, equal volumes of all gases contain the same number of molecules

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4
Q

Bar

A

A unit of pressure; 1.00 bar is equal to 100. kPa (or 0.987 atm)

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5
Q

Barometer

A

A device for measuring atmospheric pressure. The liquid is usually mercury.

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6
Q

Boyle’s Law

A

At constant temperature, the volume occupied by a given mass of a gas is inversely proportional to the applied pressure

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7
Q

Charles’s Law

A

At constant pressure, the volume occupied by a definite mass of a gas is directly proportional to its absolute temperature

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8
Q

Condensed states

A

The solid and liquid states

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9
Q

Dalton’s Law of Partial Pressures

A

The total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases

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10
Q

Diffusion

A

The movement of a substance (e.g., a gas) into a space or the mixing of one substance (e.g., a gas) with another

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11
Q

Dispersion forces

A

Weak, short-range attractive forces between short-lived temporary dipoles

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12
Q

Effusion

A

The escape of a gas through a tiny hole or a thin porous wall

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13
Q

Fluids

A

Substances that flow freely; gases and liquids

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14
Q

Gay-Lussac’s Law of Combining Volumes

A

At constant temperature and pressure, the volumes of reacting gases (and any gaseous products) can be expressed as ratios of small whole numbers

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15
Q

Ideal gas

A

A hypothetical gas that obeys exactly all postulates of the kinetic-molecular theory

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16
Q

Ideal Gas Equation

A

The product of the pressure and volume of an ideal gas is directly proportional to the number of moles of the gas and the absolute temperature

17
Q

Kinetic-molecular theory

A

A theory that attempts to explain macroscopic observations on gases in microscopic or molecular terms

18
Q

Manometer

A

A two-armed barometer

19
Q

Mole fraction

A

The number of moles of a component of a mixture divided by the total number of moles in the mixture

20
Q

Partial pressure

A

The pressure exerted by one gas in a mixture of gases

21
Q

Pascal (Pa)

A

The SI unit of pressure; it is defined as the pressure exerted by a force of one newton acting on an area of one square meter

22
Q

Pressure

A

Force per unit area

23
Q

Real gases

A

Gases that deviate from ideal gas behavior

24
Q

Root-mean-square speed, 𝓊rms

A

The square root of the mean-square speed, sqrt(u2). This is equal to sqrt(3RT/M) for an ideal gas. The root-mean-square speed is slightly different from the average speed, but the two quantities are proportional.

25
Q

Standard molar volume

A

The volume occupied by one mole of an ideal gas under standard conditions; 22.414 liters

26
Q

Standard temperature and pressure (STP)

A

Standard temperature (0ºC (273.15 K), and standard pressure, one atmosphere, are standard conditions for gases.

27
Q

Torr

A

A unit of pressure; the pressure that will support a column of mercury 1 mm high at 0ºC

28
Q

Universal gas constant

A

R, the proportionality constant in the ideal gas equation, PV=nRT

29
Q

van der Waals equation

A

An equation of state that extendes the ideal gas law to real gases by inclusion of two emperically dtermined parameters, which are different for different gases

30
Q

Vapor

A

A gas formed by boiling or evaporation of a liquid or sublimination of a solid; a term commonly used when some of the liquid or solid remains in contact with the gas

31
Q

Vapor pressure

A

The pressure exerted by a vapor in equilibrium with its liquid or solid

Chem 101 (13 decks)

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