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Gen Chem > Gases > Flashcards

Gases Flashcards

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1
Q

Pressure

A

Force exerted per unit area

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2
Q

Pascal (Pa)

A

SI unit of pressure; 1 Pa = 1 N/m^2

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3
Q

Bar (b)

A

Unit of pressure; 1 bar = 100,000 Pa

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4
Q

Pounds per Square Inch (psi)

A

Unit of pressure common in the US

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5
Q

Atmosphere (atm)

A

Unit of pressure; 1 atm = 101,325 Pa

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6
Q

Barometer

A

device used to measure atmospheric pressure

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7
Q

Torr

A

Unit of pressure; 1 torr = 1/760 atm

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8
Q

Hydrostatic Pressure

A

Pressure exerted by a fluid due to gravity

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9
Q

Manometer

A

Device used to measure the pressure of a gas trapped in a container

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10
Q

Amonton’s Law (Gay-Lussac’s Law)

A

Pressure of a given number of moles of gas is directly proportional to its kelvin temperature when the volume is held constant

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11
Q

Absolute Zero

A

Temperature at which the volume of a gas would be zero according to Charles’s law

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12
Q

Charles’s Law

A

Volume of a given number of moles of gas is directly proportional to its kelvin temperature when the pressure is held constant

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13
Q

Boyle’s Law

A

Volume of a given number of moles of gas held at constant temperature is inversely proportional to the pressure under which it is measured

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14
Q

Avogardro’s Law

A

Volume of a gas at constant temperature and pressure is proportional to the number of gas molecules

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15
Q

Ideal Gas Law

A

Relation between the pressure, volume, amount, and temperature of a gas under conditions derived by combination of the simple gas laws

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16
Q

Ideal Gas Content (R)

A

Constant derived from the ideal gas equation R = 0.08206 L atm mol^-1K^-1 or 8.314 L kPa mol^-1K^-1

17
Q

Ideal Gas

A

Hypothetical gas whose physical properties are perfectly described by the gas laws

18
Q

Standard Conditions of Temperature and Pressure (STP)

A

273.15 K (0*C) and 1 atm (101.325 kPa)

19
Q

Standard Molar Volume

A

Volume of 1 mole of gas at STP, approximately 22.4 L for gases behaving ideally

20
Q

Partial Pressure

A

Pressure exerted by an individual gas in a mixture

21
Q

Dalton’s Law of Partial Pressures

A

Total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the component gases

22
Q

Mole Fraction (X)

A

Concentration unit defined as the ratio of the molar amount of a mixture component to the total number of moles of all mixture components

23
Q

Vapor Pressure of Water

A

Pressure exerted by water vapor in equilibrium with liquid water in a closed container at a specific temperature

24
Q

Mean Free Path

A

Average distance a molecule travels between collisions

25
Q

Diffusion

A

Movement of an atom or molecule from a region of relatively high concentration to one of relatively low concentration (discussed in this chapter with regard to gaseous species, but applicable to species in any phase)

26
Q

Rate of Diffusion

A

Amount of gas diffusing (through a given area over a given time)

27
Q

Effusion

A

Transfer of gaseous atoms or molecules from a container to a vacuum through very small openings

28
Q

Graham’s Law of Effusion

A

Rates of diffusion and effusion of gases are inversely proportional to the square roots of their molecular masses

29
Q

Kinetic Molecular Theory (KMT)

A

Theory based on simple principles and assumptions that effectively explains ideal gas behavior

30
Q

Root Mean Square Speed

A

Measure of average speed for a group of particles calculated as the square root of the average squared speed

31
Q

Compressibility Factor (Z)

A

Ratio of the experimentally measured molar volume for a gas to its molar volume as computed from the ideal gas equation

32
Q

Van der Waals Equation

A

Modified version of the ideal gas equation containing additional terms to account for non-ideal gas behavior

Gen Chem (10 decks)

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