Gases

Question 1

Pressure

Answer 1

Force exerted per unit area

Question 2

Pascal (Pa)

Answer 2

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

Question 3

Bar (b)

Answer 3

Unit of pressure; 1 bar = 100,000 Pa

Question 4

Pounds per Square Inch (psi)

Answer 4

Unit of pressure common in the US

Question 5

Atmosphere (atm)

Answer 5

Unit of pressure; 1 atm = 101,325 Pa

Question 6

Barometer

Answer 6

device used to measure atmospheric pressure

Question 7

Torr

Answer 7

Unit of pressure; 1 torr = 1/760 atm

Question 8

Hydrostatic Pressure

Answer 8

Pressure exerted by a fluid due to gravity

Question 9

Manometer

Answer 9

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

Question 10

Amonton’s Law (Gay-Lussac’s Law)

Answer 10

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

Question 11

Absolute Zero

Answer 11

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

Question 12

Charles’s Law

Answer 12

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

Question 13

Boyle’s Law

Answer 13

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

Question 14

Avogardro’s Law

Answer 14

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

Question 15

Ideal Gas Law

Answer 15

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

Question 16

Ideal Gas Content (R)

Answer 16

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

Question 17

Ideal Gas

Answer 17

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

Question 18

Standard Conditions of Temperature and Pressure (STP)

Answer 18

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

Question 19

Standard Molar Volume

Answer 19

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

Question 20

Partial Pressure

Answer 20

Pressure exerted by an individual gas in a mixture

Question 21

Dalton’s Law of Partial Pressures

Answer 21

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

Question 22

Mole Fraction (X)

Answer 22

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

Question 23

Vapor Pressure of Water

Answer 23

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

Question 24

Mean Free Path

Answer 24

Average distance a molecule travels between collisions

Question 25

Diffusion

Answer 25

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)

Question 26

Rate of Diffusion

Answer 26

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

Question 27

Effusion

Answer 27

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

Question 28

Graham's Law of Effusion

Answer 28

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

Question 29

Kinetic Molecular Theory (KMT)

Answer 29

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

Question 30

Root Mean Square Speed

Answer 30

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

Question 31

Compressibility Factor (Z)

Answer 31

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

Question 32

Van der Waals Equation

Answer 32

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