Gases and the Kinetic Molecular Theory Flashcards

Vocabulary flashcards covering the kinetic molecular theory, gas properties, gas pressure conversions, individual and combined gas laws, ideal gas law calculations, and Dalton's law of partial pressures.

Kinetic Molecular Theory

A theoretical model stating that all particles of matter are in motion at all times.

Ideal Gas

A hypothetical gas whose particles are in constant random motion moving in straight lines, act as point masses (possessing mass but no volume), and experience only perfectly elastic collisions with no intermolecular attractions.

Point Mass

An idealized particle that possesses mass but occupies no physical volume.

Elastic Collision

A collision between gas particles or container walls in which total kinetic energy is conserved.

Real Gas

A gas whose particles possess actual volume and experience intermolecular forces; it deviates from ideal gas behavior at very low temperatures and very high pressures.

Atmospheric Pressure

The force per unit area exerted on the Earth's surface by the weight of a column of air pulled by gravity.

Mercury Barometer

An instrument designed using liquid mercury ($\text{Hg}_{(l)}$) to measure atmospheric pressure based on the height of a mercury column.

Standard Atmospheric Pressure Equivalents

The standard values of pressure defined as $760\text{ mmHg} = 1\text{ atm} = 101.325\text{ kPa}$, along with the conversion $1\text{ bar} = 100\text{ kPa}$.

Boyle's Law

A gas law stating that the volume of a gas varies inversely with pressure at a constant temperature and mass ($P_1 V_1 = P_2 V_2$).

Absolute Zero

The lowest theoretical temperature, equal to $-273.15^\text{o}\text{C}$ or $0\text{ K}$, at which the volume of an ideal gas extrapolates to zero.

Kelvin Scale

An absolute temperature scale suggested by Lord Kelvin where $0\text{ K}$ represents absolute zero; calculated using $T = t + 273.15$.

Charles' Law

A gas law stating that the volume of a gas varies directly with its absolute temperature at a constant pressure and mass ($\frac{V_1}{T_1} = \frac{V_2}{T_2}$).

Combined Gas Law

A gas law that unifies Boyle's Law and Charles' Law into one equation for a fixed mass of gas ($\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$).

STP

Standard Temperature and Pressure, defined as $273.15\text{ K}$ ($0^\text{o}\text{C}$) and $101.325\text{ kPa}$.

SATP

Standard Ambient Temperature and Pressure, defined as $298.15\text{ K}$ ($25^\text{o}\text{C}$) and $100.000\text{ kPa}$.

Law of Combining Volumes

A law formulated by Gay-Lussac stating that, when measured at constant temperature and pressure, the volumes of gaseous reactants and products combine in simple whole-number ratios.

Ideal Gas Law

An equation relating all four gas parameters ($P$, $V$, $n$, and $T$) expressed as $PV = nRT$.

Universal Gas Constant ($R$)

The proportionality constant in the ideal gas equation, equal to $8.314\text{ kPa}\times\text{L}\times\text{mol}^{-1}\times\text{K}^{-1}$.

Dalton's Law of Partial Pressures

A principle stating that the total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of each individual gas ($P_{\text{total}} = P_1 + P_2 + P_3 + \text{...}$).

Viscosity

The resistance of a fluid to flow; gases have low viscosity, allowing them to flow easily and escape rapidly through small openings.

Miscibility

The ability of gases to mix completely and evenly with one another in all proportions.