Chapter 6: Gases and Pressure

Vocabulary practice flashcards covering the kinetic-molecular theory, gas laws (Boyle's, Charles's, Gay-Lussac's, Avogadro's, Ideal, Dalton's), and atmospheric properties.

Kinetic-molecular theory of gases

A theory describing a gas as particles moving randomly and rapidly, where particle size is small compared to space, no attractive forces exist, and kinetic energy increases with temperature.

Pressure ($P$)

The force ($F$) exerted per unit area ($A$), calculated as $\text{Pressure} = \frac{F}{A}$.

Atmosphere (atm) conversion

$1\text{ atmosphere (atm)}$ is equal to $760.\text{ mm Hg}$, $760.\text{ torr}$, $14.7\text{ psi}$, or $101,325\text{ Pa}$.

Boyle’s law

For a fixed amount of gas at constant temperature, the pressure and volume of the gas are inversely related: $P \times V = k$ or $P_1V_1 = P_2V_2$.

Charles’s law

For a fixed amount of gas at constant pressure, the volume of the gas is proportional to its Kelvin temperature: $\frac{V}{T} = k$ or $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.

Gay–Lussac’s law

For a fixed amount of gas at constant volume, the pressure of a gas is proportional to its Kelvin temperature: $\frac{P}{T} = k$ or $\frac{P_1}{T_1} = \frac{P_2}{T_2}$.

Combined gas law

An equation that combines Boyle's, Charles's, and Gay-Lussac's laws to show the relationship between $P$, $V$, and $T$: $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$.

Avogadro’s law

At constant pressure and temperature, the volume of a gas is proportional to the number of moles ($n$) present: $\frac{V}{n} = k$ or $\frac{V_1}{n_1} = \frac{V_2}{n_2}$.

STP

Standard conditions of temperature and pressure, defined as $1\text{ atm}$ ($760\text{ mm Hg}$) for pressure and $273\text{ K}$ ($0\text{ }^\text{o}\text{C}$) for temperature.

Standard molar volume

The volume of $22.4\text{ L}$ occupied by $1\text{ mole}$ of any gas at STP.

Ideal gas law

A single equation that combines pressure, volume, moles, and temperature: $PV = nRT$.

Universal gas constant ($R$)

A constant used in the ideal gas law; its value is $0.0821\text{ L} \times \text{atm} / (\text{mol} \times \text{K})$ for atm or $62.4\text{ L} \times \text{mm Hg} / (\text{mol} \times \text{K})$ for mm Hg.

Dalton’s law

States that the total pressure ($P_{\text{total}}$) of a gas mixture is the sum of the partial pressures of its component gases: $P_{\text{total}} = P_A + P_B + P_C$.

Ozone ($O_3$)

A gas formed in the upper atmosphere from $O_2$ and $O$ that acts as a shield by absorbing destructive ultraviolet radiation.

Global warming

An increase in the average temperature of the earth's atmosphere, contributed to by greenhouse gases like $CO_2$ which absorb thermal energy.