CH 101: Quiz #3

Boyle’s Law

P₁V₁ = P₂V₂

Charles’s Law

(V₁/T₁) = (V₂/T₂)

Avogadro’s Law

(V₁/n₁) = (V₂/n₂)

Gay-Lussac’s Law

(P₁/T₁) = (P₂/T₂)

Combined Gas Law

(P₁V₁/T₁) = (P₂V₂/T₂)

Ideal Gas Law

PV=nRT

Kinetic Molecular Theory

• gases consist of molecules in constant, random motion

• pressure arises from collisions with container walls

• no attractive or repulsive forces between molecules, collision are elastic

• volume of molecule is negligible

mole fraction

X_A = (n_i/n_total)

density equation with molar mass

D = (MP/RT)

rate of diffusion equation

(amount of gas passing through an area/unit of time)

rate of effusion equation

(amount of gas transferred/time)

root-mean squared speed

the molecular speed that is inversely proportional to the molecular mass

root-mean squared speed equation

v_rms = (3RT/M)^1/2

melting phase change

solid —> liquid

freezing phase change

liquid —> solid

vaporization phase change

liquid —> gas

condensation phase change

gas —> liquid

sublimation phase change

solid —> gas

deposition

gas —> solid

evaporation

phase change from liquid —> gas at a temperature below the boiling point

vaporization

phase change from liquid —> gas at the boiling point

boiling point

the temperature at which vapor pressure = atmospheric pressure

normal boiling point

temperature at which vapor pressure of a liquid is equal to one atmosphere

triple point

the temperature and pressure at which all 3 states of matter coexist

strong acids

HCl, HBr, HI, HNO₃, HClO₃, HClO₄, H₂SO₄

diffusion

the process by which molecules disperse in space in response to differences in concentration

effusion

the escape of gas molecules through a tiny hole such as a pinhole in a balloon into a vacuum

intramolecular forces

forces holding atoms together to form molecules

intermolecular forces

attractive forces that hold particles together particularly in condensed phases

dipole-dipole interactions

attractive forces between polar molecules

hydrogen bonding

special type of dipole-dipole interaction that occurs only in molecules that contain H bonded to a small, highly electronegative atom like N, O, and F

London-Dispersion Forces

attractive forces that act between all molecules, including non-polar molecules, resulting from the formation of instantaneous dipoles and induced dipoles, also called dispersion forces

ion-dipole interactions

coulombic attractions between ions and polar molecules, interactions occur in mixtures of ionic and polar species

instantaneous dipole

when a molecule has a non-uniform

equilibrium vapor pressure

pressure exerted by the molecules that have escaped to the gas phase once the pressure has stopped increasing

phase diagram

combines plots of pressure vs. temperature for the liquid —> gas, solid —> liquid, and solid —> gas phase transition equilibria of a substance

solution

homogeneous mixture of two or more substances

solvent

component of a solution present at a significantly greater concentration

electrolytes

compounds or substances that when dissolved in water yields ions in a solution

nonelectrolytes

substances that do not yield ions when dissolved in water

strong electrolyte

physical or chemical process that generates the ions is essentially 100% efficient (all of the dissolved compound yields ions)

weak electrolyte

only a relatively small fraction of dissolved substance undergoes the ion-producing process

Arrhenius acid

a substance that produces H⁺ ions when dissolved in water

Arrhenius base

a substance that produces OH^- ions when dissolved in water

solubility

the maximum concentration that may be achieved under given conditions when the dissolution process is at equilibrium

saturated

when a solutes concentration is equal to its solubility

unsaturated

when a solute’s concentration is less than its solubility

dilute

a solution containing a relatively low concentration of solute

concentrated

a solution containing a relatively high concentration

supersaturated

a solution where a solute concentration exceeds its solubility

miscible

liquids mixed in any proportions to yield solutions and have infinite mutual solubility

immiscible

two liquids that do not form a homogeneous mixture when added together

hydration

process by which water molecules surrounding solute particles

Bronsted acid

a substance that donates a proton (H⁺)

Bronsted base

a substance that accepts a proton (H⁺)

conjugate base

an acid donates H⁺ and it reacts as proton acceptor in the reverse reaction

conjugate acid

an acid accepts H⁺ and it reacts as a proton donor in the reverse reaction

neutralization reaction

a reaction between an acid and a base