question

Boyle's Law

answer

P1V1=P2V2

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Charles' Law

answer

V1/T1=V2/T2

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Combined Gas Law

answer

P1V1/T1=P2V2/T2

question

Avogadro's Law

answer

At the same temperature and pressure, equal volumes of all gases contain the same number of molecules.

question

Standard Molar Volume

answer

22.4 L -- One mole of an ideal gas occupies 22.4 L at 0C and 1 atm of pressure.

question

Ideal Gas Equation

answer

PV=nRT

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Dalton's Law of Partial Pressures

answer

The total pressure exerted by a mixture of ideal gases is the sum of the partial pressures of those gases.

question

Vapor Pressure

answer

Pressure exerted by its gaseous molecules in equilibrium with the liquid.

question

Kinetic-Molecular Theory

answer

1. Gases consist of discrete molecules. The individual molecules are very small and far apart relative to their sizes.

2. Gaseous molecules are in continuous, rapid random, straight-line motion with varying velocities.

3. The collisions between gas molecules and with the walls of the container are elastic; the total energy is conserved during a collision.

4. Between collisions, the molecules exert no attractive or repulsive forces on one another; each molecule travels in a straight line with a constant velocity.

question

Root Mean Square

answer

Urms=sq rt(3RT/Mm)

R=8.314 kg m2/s2 K mol

Molar mass, Mm, must be in KG/mol

question

Effusion

answer

Gases exiting through the walls of a container with porous walls.

question

Diffusion

answer

The movement of a substance into a space or the mixing of one substance with another.

question

Ratio of Rate of Effusion

answer

R1/R2=sqrt(M2/M1) OR (D2/D1)

question

Deviations from Ideality

answer

When molecules become close together through increased T or P -- intermolecular forces become important.

question

Miscible Liquids

answer

Diffuse into each other; they are soluble in each other and form homogeneous solutions.

question

Intermolecular Forces

answer

Forces between (among) individual particles (atoms, ions, molecules).

question

Ion-Ion Interactions

answer

Force of attraction between two oppositely charged ions is governed by Coulomb's Law:

F=abs(q1q2)/r2

F=magnitude of force
r=distance in m
q1,q2=charges on bodies (coulombs)

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Intermolecular Interaction Strengths

answer

I-I>HB>D-D>>LF

question

Dipole-Dipole

answer

Occur between the + end of one polar molecule and the - end of the other.

question

Hydrogen Bonding

answer

Especially strong D-D interaction. Occurs between an H atom in one molecule (attached to an F, O, or N), and an F, O, or N atom in another molecule.

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Dispersion Forces (London Forces)

answer

Present in all substances. ONLY kind of interactions for nonpolar substances. Result from the attraction of the nucleus of one atom for the electron cloud of another atom (in a different molecule). They increase with increasing polarizability, the ability of an electron cloud to be distorted. Polarizability increases with increasing numbers of electrons and therefore with increasing sizes of molecules.

question

Ion-Dipole Interactions

answer

Ion and Dipole. Weaker than Dipole-Dipole.

question

Change in EN

answer

Nonpolar: 0-0.5
Polar: 0.5-2.0
Ionic: > 2.0

question

Viscosity

answer

Resistance to flow. One measure of the forces of attraction within a liquid. Honey = high viscosity; gasoline = low viscosity.

question

Surface Tension

answer

Measure of the inward forces that must be overcome to expand the surface of a liquid. Molecules on the surface are attracted only toward the interior, while those on the interior are attracted equally in all directions.

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Capillary Action

answer

Capillary Rise: Adhesive Forces > Cohesive Forces
Capillary Fall: Cohesive Forces > Adhesive Forces

question

Evaporation

answer

Process by which molecules escape from the surface of a liquid (vaporize). Occurs more rapidly as temperature increases because a greater fraction of molecules possess the necessary escape velocity and kinetic energy.

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LeChatelier's Principle

answer

A system at equilibrium, or changing toward equilibrium, responds in the way that tends to relieve or "undo" any stress placed on it.

question

Vapor Pressure

answer

Pressure exerted by the vapor of the liquid on its surface at equilibrium in a closed container. Because vapor pressures increase as temperature increases, evaporation occurs more rapidly as T increases.

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Boiling Point

answer

Temperature at which the vapor pressure of the liquid equals the applied (usually atmospheric) pressure.

question

Distillation

answer

Process by which a mixture or solution is separated into its components on the basis of differences in BPs of the components.

question

Specific Heat

answer

Amount of heat required to raise the T of 1g of a substance 1C with no change in state.

Q=mC(change in T)

question

Molar Heat Capacity

answer

Amount of heat required to raise the temperature of 1 mol of a substance 1C with no change in state.

Q=mol x molar heat capacity x change in T

question

Heat of Vaporization

answer

Amount of heat that must be absorbed to convert 1g of a liquid at its BP to a gas with no change in temperature. Usually J/g.

question

Heat of Condensation

answer

Reverse of Heat of Vaporization. Amount of heat that must be released to liquefy 1g of a gas at its condensation (BP) with no change in T.

question

Molar Heat of Vaporization

answer

The amount of heat that must be absorbed to convert one mole of a liquid at its BP to a gas with no change in T.

question

Molar Heat of Condensation

answer

Reverse of molar heat of vaporization.

question

Melting Point

answer

Temperature at which liquid and solid coexist at equilibrium under a pressure of 1 atm.

question

Heat of Fusion

answer

The amount of heat required to melt 1g of a solid at its melting point with no change in T. Endothermic.

question

Heat of Crystallization

answer

Amount of heat liberated by the crystallization of one gram of liquid at its freezing point. Exothermic.

question

Specific Heat of Water

answer

4.18 J/gC

question

Density of Water

answer

1.00 g/mL

question

Specific Heat of Ice

answer

2.09 J/gC

question

Sublimation

answer

Conversion of a solid directly into vapor. Dry Ice is solid CO2. The white vapors are due to water condensing in the very cold gaseous CO2 near the solid.

question

Deposition

answer

Vapor directly to solid.

question

Triple Point

answer

Point at which three phases of a substance can coexist in equilibrium.

question

Critical Temperature

answer

Temperature above which a gas cannot be liquefied, i.e., the temperature above which the liquid and gas do not exist as distinct phases.

question

Amorphous Solids

answer

Have no well-defined ordered structure. Waxes, asphalt, and glass.

question

Critical Pressure

answer

Pressure required to liquefy a gas at its critical temperature.

question

Critical Point

answer

The combination of critical temperature and critical pressure.

question

Metallic Solids

answer

Metals.

question

Ionic Solids

answer

Consist of positive and negative ions arranged in a definite crystal structure. Attractions between oppositely charged ions are strong.

question

Molecular Solids

answer

Consist of discrete molecules that occupy positions in unit cells. Intermolecular forces are relatively weak. London Forces and D-D.

question

Covalent Solids

answer

Individual atoms are covalently bonded to several other atoms; thus they are very hard with very high melting points. Diamond, graphite, SO2 (sand), SiC.

Molecular less than Metallic less than Ionic less than Covalent

question

Two major factors affect dissolution of solutes

answer

Enthalpy and Entropy

question

Crystal Lattice Energy

answer

Measure of attractive forces among particles of a solid. Increases as the charges on ions increase. The higher the CLE, the stronger the bond.

question

Enthalpy

answer

Change of energy content of solution (ChangeHsoln). If change Hsoln is exothermic (<0), dissolution is favored. -changeH

question

Entropy

answer

Change in disorder (randomness( of the solution. ChangeSmixing.

NaCl --> Na+ + Cl- increasing entropy +changeS

question

Molality

answer

mol solute/kg solvent

question

Molarity

answer

mol solute/L solution

question

Mole Fraction

answer

Xa=(# mols of A)/(# mols of A + # mols of B)

question

Percent by Mass

answer

g solute/100 g solution

Chem 1212: Chapters 12-14 – Flashcards

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