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Chem 2 Exam 1

Chapters 11 and 12

QuestionAnswer
calculating mole fraction want moles/ total moles
Molarity moles solute/ Liter Solution
Molality moles solute/ kg solvent
Ionic usually dissolves only in polar
Colloids when different substances dont mingle
Solutions when different substances comingle
Homogeneous Solutions
Heterogeneous Colloids
Solvent has higher or lower proportion higher
Solute has higher or lower proportion lower
Solutions are in the same state as solvent
Do solutes settle out no never fully
Solute concentration can be varied continuously
Electrolyte strong electrical conductivity, solute ionized when dissolved
Nonelectrolyte solutions that can't conduct electric current because solute cant produce ions
Intermolecular Forces Dispersion, Dipole, Hydrogen, Ion-Dipole
Dispersion occurs in all molecules (nonpolar?)
Dipole Polar
Hydrogen H connect to ONF
Ion Dipole Ion and Polar Molecule
Hess's Law if a reaction is carried out in a series of steps (change in H) for reaction= sum of enthalpy changes
Exothermic produce/give off energy
Endothermic take in/ consume energy
Density formula mass/volume
Predicting Solubility effects of intermolecular forces when dissolving polar use polar etc.
Immiscible Don't mix like oil and water
Miscible form solutions with emulsifier
Emulsifiers add soap to oil/water to mix them
Solubility maximum solute concentration
Solids at higher temp... increased solubility
Gases at higher temp... decreased solubility
solubility at higher pressures... are increased
Mole Fraction moles A/Sum of Moles
Molarity is best when Temp is constant
Molality, Mass%, and mole fraction best when Temp Changing
Density is needed for Molarity
Familiar Solution Properties depend on nature of solute dissolved
Colligative Property depends on concentration of solute not nature of the solute particles
Osmosis selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one
Isotonic concentration of particles equal
Hypotonic concentration of particles lower inside
Hypertonic Concentration of particles higher inside
Enthalpy Change exothermic vs endothermic, final - intial
Thermodynamics tell us direction and extent
Kinetics tell us fast or slow
Kinetic Molecular Theory constant motion that changes direction when bump into another particle
Reaction rates matter of concentration and time
relative rate expressions rates related by stoichiometry
Factors affecting reaciton rates chemical nature, surface area, concentration/pressure, temp, catalyst
Rate laws effect of all reaction concentrations
reaction orders X and Y superscripts, not always whole, must be determined experimentally
Overall Reaction Order X+Y reaction orders
Rate law unit for first order s^-1
Rate law unit for second order M^-1 s^-1
Rate law unit for third order M^-2 s^-1
Rate law unit for zero order M/s
Radioactive decay is the same as half life
Collision factors # collisions/time, Orientation, Collision energy(fast/slow)
Activation Energy minimum amount of e to initiate reaction
reaction rates usually ____ w/ temperature increase
Catalyzed reactions usually _______ reaction rates lower
As Ea increases, what happens to K decreases
As T increases what happens to K increases
Reaction Mechanisms Series of elementary steps
intermediates products of one reactions that are consumed as reactants of another section
Heat of reaction is difference of product and reactants
Determine the activation energy difference between reactants and top barrier
Determine activation energy of reverse reaction difference between products and top barrier
Molecularity prefixes of an elementary reaction Uni, Bi, Ter, Quad
How to find molecularity prefizes add coefficients of reactants
what is the rate determining barrier highest change barrier
Created by: brkolstoe
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