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60 Cards in this Set
- Front
- Back
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Define Pressure
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Pressure = Force/Area
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Standard Units for: Pressure and Temperature
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Atmospheres (atm) and Kelvin (K)
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Avagadro's law
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V1/n1 = V2/n2
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Boyle's Law
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P1V1 = P2V2
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Charles' Law
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V1/T1 = V2/T2
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What is STP?
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Standard Temperature and Pressure
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Average Kinetic Energy is proportional to what property?
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Temperature: As long as T is constant, AKE is constant
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Effusion
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spread of a gas through a tiny hole into an evacuated space
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Diffusion
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Spread of a substance throughout another substance
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Factors affecting states of matter
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Temperature and Pressure
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List IMF's in decreasing strength
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Ionic Bonding
Ion - Dipole Hydrogen Bonding Dipole-Dipole LDF |
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Hydrogen Bonds are with what other atoms
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O
F N |
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Resistance to Flow
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Viscosity
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Endothermic Phase Changes
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Melting
Evaporation Sublimation |
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Exothermic Phase Changes
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Freezing
Condensation Deposition |
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Dissolved in a substance
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Solute
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Substance dissolved into this
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Solvent
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solution -- solute + solvent
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Crystallization
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solute + solvent -- solution
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dissolution
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three types of solution
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unsaturated
saturated supersaturated |
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mole fraction
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mole solute/mole solution
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ppm
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mass solute/mass solution x 10^6
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molarity
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moles solute/L solution
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molality
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mole solute/kg solvent
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4 colligative properties
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Vapor Pressure
Boiling Point Elevation Freezing Point Depression Osmotic Pressure |
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Vapor Pressure
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VP = (mole fraction)(initial VP)
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Boiling Point Elevation
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T change = (Kb constant)(molality)
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Freezing Point Depression
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T change = (Kf constant)(molality)
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Osmosis
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the movement of concentrated soln to dilute soln through a semi-permeable membrane
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Osmotic Pressure
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Amount of pressure required to prevent osmosis
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Studies the rate of a reaction
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Kinetics
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4 factors affecting rxn rate
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concentration
temperature catalyst physical state |
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slope of reaction rate graph
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rate constant
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general rate law
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rate = k [A]^m [B]^n
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part of rate law not dependent on concentration
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k. rate constant
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overall reaction order
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m + n
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first order graph
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ln [A] vs t
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amount of energy required for a reaction to occur
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activation energy
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Q>K
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reaction favors products, shift left
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Q<K
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reaction favors reactants, shift right
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concentration of reactant increased: where does the reaction shift
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products, right
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temp decreased for endothermic
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left, reactants
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pressure decrease
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side with more moles
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Bronstead Lowry Acid
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proton donor, H+
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Bronstead Lowry Base
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proton acceptor, H+
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Lewis Acid
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Electron pair acceptor
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Lewis Base
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Electron pair donor
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Acid, Base, Conjugate relationships
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A + B --- CB + CA
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7 Strong Acids
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HNO3, HI, HCl, H2SO4, HBr, HClO3, HClO4
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8 Strong Bases
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KOH, LiOH, Ca(OH)2, Sr(OH)2, Cs(OH), NaOH, RbOH, Ba(OH)2
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pH
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- log [H+]
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Henderson Hasselbach
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- log (Ka) + log (base/acid)
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strong base + weak acid
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basic solution
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molar solubility
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x in equilibrium chart
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loss of electrons
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oxidation
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gain of electrons
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reduction
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electrode where reduction takes place
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cathode
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electrode where oxidation takes place
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anode
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electrochemistry cell equation
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Ecell = Ered (reduction) - Ered (oxidation)
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EMF - Concentration Relationship
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dec. react = dec EMF
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