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31 Cards in this Set
- Front
- Back
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rate law forward
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k[R1][R2] - det experimentally
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factors affecting rxn rate
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T, [reactant], medium, catalysts (take rxn to equil but do not change equil b/c equally fast fwd and reverse rxn)
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P, V and moles (Le Chatlier's)
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inc P or dec V = favor side w/ fewer moles gas
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Rxn orders
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sum of exponents in rate law (can have fractional, mixed order rxn)
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K = 1, K >1, K<1
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equal P and R, more P, more R
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enthalpy
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measure of heat change at constant pressure
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(standard) enthalpy of rxn
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sum Hprod - sum Hreact (at standard conditions - b/c Hf element = 0)
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standard heat of formation
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Hf = characteristic of compound formed from elem in standard state b/c Hf element = 0
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Hess's Law
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enthalpies of rxn are addititive (manipulate steps to get net rxn (mult coeff = mult enthalpies) + switch direc of rxn = switch sign of H)
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Bond dissociation energy related to enthalpy
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can give E of formation of compound (intermed steps); ∆Hrxn = Bonds Broken - Bonds Formed
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Entropy
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∆S = Q/T (greater entropy = greater disorder), ∆Suniv = ∆Ssystem + ∆Ssurround = > or = (if equil) 0
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Gibbs free E
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∆G = ∆H - T∆S, (if neg, indicates max amt W can be done b/c in J)
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heat capacity
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specific heat c * mass
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specific heat and amt heat transfer (relation)
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higher = higher per 1 degree inc
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What forms faster - more KN or TD stable product?
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KN b/c lower Ea, but if T high enough + molec has enough E, will pref TD product
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acetylene structure
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ethyne! C2H2
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enthalpy, entropy, and free energy are all __ functions
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state functions - path independent
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1 atm = ___ torr/mm Hg
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760
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Ideal Gas Assumptions
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no IMF, elastic collissions, molec no vol, high T, low P
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Van-der-Waals eq for real gasses (actual P and V are ___)
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(P+an^2/v^2)(V-nb) = nrt ; actual P less, V more
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Dalton's Law of Partial Pressures
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Pa = XaPt
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Kinetic Molecular Theory of Gas says
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properties of whole gas dependent on motion of individ particles
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Kinetic Molec Theory Assumptions
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no IMF, KE for all gasses same at same T, elastic, continuous motion, particles = 0 vol
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Avg Molec Speed
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KE = 3/2kT (k = boltman's) = for 1 particle!!
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RMS speed of a Gas
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Sq Rt (3RT/MM)
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Rate of Effusion and Diffusion equations
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Sq Rt (inverse of MM's) set up ratio of RMS + cancel numerator
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3 types of cubic unit cells (make up crystals)
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simple cube, body cube (1 more molec in middle) , face-centered cube (1 more molec per side)
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Characteristics of Ionic structures
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poor e- conduc in solid, strong IMF = immobile (metallic strucutres - strong covalent bonds)
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Freezing pt, Boiling pt effect by solute molecs + equation (quant)
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change = Kf or Kb*m (molality) (fp goes down, bp goes up)
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Eq for Osmotic Pressure
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P = MRT (more solute = > p b/c M = molarity)
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Raoult's Law
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VP dec as # solutes inc: Pa=Pao*Xa (solute or solvent) - only for ideal solns where attraction b/w all molecs is the same
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