Exam 2 NoteCard

# Exam 2 NoteCard - If Q = 1 = equilibrium If Q> 1 = rnx...

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Kinetics: Factors that Influence Reaction Rate: Temp, Conc, Catalyst, Particle Size Rate of Rnx: rate (mol/L*T) = ΔConc / ΔTime aA = dD rate = -1/a Δ[A]/ ΔTime = 1/d Δ[D] / ΔTime Rate Law: rate = k [A] x [B] y 0 th Order Rnx: rate = k [A] 0 = k Δ[A]/ ΔTime = -k[A] [A] 0 – [A] = -kt 1 st Order Rnx: rate = k [A] 1 = k[A] Δ[A]/ ΔTime = -k[A] ln([A] 0 / [A])= -kt 2 nd Order Rnx: rate = k [A] 2 Δ[A]/ ΔTime = -k[A] 2 (1/[A]) – (1/[A] 0 ) = kt Units: rate = mol/L*Time [A] = mol/L or M 0 th = mol/L*Time 1 st = Time -1 2 nd = L/mol*Time Half Life: T 1/2 = 0.693 / k Arrhenious Equation = Activation Energy: ln(k 1 /k 2 ) = -Ea/R (1/T 1 – 1/T 2 ) Ea = J / mol Equilibrium: Equilibrium Expression: K eq = [products] / [reactants] If K < 1 = reactant favored If K > 1 = product favored K = Molarity 2 Reaction Quotient: When NOT at an equilibrium If Q < 1 = rnx goes left
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Unformatted text preview: If Q = 1 = equilibrium If Q > 1 = rnx goes right K c Expressions: K c = [products] / [reactants] K p Expressions: K p = P(products) / P(reactants) P = [C] RT = K c (RT) n n = change in moles of gas Disturbing Equilibriums: Rise T = shift in endothermic = change in k Drop T = shift in exothermic = change in k Add React. = shift right = no k change Add Prod = shift left = no k change Disturbing Equilibriums (Gases only): Inc. P / Dec. Vol = reduce mols of gas = no k change Dec. P / Inc. Vol = increase mols of gas = no k change Nuclear Chemistry: α Bombarding 14 7 N + 4 2 α → 17 8 O + 1 1 H N Bombarding 98 42 Mo + 1 N → 99 42 Mo + γ R = 8.31447 J/mol*K R = .082057 L*atm/mol*T...
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## This note was uploaded on 04/29/2008 for the course CHEM 104 taught by Professor Tomasik during the Spring '08 term at University of Wisconsin.

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