(a).G=H-T·S,△G=△H-T·△s,△G°=△H°-T·△S° (b). AG is strongly temperature dependent; (AH and AS are not strongly affected by t) (c). Using△G(△OT4G°") to predict changes:△G>0÷ spontaneous;△G=0 equilibrium; AG <0- non-spontaneous (d). Qualitative estimation of reaction direction(by signs of AH and AS) △H<0,△S>0→ spontaneous@all △H>0,△S<0→non- spontaneous@lT △H<0,△S<0→ spontaneous@lowT(T<△HAs) △H>0,△S>0→ spontaneous@ high T(T>△H△S (e). Calculation of△G298K:△G298K°=∑(△Gr,298K° products)-∑(△Gf,298K° reactants) (f). Calculation of△Gr°:△G°r=△H°298K-T·△S298K,( assume△H,△ S are not ependent) (g). Calculation of△ g from△G°:△Gr=△G"r+ R. Q,(Q=[ products]/ reactants]) 9. 12. Thermodynamics Third Law: for all materials, SoK=0 10. Chemical Equilibrium( Chapter 14, 17) 3 classes 10. 1. Introduction to chemical equilibrium 10. 2. Equilibrium constants(K)-K only depends on temperature 10.3. Calculations involving equilibrium Set up the chemical equation with "ICE(initial, change, and equilibrium concentrations, pressures, or moles, then solve the equation ofK 10.4. Relationship between K and△G°r:△Gr=- RTIn K 10.5. Predict the reaction direction by comparing the magnitude of Q and K:(Q<K, Q>K) 10.6. Hess law for Ag and K Multiple ionic equilibria in solution(using Hess Law to find out combination Pay attention to K: e.g. if (reaction 1)=2*(reaction 2)-3*(reaction 3) →△G1=2*△G2-3*△G3.K1=K2/K3 10.7. Shift of equilibrium (a). Qualitatively, use Le Chatelier's principle to predict the shift direction (b). Quantitatively, set up"ICE"equation to solve the equation ofk (c). Change of K with T: In(K2/K1=-AH/[R(1/T2-1TDI 10.8. Learn how to plot Concentration- Time graphs 11. Chemical Kinetics( Chapter 18) 3 classes 11.1. Rates of Reactions. Rate and concentration v=△c/At=dC/dt for aa+bb dd:v=-dA/adt=-dB/b t=dD/ddt 112. Rate laws How to find rate laws based on reactants ' concentrations and reaction rates Differential rate laws:v=k·[AP·[B Integrated rate laws: C-t(a)．G = H – T ∙ S, ΔG = ΔH – T ∙ ΔS, ΔGo = ΔHo – T ∙ ΔS o (b)．ΔG is strongly temperature dependent; (ΔH and ΔS are not strongly affected by T) (c)．Using ΔG (NOT ΔGo !!) to predict changes: ΔG > 0 → spontaneous; ΔG = 0 → equilibrium; ΔG < 0 → non-spontaneous (d)．Qualitative estimation of reaction direction (by signs of ΔH and ΔS)  ΔH < 0, ΔS > 0 → spontaneous @ all T  ΔH > 0, ΔS < 0 → non-spontaneous @ all T  ΔH < 0, ΔS < 0 → spontaneous @ low T (T < ΔH/ΔS)  ΔH > 0, ΔS > 0 → spontaneous @ high T (T > ΔH/ΔS) (e)．Calculation of ΔG298Ko : ΔG298Ko = ∑ (ΔGf, 298Ko products) – ∑(ΔGf, 298Ko reactants) (f)．Calculation of ΔGT o : ΔGo T = ΔHo 298K – T ∙ ΔS o 298K , (assume ΔH, ΔS are not temperature dependent) (g)．Calculation of ΔG from ΔGo : ΔGT =ΔGo T + R∙T∙ln Q , (Q = [products] / [reactants]) 9.12．Thermodynamics Third Law: for all materials, S0K = 0 10．Chemical Equilibrium (Chapter 14, 17) 3 classes 10.1．Introduction to chemical equilibrium 10.2．Equilibrium constants (K) – K only depends on temperature! 10.3．Calculations involving equilibrium  Set up the chemical equation with “ICE” (initial, change, and equilibrium) concentrations, pressures, or moles, then solve the equation of K. 10.4．Relationship between K and ΔGo T: ΔGo T = – R∙T∙ln K 10.5．Predict the reaction direction by comparing the magnitude of Q and K: (Q < K, Q > K) 10.6．Hess law for ΔG and K  Multiple ionic equilibria in solution (using Hess Law to find out combination coefficients)  Pay attention to K: e.g. if (reaction 1) = 2 * (reaction 2) – 3 * (reaction 3) → ΔG1 = 2 *ΔG2 – 3 *ΔG3, K1 = K2 2 / K3 3 10.7．Shift of equilibrium (a)．Qualitatively, use Le Châtelier’s principle to predict the shift direction (b)．Quantitatively, set up “ICE” equation to solve the equation of K. (c)．Change of K with T: ln (K2/K1) = – ΔHo / [R (1/T2 – 1/T1)] 10.8．Learn how to plot Concentration ~ Time graphs 11．Chemical Kinetics (Chapter 18) 3 classes 11.1．Rates of Reactions, Rate and concentration  v = Δc/Δt = dC/dt  for aA + bB → dD: v = – dA/a∙dt = – dB/b∙dt = dD/d∙dt 11.2．Rate laws  How to find rate laws based on reactants’ concentrations and reaction rates  Differential rate laws: v = k ∙ [A]m ∙ [B]n  Integrated rate laws: C ~ t