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r The Master Chemistry Blueprint L r [Ee eel Kinetics & Equilibrium Dynamics (Exam Control Board) “a [> cS FLOW ANALYSIS |~———~_ STABILITY CHECKS => | — (-— : ma none ARRHENIUS “ VARIABLES General Formula: Two-State Ratio: ne) ela) Finding A: Use e~™ from graph. » & A RATE LAW DIAGNOSTICS REACTION ORDER MATRIX - T Finding Order (x) from Initial Rates:||||| grqer| _. Rate & Linear Graph | Half-Life | Specific Integrated Law | (y vs x) (ty/2) k-units A=B* >B=Al* : In(A) _ log(A) [Alo gees ee «qrl Log Trick: x In(B) or log(B) | Rate = k =< : al M : ‘ (Where A = Rate Ratio, [A]; = -kt + [Alo yale: HTT aie B = Concentration Ratio) t over time) Manipulating k-unit neralized): anipulating k-units (Generalized) In(2) 0.693 [M]@-" « s-1 Ae Rate=k[A] |= ae er 2 se In[A}, = -kt + InfAlo| = (Rule: tyois| § Variations to expect on exams: bi j t constant) M"-1 xs 1 Mi-” Rate=KAJ* | — K[Alo s 2nd | ve _i_ = (Rule: ty2 Mt+s" -1, yi-n Alt” A increases s *M [Al [Alo t over time) (Where n = total order) CRITICAL KINETICS R-VALUE: R = 8.314 J/(mol*K) A\ NotebookLM SYSTEM STRESS DIAGNOSTICS (LE CHATELIER) 1. CONCENTRATION (CONSTANT T, V) e Increase Reactant > Shifts Right (->) e Increase Product > Shifts Left (<-) e Decrease Reactant > Shifts Left (<-) e Decrease Product > Shifts Right (->) 2. VOLUME & PRESSURE (CONSTANT T) e Decrease V (Increase P) > Shifts to side with FEWER moles of gas. e Increase V (Decrease P) > Shifts to side with MORE moles of gas. N204(g) <-> 2N02(g) (Colorless to Brown). If P increases, instantaneous concentration of BOTH increases before shifting toward N204. Rule: If delta_n = 0, pressure has no effect. 3. TEMPERATURE (ONLY STRESS THAT CHANGES K VALUE) e Exothermic (delta_H < 0): Heat is a product. Add heat -> Shift Left (<-), K decreases. e Endothermic (delta_H > Q): Heat is a reactant. Add heat -> Shift Right (->), K increases. AX EXAM TRAPS & HAZARDS ICE Tables: If initial > products are unmentioned, assume @. If ALL initial concentrations are provided, | you MUST calculate Q first to find shift direction. od Inert Gases: Adding an inert gas at constant volume produces NO SHIFT in equilibrium. Catalysts: Adding a catalyst reaches equilibrium faster, but causes NO SHIFT in position. The R Constant Trap: >) Kinetics Arrhenius = 8.314 J/(mol#K). Equilibrium Kp/Ke = @.08206 L*atm/(mol*K). 
