[{"data":1,"prerenderedAt":112},["ShallowReactive",2],{"cheatsheet-chemical-equilibrium":3},{"sheet":4},{"sheetSlug":5,"topicSlugs":6,"primaryTopic":7,"title":8,"subtitle":9,"sections":10},"chemical-equilibrium",[5],21,"Chemical Equilibrium","K expressions, Kp/Kc, the reaction quotient, ICE tables, and Le Chatelier's principle.",[11,23,31,39,47,56,64,97,103],{"heading":12,"kind":13,"items":14},"Equilibrium constant","rules",[15],{"ref":16,"mode":19,"provenance":20,"text":21,"source_hash":22},{"type":17,"topic":7,"id":18,"field":17},"rule","EQ-R001","transform","owned_workbook","Kc = [products]^ν / [reactants]^ν (Kp uses partial pressures). EXCLUDE pure solids and liquids. N₂ + 3H₂ ⇌ 2NH₃: Kc = [NH₃]²/([N₂][H₂]³). For CaCO₃(s) ⇌ CaO(s) + CO₂(g): Kp = P(CO₂).","202d94bf2c46e3c6ccba6ccbd5df53fcd6733a7b2c1fdb77c637d99f72f6adde",{"heading":24,"kind":13,"items":25},"Kp and Kc",[26],{"ref":27,"mode":19,"provenance":20,"text":29,"source_hash":30},{"type":17,"topic":7,"id":28,"field":17},"EQ-R003","Kp = Kc(RT)^Δn, R = 0.0821, T in K, Δn = (mol gas products) − (mol gas reactants), counting gases only. Δn = 0 → Kp = Kc.","05c072f9d3e05843e229a5606b57502cfe3673a579ef6d9d007377b50bd8957c",{"heading":32,"kind":13,"items":33},"Manipulating K",[34],{"ref":35,"mode":19,"provenance":20,"text":37,"source_hash":38},{"type":17,"topic":7,"id":36,"field":17},"EQ-R002","Reverse a reaction → K_rev = 1/K. Add reactions → K_net = K₁·K₂·… Scale all coefficients by x → K_scaled = K^x. Convert moles to molarity (M = mol/V) before substituting.","8b9ca612088609fd811fb593863b7367a07aa6da6bd1d924b4ad23129e22a7d1",{"heading":40,"kind":13,"items":41},"Q vs K direction",[42],{"ref":43,"mode":19,"provenance":20,"text":45,"source_hash":46},{"type":17,"topic":7,"id":44,"field":17},"EQ-R006","Q has K's form with current concentrations. Q \u003C K → shifts right (toward products); Q > K → shifts left; Q = K → at equilibrium.","84209b7e1fe6518e9e385f2add9c4cefc5ab26be7e9483a8571d4574268fa678",{"heading":48,"kind":49,"items":50},"ICE table","steps",[51],{"ref":52,"mode":19,"provenance":20,"text":54,"source_hash":55},{"type":17,"topic":7,"id":53,"field":17},"EQ-R005","Initial / Change (±νx) / Equilibrium rows, then solve K for x. Three paths: perfect square (take √), x-small approximation (valid when K \u003C 10⁻³ or [init] ≫ x; check x \u003C 5%), or the quadratic formula (keep the positive root). Always back-substitute to confirm K.","52781bf831ee6f803254545450e14c126043cefdbf4a0f0526cfea99e612b2f9",{"heading":57,"kind":49,"items":58},"Decomposition from total P",[59],{"ref":60,"mode":19,"provenance":20,"text":62,"source_hash":63},{"type":17,"topic":7,"id":61,"field":17},"EQ-R004","Given only total pressure + product ratio (e.g. NH₄HS(s) ⇌ NH₃ + H₂S, 1:1): write each partial pressure in one unknown, sum to the total, solve, then substitute into Kp.","4adec39445739a78ae7a1bd313b05a6a2dae0d85244797ec2108d726df649edc",{"heading":65,"kind":66,"columns":67,"items":70},"Le Chatelier's principle","data",[68,69],"Stress","Shift",[71],{"ref":72,"mode":19,"provenance":20,"rows":74,"source_hash":96},{"type":17,"topic":7,"id":73,"field":17},"EQ-R007",[75,78,81,84,87,90,93],[76,77],"add reactant / remove product","right",[79,80],"remove reactant / add product","left",[82,83],"V↓ (P↑), Δn ≠ 0","toward fewer moles of gas",[85,86],"V↑ (P↓), Δn ≠ 0","toward more moles of gas",[88,89],"T↑, endothermic","right (K increases)",[91,92],"T↑, exothermic","left (K decreases)",[94,95],"catalyst / inert gas at const V","no shift","a37fd0ffc20e732fe7f6095c27dc1ec1dc7b27596f8d05112f32a0cbf3b1ae1d",{"heading":98,"kind":13,"items":99},"Temperature is special",[100],{"ref":101,"mode":19,"provenance":20,"text":102,"source_hash":96},{"type":17,"topic":7,"id":73,"field":17},"Only temperature changes the value of K. Every other stress leaves K fixed and the system shifts to restore Q = K.",{"heading":104,"kind":13,"items":105},"K magnitude → extent",[106],{"ref":107,"mode":19,"provenance":109,"text":110,"source_hash":111},{"type":17,"topic":7,"id":108,"field":17},"EQ-R008","original","K ≫ 1 (> 10³): products dominate (essentially complete). K ≪ 1 (\u003C 10⁻³): reactants dominate. 10⁻³ ≤ K ≤ 10³: comparable amounts of both. Rule-of-thumb thresholds for extent prediction.","6d068bdd02b11c19586c7f685448db07947a5df0aa1a2fb24089a75a4432ee0a",1787246033411]