[{"data":1,"prerenderedAt":113},["ShallowReactive",2],{"cheatsheet-stoichiometry":3},{"sheet":4},{"sheetSlug":5,"topicSlugs":6,"primaryTopic":7,"title":8,"subtitle":9,"sections":10},"stoichiometry",[5],10,"Stoichiometry","Mole ratios, mass-to-mass, limiting reactant, excess, and percent yield.",[11,23,31,39,48,56,64,72,80,88,96,104],{"heading":12,"kind":13,"items":14},"Balance first","rules",[15],{"ref":16,"mode":19,"provenance":20,"text":21,"source_hash":22},{"type":17,"topic":7,"id":18,"field":17},"rule","BS-R001","transform","owned_workbook","Balance the equation before any calculation. The coefficients are the source of every mole ratio you will use.","1c5ba7881b10a2a3eadfc7f91f3883c3f7a8b27f74110821ceeed6d00bd94622",{"heading":24,"kind":13,"items":25},"Mole ratio (stoichiometric factor)",[26],{"ref":27,"mode":19,"provenance":20,"text":29,"source_hash":30},{"type":17,"topic":7,"id":28,"field":17},"BS-R002","Coefficients give the conversion factor between substances. The factor from A to B is (coefficient of B) / (coefficient of A).","f1c420094b113457c98dd8ba324aa76a210b4b561e5fc2d8ab9e59beeab17e76",{"heading":32,"kind":13,"items":33},"Convert to moles first",[34],{"ref":35,"mode":19,"provenance":20,"text":37,"source_hash":38},{"type":17,"topic":7,"id":36,"field":17},"BS-R003","Anything not in moles must become moles before the ratio: mass ÷ molar mass; gas at STP ÷ 22.4 L/mol; particle count ÷ Nₐ.","6b8d3ea31641443eadcfb647c380253fde4841fa9ea5811e164e5733349d204f",{"heading":40,"kind":41,"items":42},"Mass-to-mass (four steps)","steps",[43],{"ref":44,"mode":19,"provenance":20,"text":46,"source_hash":47},{"type":17,"topic":7,"id":45,"field":17},"BS-R004","mass A → mol A (÷ MM_A) → mol B (× stoichiometric factor) → mass B (× MM_B). Carry units so they cancel.","892b02f0db6984a8a4b4d6df8506723f390c3948c57e7f4698b8f2973e2ba610",{"heading":49,"kind":41,"items":50},"Find the limiting reactant",[51],{"ref":52,"mode":19,"provenance":20,"text":54,"source_hash":55},{"type":17,"topic":7,"id":53,"field":17},"BS-R010","When both reactant amounts are given: convert each to moles, divide each by its coefficient; the smaller quotient is the limiting reactant. (Or compute product from each; the smaller wins.)","620c498b0e99e47bee9ca5e19efad4dba9c04c5ae92a4df6273cfa25d7d27eac",{"heading":57,"kind":13,"items":58},"Use the limiting reactant",[59],{"ref":60,"mode":19,"provenance":20,"text":62,"source_hash":63},{"type":17,"topic":7,"id":61,"field":17},"BS-R011","Compute product from the limiting reactant's moles only (never the excess): × stoichiometric factor × product molar mass.","8fd175e9ef49c0b4949511dcfc5f170dee373a1bc4dcccb5ab75db4d169ee1d4",{"heading":65,"kind":13,"items":66},"Excess reactant remaining",[67],{"ref":68,"mode":19,"provenance":20,"text":70,"source_hash":71},{"type":17,"topic":7,"id":69,"field":17},"BS-R012","Consumed excess = mol LR × (excess coeff / LR coeff) × MM_excess. Remaining = initial excess − consumed. A negative result means the LR was misidentified.","eb9ea1088073c2977a205d3f1e8a0d519d7ede1d26d9fb6d214bf4a86682272b",{"heading":73,"kind":13,"items":74},"Percent yield",[75],{"ref":76,"mode":19,"provenance":20,"text":78,"source_hash":79},{"type":17,"topic":7,"id":77,"field":17},"BS-R006","Percent yield = (actual / theoretical) × 100. Theoretical comes from the limiting reactant at 100% conversion.","26b53552b56a19e0284f311d54dfbd85a6e512467582d4727180e1886e4f03d9",{"heading":81,"kind":13,"items":82},"Theoretical from a known yield",[83],{"ref":84,"mode":19,"provenance":20,"text":86,"source_hash":87},{"type":17,"topic":7,"id":85,"field":17},"BS-R007","Given actual amount and percent yield: theoretical = (actual × 100) / percent yield.","579c112311199b1f4c4a03f1a91f17a7192b45827833b5108cccd4d59e494f87",{"heading":89,"kind":41,"items":90},"Reverse-yield (work backwards)",[91],{"ref":92,"mode":19,"provenance":20,"text":94,"source_hash":95},{"type":17,"topic":7,"id":93,"field":17},"BS-R014","Given actual product + percent yield, find reactant needed: actual → theoretical (via % yield) → mol product → mol reactant (ratio) → mass reactant (× MM).","310f4c29da9de0dcc774a1defe8d067978ed191354f983d66eb7f5545b39b496",{"heading":97,"kind":13,"items":98},"Gas at STP",[99],{"ref":100,"mode":19,"provenance":20,"text":102,"source_hash":103},{"type":17,"topic":7,"id":101,"field":17},"BS-R017","At STP (273.15 K, 1 atm) one mole of any ideal gas occupies 22.4 L. Use 22.4 L/mol to convert moles ↔ volume for gas-phase species only (not liquids/solids).","b414a17d50767fbf5a2063fe7802e8b14b9a82ca9a9f64c56d293079878973e2",{"heading":105,"kind":106,"items":107},"Mass-balance check","pitfalls",[108],{"ref":109,"mode":19,"provenance":20,"text":111,"source_hash":112},{"type":17,"topic":7,"id":110,"field":17},"BS-R013","Conservation of mass: total mass of reactants consumed = total mass of products formed. Use it as an independent check on the answer.","5fe5a1e9a4545dd9f96774613b52242694b9a2368b4ad1c969e7ea6223981d23",1787246033342]