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Stoichiometry •The quantitative study of chemical reactions Stoichiometric Steps • Set up & balance rxn • Change stuff given to moles • Change moles given to ask • Change what’s asked for to the proper unit Step 1 •Determine products of a reaction if they are not given •Balance the reaction Step 2 •Use molar conversion to change whatever is given to moles Step 3 •Use the molar ratio from the balanced reaction to convert the moles of what is given to the moles of what’s asked for. Step 4 •Use molar conversions to change the moles of what is asked for to the proper unit Calculate the volume of NH3 formed at STP when 6.00 kg of H2 react with excess N2 to form NH3 Calculate the volume of NH3 formed at STP when 6.00 kg of H2 react with excess N2 to form NH3 Calculate the mass of PbI2 formed when 66.2 g of Pb(NO3)2 is combined with excess KI. Calculate the number of molecules of oxygen gas required to burn 3.5 ng of C5H10 Calculate the mass of MgCO3 formed when 18.4 g of MgBr2 is combined with a solution containing excess K2CO3. Calculate the volume of CO2 formed at STP when 16.8 g of MgCO3 is decomposed creating CO2 & MgO. Limiting Reactant •The reactant that gets used up •The reactant that determines the amount of product formed Excess Reactant •The reactant that does not get used up Stoichiometry with Multiple Reagents •Perform same steps for all reactants •Choose least amount of product Calculate the mass of glucose (C6H12O6) formed when 880 g of carbon dioxide is combined with 720 g of water in photosynthesis Calculate the # of molecules of NH3 formed when 4.0 mg of H2 react with 1.12 mL of N2 gas at STP. Theoretical Yield • The amount determined through stoichiometry • The amount solved for on paper Experimental Yield •The amount obtained in the lab •Actual yield Percent yield % Yield = (Exp/Theo) x 100 % 68 g NH3 was obtained in lab when 140 g of N2 reacts with excess H2. Calculate percent yield. 510 g PH3 were obtained in the lab when 0.62 kg of P4 reacted with excess H2. Calculate percent yield. Determine the volume of O2 released at STP when 32 kg of Fe2O3 is purified with an 80.0 % yield making Fe & O2 Calculate the volume of oxygen gas at STP required to burn 12 kg of erythrose (C4H8O4) Calculate the mass of BaSO4 formed when 41.6 g of BaCl2 is added to 17.4 g K2SO4 giving a 50.0 % yield: Calculate the mass of CaSO4 formed when 2.00 g of calcium bromide is added to 75 mL of 0.40 M sodium sulfate: Terms: Stoichiometry Percent yield Limiting Reactant Excess reactant Theoretical yield Experimental yield Calculate the volume in mL of oxygen gas at STP required to burn 50.0 mg C5H8O2: 3.67 g of PbBr2 was obtained in lab when 6.62 g of Pb(NO3)2 was added to 11.9 g KBr. Calculate the % yield. Calculate the volume of gaseous product formed when 4.2 kg of MgCO3 is heated with a 75 % yield: MgCO3 MgO + CO2 Calculate the volume of Cl2 collected at STP when 3.80 mg of F2 at STP is bubbled through a 0.050 mL solution of 0.020 M KCl: Calculate the volume in mL of gaseous products formed at STP when 6.0 mg of C2H6 is burned in excess oxygen: 33.1 g of Pb(NO3)2 was added to 1500 mL 0.10 M KI. Calculate mass of PbI2 formed. Chm II: Calculate the mass of water & NaCl formed when 6.0 g of sodium hydroxide is added to a 250 mL solution 0.40 M hydrochloric acid: Chm II: 33.1 g of Pb(NO3)2 was added to 1500 mL 0.10 M KI. Calculate mass of PbI2 formed. Chm II: 29.7 g of BaBr2 was added to 1500 mL 0.10 M K2SO4. Calculate mass of BaSO4 formed. An 30.0 g unknown sample (containing only C, H, & O) was burned in excess oxygen yielding 66 g CO2 & 36 g H2O. Calculate its empirical formula : An 240 g unknown sample (containing only C, H, S, & O) was burned in excess oxygen yielding 352 g CO2, 144 g H2O, & 128 g, SO2. Calculate its empirical formula : Calculate the mass of solid product formed when 3.31 g of Pb(NO3)2 is added to a 75.0 mL solution 0.20 M KI: Name the Following: BaCl2 Mn2O3 SF2 NH3 CaSO4 (NH4)3PO3 Fe(NO3)2 KClO3 Derive formulas for Sodium hydroxide Calcium carbonate Iron(III)phosphate Dinitrogen tetroxide Make conversions: •64 kg SO2 to mL gas •11.2 mL NH3 to atoms •180 km/hr to cm/s