Stoichiometry-the study of the ____________ relationships between the amounts of __________ used and the amounts of __________ formed during a __________ __________ quantitative reactants productschemicalreaction I. Converting Moles of Reactant to Mass of Product and from Mass of Product to Moles of Reactant What mass, in grams, of chlorine gas can be produced from the decomposition of 2.50 moles of Sodium chloride? 2.50 moles NaClx 1 mole Cl 2 ___________ 2 mole NaCl =88.6 g Cl 2 conversion factor 2NaCl2Na+1Cl 2 x g Cl 2 ___________ 1 mole Cl 2 How many moles of 2,2,3-trimethylpentane are required to produce grams of water in a complete combustion reaction? g H 2 Ox 1 mole H 2 O ___________ g H 2 O = moles C 8 H 18 x 2 moles C 8 H 18 _____________ 18 mole H 2 O CO 2 +O2O2 +H2OH2OC 8 H

Stoichiometry I. Converting Moles of Reactant to Mass of Product and from Mass of Product to Moles of Reactant What mass, in grams, of citric acid (H 3 C 6 H 5 O 7 ) can be produced from the fermentation of moles of sucrose (C 12 H 22 O 11 ) in air? moles C 12 H 22 O 11 x 2 mole H 3 C 6 H 5 O 7 ______________ 1 mole C 12 H 22 O 11 =2882 g H 3 C 6 H 5 O 7 x g H 3 C 6 H 5 O 7 _________________ 1 mole H 3 C 6 H 5 O 7 How many moles of Copper(II) sulfate are required to produce 50.0 grams of Zinc sulfate in a single displacement reaction? 50.0 g ZnSO 4 x 1 mole ZnSO 4 ___________ g ZnSO 4 =0.310 moles CuSO 4 x 1 mole CuSO 4 _____________ 1 mole ZnSO 4 ZnSO 4 +Zn+CuCuSO H3C6H5O7H3C6H5O7 +O2O2 +H2OH2OC 12 H 22 O

Stoichiometry II. Converting Mass of Reactant to Mass of Product and from Mass of Product to Mass of Reactant What mass, in grams, of water can be obtained from the decomposition of 25.0 grams of Ammonium nitrate? 25.0 grams NH 4 NO 3 x 1 mole NH 4 NO 3 ______________ grams NH 4 NO 3 =11.3 g H 2 O conversion factor 1NH 4 NO 3 1N 2 O+2H 2 O x 2 moles H 2 O ___________ 1 mole NH 4 NO 3 x grams H 2 O _____________ 1 mole H 2 O What mass, in grams, of methane is required to produce 50.0 grams of chloroform? 50.0 grams CHCl 3 x 1 mole CHCl 3 ______________ grams CHCl 3 =6.72 g CH 4 1CH 4 1CHCl 3 +3HCl x 1 mole CH 4 ___________ 1 mole CHCl 3 x grams CH 4 ______________ 1 mole CH 4 3Cl 2 +

Stoichiometry II. Converting Mass of Reactant to Mass of Product and from Mass of Product to Mass of Reactant What mass, in grams, of nitrogen can be obtained from the decomposition of grams of Sodium azide? grams NaN 3 x 1 mole NaN 3 ______________ grams NaN 3 =64.64 g N 2 2NaN 3 3N 2 +2Na x 3 moles N 2 ___________ 2 mole NaN 3 x grams N 2 _____________ 1 mole N 2 What mass, in grams, of Hydrogen is required to produce 45.0 grams of methanol, in a synthesis reaction with Carbon monoxide ? 1CO1CH 3 OH2H grams CH 3 OHx 1 mole CH 3 OH ______________ grams CH 3 OH =5.66 g H 2 x 2 mole H 2 ___________ 1 mole CH 3 OH x grams H 2 ______________ 1 mole H 2

Stoichiometry III. Determining the Limiting Reactant If grams of sulfur react with grams of chlorine in a synthesis reaction, what mass, in grams, of Disulfur dichloride is produced? grams Cl 2 x 1 mole Cl 2 ______________ grams Cl 2 =190.4 g S 2 Cl 2 1S 8 4Cl 2 4S 2 Cl 2 x 4 moles S 2 Cl 2 ___________ 4 moles Cl 2 x grams S 2 Cl 2 _______________ 1 mole S 2 Cl g S 8 x 1 mole S 8 ___________ g S 8 = moles S g Cl 2 x 1 mole Cl 2 ___________ g Cl 2 =1.410 moles Cl 2 _____________ 1 mole S 8 4 moles Cl 2 = = =Limiting reactant In excess=

Stoichiometry III. Determining the Limiting Reactant If 25.0 grams of phosphorus react with 50.0 grams of oxygen in a synthesis reaction, what mass, in grams, of Tetraphosphorus decoxide is produced? 25.0 grams P 4 x 1 mole P 4 ______________ grams P 4 =57.3 g P 4 O 10 1P 4 5O 2 1P 4 O 10 x 1 mole P 4 O 10 ___________ 1 mole P 4 x grams P 4 O 10 _______________ 1 mole P 4 O g P 4 x 1 mole P 4 ___________ g P 4 =0.202 moles P g O 2 x 1 mole O 2 ___________ g O 2 =1.56 moles O 2 _____________ 1 mole P 4 5 moles O 2 = = =In excess Limiting reactant=

Stoichiometry IV. Calculating Percent Yield If grams of Silver nitrate react with grams of Potassium chromate and grams of Silver chromate is produced, what is the percent yield of Silver chromate? x 1 mole AgNO 3 ______________ grams AgNO 3 =0.488 g Ag 2 CrO 4 2AgNO 3 (aq)1K 2 CrO 4 (aq)1Ag 2 CrO 4 (s) x 1 mole Ag 2 CrO 4 ___________ 2 mole AgNO 3 x grams Ag 2 CrO 4 __________________ 1 mole Ag 2 CrO g AgNO 3 x 1 mole AgNO 3 ___________ g AgNO 3 = moles AgNO g K 2 CrO 4 x 1 mole K 2 CrO 4 ___________ g K 2 CrO 4 = moles K 2 CrO 4 _________________ 2 moles AgNO 3 1 moles K 2 CrO 4 = = =In excess Limiting reactant= -the ________ ______ is the ______ of the _______ ______ to the ____________ ______ expressed as a ________ percentyieldratio actualyield theoreticalyield percent Percent Yield= Actual Yield _____________ Theoretical Yield x100 +2KNO 3 (aq) g AgNO 3 Theoretical Yield Percent Yield= Actual Yield _____________ Theoretical Yield x100Percent Yield= _____________ x g Ag 2 CrO g Ag 2 CrO 4 =93.2%

Stoichiometry IV. Calculating Percent Yield If 40.0 grams of Hydrogen fluoride react with 40.0 grams of Silicon dioxide and 45.8 grams of Dihydrogen hexafluorosilicate is produced, what is the percent yield of Dihydrogen hexafluorosilicate? x 1 mole HF __________ g HF =48.0 g H 2 SiF 6 1SiO 2 (s)6HF(aq)1H 2 SiF 6 (aq) x 1 mole H 2 SiF 6 ___________ 6 mole HF x grams H 2 SiF 6 __________________ 1 mole H 2 SiF g HFx 1 mole HF ___________ g HF =2.00 moles HF 40.0 g SiO 2 x 1 mole SiO 2 ___________ g SiO 2 =0.666 moles SiO 2 ___________ _________________ 6 moles HF 1 moles SiO 2 = = =In excess Limiting reactant= +2H 2 O(l) 40.0 g HF Theoretical Yield Percent Yield= Actual Yield _____________ Theoretical Yield x100Percent Yield= _____________ x g H 2 SiF g H 2 SiF 6 =95.4%