1. 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 70.906 g Cl 2 ___________ 1 mole Cl 2 How many moles of 2,2,3-trimethylpentane are required to produce 100.0 grams of water in a complete combustion reaction? 100.0 g H 2 Ox 1 mole H 2 O ___________ 18.02 g H 2 O =0.6166 moles C 8 H 18 x 2 moles C 8 H 18 _____________ 18 mole H 2 O CO 2 +O2O2 +H2OH2OC 8 H 18 1821625

2. 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 7.500 moles of sucrose (C 12 H 22 O 11 ) in air? 7.500 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 192.12 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 ___________ 161.5 g ZnSO 4 =0.310 moles CuSO 4 x 1 mole CuSO 4 _____________ 1 mole ZnSO 4 ZnSO 4 +Zn+CuCuSO 4 1111 H3C6H5O7H3C6H5O7 +O2O2 +H2OH2OC 12 H 22 O 11 3123

3. 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 ______________ 80.04 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 18.02 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 ______________ 119.38 grams CHCl 3 =6.72 g CH 4 1CH 4 1CHCl 3 +3HCl x 1 mole CH 4 ___________ 1 mole CHCl 3 x 16.043 grams CH 4 ______________ 1 mole CH 4 3Cl 2 +

4. 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 100.0 grams of Sodium azide? 100.0 grams NaN 3 x 1 mole NaN 3 ______________ 65.011 grams NaN 3 =64.64 g N 2 2NaN 3 3N 2 +2Na x 3 moles N 2 ___________ 2 mole NaN 3 x 28.014 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 2 + 45.0 grams CH 3 OHx 1 mole CH 3 OH ______________ 32.042 grams CH 3 OH =5.66 g H 2 x 2 mole H 2 ___________ 1 mole CH 3 OH x 2.016 grams H 2 ______________ 1 mole H 2

5. Stoichiometry III. Determining the Limiting Reactant If 200.0 grams of sulfur react with 100.0 grams of chlorine in a synthesis reaction, what mass, in grams, of Disulfur dichloride is produced? 100.0 grams Cl 2 x 1 mole Cl 2 ______________ 70.906 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 135.038 grams S 2 Cl 2 _______________ 1 mole S 2 Cl 2 + 200.0 g S 8 x 1 mole S 8 ___________ 256.53 g S 8 =0.7796 moles S 8 100.0 g Cl 2 x 1 mole Cl 2 ___________ 70.906 g Cl 2 =1.410 moles Cl 2 _____________ 1 mole S 8 4 moles Cl 2 = =0.7796 0.3525=Limiting reactant In excess=

6. 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 ______________ 123.90 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 283.89 grams P 4 O 10 _______________ 1 mole P 4 O 10 + 25.0 g P 4 x 1 mole P 4 ___________ 123.90 g P 4 =0.202 moles P 4 50.0 g O 2 x 1 mole O 2 ___________ 31.998 g O 2 =1.56 moles O 2 _____________ 1 mole P 4 5 moles O 2 = =0.202 0.312=In excess Limiting reactant=

7. Stoichiometry IV. Calculating Percent Yield If 0.500 grams of Silver nitrate react with 0.500 grams of Potassium chromate and 0.455 grams of Silver chromate is produced, what is the percent yield of Silver chromate? x 1 mole AgNO 3 ______________ 169.87 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 331.728 grams Ag 2 CrO 4 __________________ 1 mole Ag 2 CrO 4 + 0.500 g AgNO 3 x 1 mole AgNO 3 ___________ 169.87 g AgNO 3 =0.00294 moles AgNO 3 0.500 g K 2 CrO 4 x 1 mole K 2 CrO 4 ___________ 194.19 g K 2 CrO 4 =0.00257 moles K 2 CrO 4 _________________ 2 moles AgNO 3 1 moles K 2 CrO 4 = =0.00147 0.00257=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) 0.500 g AgNO 3 Theoretical Yield Percent Yield= Actual Yield _____________ Theoretical Yield x100Percent Yield= _____________ x100 0.488 g Ag 2 CrO 4 0.455 g Ag 2 CrO 4 =93.2%

8. 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 __________ 20.006 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 144.09 grams H 2 SiF 6 __________________ 1 mole H 2 SiF 6 + 40.0 g HFx 1 mole HF ___________ 20.006 g HF =2.00 moles HF 40.0 g SiO 2 x 1 mole SiO 2 ___________ 60.084 g SiO 2 =0.666 moles SiO 2 ___________ _________________ 6 moles HF 1 moles SiO 2 = = 0.333 0.666=In excess Limiting reactant= +2H 2 O(l) 40.0 g HF Theoretical Yield Percent Yield= Actual Yield _____________ Theoretical Yield x100Percent Yield= _____________ x100 48.0 g H 2 SiF 6 45.8 g H 2 SiF 6 =95.4%