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Mr. Quinn & Ms. Tom February 11, 2014 Aim: How do we determine the limiting reagent in a chemical reaction? Do Now: balance the following chemical equation. ___ YCl 3 + ___ NbBr 5 __ YBr 3 + ___ NbCl 5

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The Steps 1.Balance the equation 2.Solve for the amount of product formed for each reactant You will get different numbers 3.Whichever reactant formed a smaller amount of product is your limiting reagent.

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Example 1: Carbon and Fluorine Graphite (C) burns in fluorine according to the following unbalanced equation. If 16 g of carbon are burned with 48 g of fluorine, what is the limiting reagent? 1.Balance the equation (list the elements, tally the elements, solve) C + F 2 CF 4

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Example 1: Carbon and Fluorine 1 C + 2 F 2 1 CF 4 2.Find the molar mass of both reactants and one product Graphite (C) Fluorine (F 2 ) ElementNumberMassTotal ElementNumberMassTotal C112 F2 Sum of everything: CF 4 ElementNumberMassTotal C F Sum of everything:

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Example 1: Carbon and Fluorine 3.Use dimensional analysis to predict the product formation from both reactants. Starting Mass (From problem) Reciprocal of Molar Mass Reactant 2 (F 2 ) Mole ratio from balanced equation (F 2 :AlF 3 ) Molar mass of product (AlF 3 ) Result (in g of AlF 3 ) X X X = Starting Mass (From problem) Reciprocal of Molar Mass Reactant 1 (C) Mole ratio from balanced equation (Al:AlF 3 ) Molar mass of product (AlF 3 ) Result (in g of AlF 3 ) X X X =

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Example 2: Aluminum and Fluorine Aluminum (Al) burns in fluorine according to the following unbalanced equation. If 16 g of aluminum are burned with 57 g of fluorine, what is the limiting reagent? 1.Balance the equation (list the elements, tally the elements, solve) Al + F 2 AlF 3

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Example 1: Aluminum and Fluorine 2 Al + 3 F 2 2 AlF 3 2.Find the molar mass of both reactants and one product Aluminum (Al) Fluorine (F 2 ) ElementNumberMassTotal ElementNumberMassTotal Al1 F Sum of everything: AlF 3 ElementNumberMassTotal Sum of everything:

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Example 1: Aluminum and Fluorine 3.Use dimensional analysis to predict the product formation from both reactants. Starting Mass (From problem) Reciprocal of Molar Mass Reactant 2 (Al) Mole ratio from balanced equation Molar mass of product (AlF 3 ) Result (in g of AlF 3 ) X X X = Starting Mass (From problem) Reciprocal of Molar Mass Reactant 1 (Al) Mole ratio from balanced equation Molar mass of product (AlF 3 ) Result (in g of AlF 3 ) X X X =

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Example 1: Sulfur and Fluorine Sulfur (S 8 ) burns in fluorine according to the following unbalanced equation. If 128 g of sulfur are burned with 144 g of fluorine, what is the limiting reagent? 1.Balance the equation (list the elements, tally the elements, solve) S 8 + F 2 SF 2

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Example 1: Carbon and Fluorine 1 S 8 + 8 F 2 8 SF 2 2.Find the molar mass of both reactants and one product

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Example 1: Carbon and Fluorine 3.Use dimensional analysis to predict the product formation from both reactants. Starting Mass (From problem) Reciprocal of Molar Mass Reactant 2 Mole ratio from balanced equation Molar mass of product Result X X X = Starting Mass (From problem) Reciprocal of Molar Mass Reactant 1 Mole ratio from balanced equation Molar mass of product Result X X X =

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Drill – 2/28/11 Sodium chloride decomposes into sodium and chlorine. How much (in grams) sodium chloride is required to produce 50.0g of chlorine gas?

Drill – 2/28/11 Sodium chloride decomposes into sodium and chlorine. How much (in grams) sodium chloride is required to produce 50.0g of chlorine gas?

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