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Chemistry 12.3

Chemistry 12.3. “Limiting Reagent and Percent Yield”. I. Limiting / Excess Reactants. A. Limiting Reactant 1. Def – the substance you run out of in a reaction. a. “It is limiting” B. Excess Reactant 1. Def – the substance that has extra/leftover in a reaction.

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Chemistry 12.3

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  1. Chemistry12.3 “Limiting Reagent and Percent Yield”

  2. I. Limiting / Excess Reactants A. Limiting Reactant 1. Def – the substance you run out of in a reaction. a. “It is limiting” B. Excess Reactant 1. Def – the substance that has extra/leftover in a reaction. a. “It is in abundance”

  3. C. Ex: N2 + 3H2 2NH3 -if I have 3 moles of N2 and 8 moles of H2, which will be my limiting reactant? -what will be my excess reactant? H2 N2

  4. D. Question: Sodium chloride can be prepared by the reaction of sodium metal with chlorine gas. 2 Na + Cl2 2 NaCl Suppose the 6.7 mol Na reacts with 3.2 mol of Cl2.What is the limiting reactant? How much salt can be made? Given Mole Ratio Amount Produced

  5. 6.7 mol Na 1 mol Cl2 x = 3.35 mol Cl2 2 mol Na 3.2 mol Cl2 How much chlorine do we have? Limiting Reactant = Excess Reactant = How much salt? = chlorine sodium 6.40 mol NaCl

  6. In Class Assignment Copper plus sulfur produce copper (I) sulfide. a. What is the limiting reactant when 80.0 g of Cu (I) react with 25.0 g of sulfur? b. What is the total amount in grams of copper (I) sulfide that can be made? a. Limiting reactant = Copper b. Amount produced = 100. grams of Cu2S

  7. II. Percent Yield A. Calculating Percent Yield 1. Formula Percent Yield = 2. parts… a. Theoretical yield = maximum product that could be made. Comes from the chemical formula. b. Actual yield = the amount of product that is made in a chemical reaction. c. Can never be more than 100% actual yield X 100 Theoretical yield

  8. -why less than 100%? 1. impure reactants 2. side reactions 3. loss of products (transferring between containers)

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