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Limiting Reagent and Theoretical Yield

Limiting Reagent and Theoretical Yield. Section 3. Limiting and Excess Reagents. Section 3 – Part 1. Objectives. Determine the limiting reagent in a reaction Calculate the amount of product formed in a reaction, based on the limiting reagent.

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Limiting Reagent and Theoretical Yield

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  1. Limiting Reagent and Theoretical Yield Section 3

  2. Limiting and Excess Reagents Section 3 – Part 1

  3. Objectives • Determine the limiting reagent in a reaction • Calculate the amount of product formed in a reaction, based on the limiting reagent. • Calculate the amount of excess reagent left over in a reaction.

  4. Limiting Reagent • If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how many salami sandwiches can you make? • The number of sandwiches you can make will be limited by the amount of salami you have, so the salami is the limiting ingredient. • The limitingreagent is the reactant you run out of first. • The limiting reagent determines the amount of product you can make • When all of this reactant is used up, the reaction will stop, and no more product will form.

  5. Excess Reagent • The excessreagentis the reactant that is not completely used up in the reaction. • Some of this reactant will remain unreacted when the reaction stops.

  6. Determining the Limiting Reagent • You must do two stoichiometry problems. • To determine the limiting reagent: • Convert the amount of eachreactant to the amount of product. This will be a 1, 2, or 3 step stoichiometry problem for each reactant. • The reactant that produces the LEAST amount of product is the limiting reagent. • The other reactant is the excess reagent. ** Note: You can convert the amount of reactants to either moles or grams of product. Moles is sufficient, but if you are asked to determine grams of product, converting to grams in one conversion problem is easiest.**

  7. Example • Copper reacts with sulfur to form copper(I) sulfide. If 10.6 g of copper reacts with 3.83 g S, what is the limiting reagent? • First: Write the balanced equation for the reaction.

  8. Example (continued) • Then: Convert grams of copper to moles of product and grams of sulfur to moles of product (2 stoichiometry problems).

  9. Example (continued) • Determine which reactant produces the LEAST amount of product. This is the limiting reagent. • The other reactant is the excess reagent.

  10. Using Limiting Reagent to Find Quantity of Product • Example: If 10.6 g of copper reacts with 3.83 g S, how many grams of product will be formed? This time, we will convert to grams of product since we are asked for that.

  11. If 10.6 g of copper reacts with 3.83 g S, how many grams of product will be formed? • 2Cu + S ® Cu2S Cu is Limiting Reagent 1 mol Cu2S 1 mol Cu 159.16 g Cu2S 10.6 g Cu 2 mol Cu 63.55g Cu 1 mol Cu2S = 13.3 g Cu2S = 13.3 g Cu2S 1 mol Cu2S 1 mol S 159.16 g Cu2S 3.83 g S 1 mol S 32.06g S 1 mol Cu2S = 19.0 g Cu2S

  12. Determining the Amount of Excess Reagent • We can determine the amount of excess reagent that is left over. • Use the limiting reagent to find out how much excess reagent you used in the reaction. • Subtract the amount used from the amount of excess reagent you started with to get the amount left over.

  13. Example: • If 4.87 mol of magnesium and 9.84 mol of HCl are reacted, what is the limiting reagent? • Mg(s) +2 HCl(aq) ® MgCl2(s) +H2(g) • How many moles of gas will be produced? • How much excess reagent remains?

  14. Example • If 10.3 g of aluminum are reacted with 51.7 g of CuSO4 how much copper will be produced? • How much excess reagent will remain?

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