1 / 12

Section 6.6—Limiting Reactants

Section 6.6—Limiting Reactants. What happens if you don’t add reactants in a molar ratio?. Planning a Meal. You go to the grocery store and you buy 1 package of Brats (5 Brats), 1 package of cheese (16 slices) and 1 package of hot dog buns (8 buns). If you use all of these….

yen
Download Presentation

Section 6.6—Limiting Reactants

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Section 6.6—Limiting Reactants What happens if you don’t add reactants in a molar ratio?

  2. Planning a Meal You go to the grocery store and you buy 1 package of Brats (5 Brats), 1 package of cheese (16 slices) and 1 package of hot dog buns (8 buns). If you use all of these… You can make this many… 5 Brats 5 meals 16 slices of cheese 16 meals 8 hot dog buns 8 meals So you have the possibility of making 5, 16 or 8 meals…which is it? You’ll never get the chance to make 8 or 16 meals…you’ll run out of Brats after 5. Once you run out of one component, you have to stop making meals.

  3. What’s a limiting reactant? Limiting Reactant– The reactant that runs out and causes the reaction to stop. In the previous example, the Brats were the limiting reactant—once they were gone, you had to stop! Once even one of the reactants runs out, the reaction stops…it can’t make any more product.

  4. Excess reactant • The reactant that is not completely used up in a reaction

  5. When solving: • Both reactants will be given info. • Use stoichiometry to find the (mass, moles, vol. etc) of EACH reactant • Whichever number is smaller will be your limiting reactant

  6. Limiting Reactant Example Example: How many moles of H2O is produced when 2.3 moles O2 and 2.3 moles H2 react? 2 H2 + O2 2 H2O

  7. Limiting Reactant Example Example: How many moles of H2O is produced when 2.3 moles O2 and 2.3 moles H2 react? 2 H2 + O2 2 H2O From balanced equation: 2 mole H2 2 mole H2O 1 mole O2 2 mole H2O 2.3 mole O2 2 mole H2O 4.6 = ________ mole H2O 1 mole O2 2.3 mole H2 2 mole H2O 2.3 = ________ mole H2O 2 mole H2

  8. Limiting Reactant Example Example: How many moles of H2O is produced when 2.3 moles O2 and 2.3 moles H2 react? 2 H2 + O2 2 H2O From balanced equation: 2 mole H2 2 mole H2O 1 mole O2 2 mole H2O 2.3 mole O2 2 mole H2O 4.6 = ________ mole H2O 1 mole O2 2.3 mole H2 2 mole H2O 2.3 = ________ mole H2O 2 mole H2 Limiting reactant!

  9. Let’s Practice Example: If you react 10.5 g of NaOH and 7.5 g of BaCl2, how many grams NaCl is produced? 2 NaOH + BaCl2 Ba(OH)2 + 2 NaCl

  10. Let’s Practice Example: If you react 10.5g of NaOH and 7.5g of BaCl2, how many grams NaCl is produced? 2 NaOH + BaCl2 Ba(OH)2 + 2 NaCl From balanced equation: 2 mole NaOH  2 mole NaCl 1 mole BaCl2 2 mole NaCl Molecular masses: 40.00 g NaOH = 1 mole NaOH 171.35 g Ba(OH)2 = 1 mole Ba(OH)2 58.44 g NaCl = 1 mole NaCl 10.50 g NaOH 1 2 mole NaCl mole NaOH 58.44 g NaCl 15.3 = _______ g NaCl 40.00 g NaOH 2 mole NaOH 1 mole NaCl 7.50 g BaCl2 1 2 mole NaCl mole BaCl2 58.44 g NaCl 5.12 = _______ g NaCl 171.35 g BaCl2 1 mole BaCl2 1 mole NaCl

  11. Lets Practice • 2Na + Cl2 2NaCl • Suppose that 6.70 mol of Na reacts with 3.20 mol of Cl2. • 1) What is the limiting reactant? • How many moles of NaCl are produced?

  12. Lets Practice • 2Cu(s) + S(s) Cu2S(s) • What is the limiting regent when 80.0g Cu reacts with 25.0g S? • How grams of Cu2S will be produced?

More Related