1 / 35

Using R.I.C.E. Tables and stoichiometry with limiting reactants

Using R.I.C.E. Tables and stoichiometry with limiting reactants. RICE tables are a common tool of chemists (college professors use then a lot!) to organize the information for stoichiometry with a reaction and set up mathematical equations when necessary to solve for unknowns.

quynh
Télécharger la présentation

Using R.I.C.E. Tables and stoichiometry with 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. Using R.I.C.E. Tables and stoichiometry with limiting reactants

  2. RICE tables are a common tool of chemists (college professors use then a lot!) to organize the information for stoichiometry with a reaction and set up mathematical equations when necessary to solve for unknowns. R = reaction (balanced) I = initial conditions (before the reaction) C = change (remove reactants, form products) E = end conditions (after the reaction)

  3. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed?

  4. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? BEWARE: Moles goes into a RICE table and moles will come out. To find volume will require a final step.

  5. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R =

  6. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O

  7. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I =

  8. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g

  9. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0

  10. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C =

  11. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C = -1x -3x +2x +2x

  12. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C = -1x -3x +2x +2x all the ethene will be burned, so x = 0.63 mol

  13. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C = -1x -3x +2x +2x -0.625 mol -1.875 mol +1.25 mol +1.25 mol

  14. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C = -1x -3x +2x +2x -0.625 mol -1.875 mol +1.25 mol +1.25 mol E =

  15. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 0.625 mol ? 0 0 C = -1x -3x +2x +2x -0.625 mol -1.875 mol +1.25 mol +1.25 mol E = 0 ?-1.875 mol 1.25 mol 1.25 mol

  16. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? How many moles of CO2 was formed?

  17. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? How many moles of CO2 was formed? 1.3 mol

  18. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? How many moles of CO2 was formed? 1.3 mol What volume of CO2 was formed?

  19. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? How many moles of CO2 was formed? 1.3 mol What volume of CO2 was formed? 1.25 mol x 22.4 L/mol = 28 L

  20. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? How many moles of CO2 was formed? 1.3 mol What volume of CO2 was formed? 1.25 mol x 22.4 L/mol = 28 L What other information do we already know?

  21. Example 1: 10. grams of ethene is combusted. What volume of carbon dioxide will be formed? • How many moles of CO2 was formed? 1.3 mol • What volume of CO2 was formed? • 1.25 mol x 22.4 L/mol = 28 L • What other information do we already know? • Moles of O2 consumed • Moles of H2O produced

  22. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed?

  23. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O

  24. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 50. g 0.625 mol 1.56 mol

  25. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 50. g 0.625 mol 1.56 mol C = -1x -3x +2x +2x WHICH X TO USE? SMALLEST X!

  26. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 50. g 0.625 mol 1.56 mol C = -1x -3x +2x +2x WHICH X TO USE? SMALLEST X! If 0.625 = 1 x, then x = 0.625 If 1.56 = 3 x, then x = 0.521 ← SMALLEST

  27. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 50. g 0.625 mol 1.56 mol C = -1x -3x +2x +2x -0.521 mol -1.56 mol +1.04 mol 1.04 mol

  28. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? R = C2H4 + 3O2→ 2CO2 + 2H2O I = 10. g 50. g 0.625 mol 1.56 mol C = -1x -3x +2x +2x -0.521 mol -1.56 mol +1.04 mol 1.04 mol E = 0.625 mol – 0.521 mol 1.56 mol – 1.56 mol 1.04 mol 1.04 mol 0.104 mol 0 1.04 mol 1.04 mol

  29. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? What volume of CO2 is actually produced? 1.04 mols x 22.4 L/mol = 23 L

  30. Example 2: 10. grams of ethene is combusted with 50. grams of O2. What volume of carbon dioxide can be formed? • What volume of CO2 is actually produced? • 1.04 mols x 22.4 L/mol = 23 L • What else do we know? • Moles of ethene left over • Moles of water actually produced

  31. Why use a RICE table for limiting reactant problems? How many RR tracks would it have taken?

  32. Why use a RICE table for limiting reactant problems? How many RR tracks would it have taken? 2 to figure out which one is limiting

  33. Why use a RICE table for limiting reactant problems? How many RR tracks would it have taken? 2 to figure out which one is limiting 1 more to find amount of excess

  34. Why use a RICE table for limiting reactant problems? How many RR tracks would it have taken? 2 to figure out which one is limiting 1 more to find amount of excess 1 more for each of the additional products

  35. Why use a RICE table for limiting reactant problems? How many RR tracks would it have taken? 2 to figure out which one is limiting 1 more to find amount of excess 1 more for each of the additional products It is your choice. We did 1 RICE table vs 4 RR Tracks. RICE tables will be necessary later. For now, it is optional.

More Related