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Stoichiometry Jeopardy

Dive into the world of stoichiometry, from identifying limiting reactants to calculating percentage yields. Learn essential concepts and solve problems with critical thinking skills. Enhance your chemistry knowledge with exciting movie quotes!

michaelporter
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Stoichiometry Jeopardy

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  1. Stoichiometry Jeopardy

  2. Vocabulary

  3. Moles/Grams Volume/Particles

  4. Critical Thinking

  5. Calculations!

  6. Movie Quotes

  7. Vocabulary Moles/Grams Volume/Particles Critical Thinking Calculations! Movie Quotes $100 $100 $100 $100 $100 FJ $200 $200 $200 $200 $200 $300 $300 $300 $300 $300 $400 $400 $400 $400 $400 DD $500 $500 $500 $500 $500

  8. The substance not completely used up in a chemical reaction Answer…

  9. Excess Reactant 100

  10. The branch of chemistry that deals with the relationship between reactants and products in a chemical reaction Answer…

  11. Stoichiometry 200

  12. The substance that controls the amount of product that can be made Answer…

  13. Limiting Reactant 300

  14. The measured amount of product obtained from a chemical reaction Answer…

  15. Actual Yield 400

  16. The ratio of the actual yield to theoretical yield X 100% Answer…

  17. Percentage Yield 500

  18. The ratio of Fe to Fe2O3 in the reaction below is Fe2O3 + 2 Al 2 Fe + Al2O3 Answer…

  19. 2 : 1(2 to 1) 100

  20. To convert from moles of what you’re given to moles of what you want, what do you need to use? Answer…

  21. Mole Ratio(aka secret magic step) 200

  22. How is density used in stoichiometry problems? Answer…

  23. Use the density of the substance to convert mL or liters of what you’re given to grams and then to moles. Then you can use the mole ratio to convert to moles of what you want to find. 300

  24. What number do you need to convert to number of atoms/molecules/particles? Answer…

  25. 6.022 X 1023 particles/mole(Avogadro’s number) 400

  26. Why must a chemical equation be balanced to solve stoichiometry problems? Answer…

  27. The coefficients in a balanced chemical equation show the relative number of moles of each substance. Mole ratios can then be found and used to convert from moles of one substance to moles of another. 500

  28. Why must a chemical equation be balanced to solve stoichiometry problems? Answer…

  29. The coefficients from a balanced chemical equation represent the relative number of moles and are used in the mole ratio conversion step. 100

  30. Explain the difference between a limiting reactant and an excess reactant. Answer…

  31. The limiting reactant controls the amount of product that can be made and will be used up in the reaction.The excess reactant will be left over after the reaction. 200

  32. How does the actual yield of a chemical reaction compare to the theoretical yield? Answer…

  33. The actual yield is LESS than the theoretical yield. 300

  34. Explain why the conversion factor 3 g Mg(OH)2 cannot be used 6 g H2Ofor the following reaction:Mg3N2 + 6 H2O 3 Mg(OH)2 + 2 NH3 Answer…

  35. The coefficients from the balanced equation represent number of moles of reactants and products – NOT grams. 400

  36. In the “Stoichiometry and Gravimetric Analysis” lab, you prepared strontium carbonate, SrCO3, according to the following equation:SrCl2 + Na2CO3 2 NaCl + SrCO3a) What type of reaction was this?b) Why was the SrCO3 rinsed in the funnel after filtering? Answer…

  37. a) Double displacementb) The SrCO3 was rinsed in the funnel to remove any NaCl that may have been present. 500

  38. How many moles of hydrogen are needed to prepare 312 moles of ammonia?N2 + 3 H2 2 NH3 Answer…

  39. 468 mol H2 100

  40. How many grams of Al are needed to completely react with 135 g of Fe2O3?Fe2O3 + 2 Al 2 Fe + Al2O3 Answer…

  41. 45.6 g Al 200

  42. How many mL of C5H8 can be made from 366 mL of C5H12?(Density of C5H8 = 0.681 g/mL)(Density of C5H12 = 0.620 g/mL)C5H12 C5H8 + 2 H2 Answer…

  43. 315 mL C5H8 300

  44. How many grams of C5H8 form from 1.89 X 1024 molecules C5H12?C5H12 C5H8 + 2 H2 Answer…

  45. 214 g C5H8 400

  46. Find the limiting reactant, the theoretical yield, and the percentage yield if 14.0 g N2 are mixed with 9.0 g H2 and 16.1 g NH3 form.N2 + 3 H2 2 NH3 Answer…

  47. N2 is limiting reactantTheoretical yield = 17.0 g NH3Percentage yield = 94.7% 500

  48. Listen… What movie is this quote from? Answer…

  49. “The Wizard of Oz”“I’ll get you my pretty, and your little dog too!”(The wicked witch of the west talking to Dorothy) 100

  50. Listen… What movie is this quote from? Answer…

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