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By: Ashlee Katie & Jaselyn

By: Ashlee Katie & Jaselyn. Chapter 4 Stoichiometry. Final Jeopardy. 100 Stoichiometry. 200 Stoichiometry. What is percent yield? How is it calculated?. 300 Stoichiometry. What mass of water is produced when 39 grams of benzene is burned?. 400 Stoichiometry.

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By: Ashlee Katie & Jaselyn

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  1. By: Ashlee Katie & Jaselyn Chapter 4 Stoichiometry

  2. Final Jeopardy

  3. 100 Stoichiometry

  4. 200 Stoichiometry What is percent yield? How is it calculated?

  5. 300 Stoichiometry What mass of water is produced when 39 grams of benzene is burned?

  6. 400 Stoichiometry 10 grams of sodium chloride is treated with excess silver nitrate. How much silver chloride is produced?

  7. 500 Stoichiometry 12 grams of copper is treated with excess nitric acid: Cu + HNO3 Cu(NO3)2 + NO + H2O How much NO is produced? Why wasn’t HCl used?

  8. 100 Limiting Reagents

  9. 200 Limiting Reagents Why is it important to identify the limiting reagent?

  10. 300 Limiting Reagents How is the limiting reagent selected?

  11. 400 Limiting Reagents 6.54 g of zinc reacts with 5.47 g of HCl. What mass of hydrogen gas will be produced?

  12. 500 Limiting Reagents N2H4 + N2O4 N2 + 4H2O 50.0 g of hydrazine is mixed with 100.0 g of dinitrogen tetroxide. How much nitrogen gas is produced? What mass of the excess reagent remains?

  13. 100 Chemical Analysis

  14. 200 Chemical Analysis Explain how the empirical formulas of hydrocarbons are determined.

  15. 300 Chemical Analysis 5.0 g of a mixture containing some Ag was analyzed to determine the percent Ag in the mixture. The mixture was dissolved in water and excess NaCl was added. What mass of AgCl formed if the mixture was 75% silver?

  16. 400 Chemical Analysis 7.321 g of an organic compound containing carbon, hydrogen, and oxygen was analyzed by combustion. 17.873 g of carbon dioxide and 7.316 g of water was produced. Find the empirical formula.

  17. 500 Chemical Analysis 0.1101 g of a compound containing C, H, and O was combusted to produce 0.2503 g CO2 and 0.1025 g of H2O. The molar mass of the compound was 115 g/mol. Find the empirical and molecular formulas.

  18. 100 Molarity

  19. 200 Molarity How would you make 100.0 mL of a 6 M solution of sodium chloride in the laboratory?

  20. 300 Molarity 50.0 g of sodium hydroxide is dissolved to make 600 mL of solution. What is its molarity?

  21. 400 Molarity What is the molarity that results from adding 25 mL of a 0.15M solution of sodium hydroxide to sufficient water to make 500 mL of solution?

  22. 500 Molarity When excess silver nitrate is added to a 25.0 mL sample of a solution of potassium chloride, 0.9256 g of silver chloride precipitated. What is the concentration of the potassium chloride solution?

  23. Daily Double

  24. Final Jeopardy Make Your Wager

  25. Final Jeopardy

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