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Hydrate Lab

Hydrate Lab. Cu(SO 4 ) . H 2 O ---- > Cu(SO 4 ) + H 2 O Use the equation above to help answer the following questions: What is the hydrate salt in this equation? What is the anhydrous salt in this equation? What is the difference between a hydrated salt and an anhydrous salt?

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Hydrate Lab

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  1. Hydrate Lab Cu(SO4) . H2O ----> Cu(SO4) + H2O Use the equation above to help answer the following questions: • What is the hydrate salt in this equation? • What is the anhydrous salt in this equation? • What is the difference between a hydrated salt and an anhydrous salt? • Is this a physical or chemical reaction?

  2. Hydrate Lab Cu(SO4) . H2O ----> Cu(SO4) + H2O

  3. Copper Sulfate Hydrate

  4. Bell Ringer • Calculate the percent composition of water in this hydrate: Mg(SO4) .7H2O (Epsom Salt) 2. N2 + H2 ----------> NH3 a. What type of chemical reaction is this? b. Balance the chemical equation. c. What does this balanced chemical equation tell you?

  5. Bell Ringer: Hydrates (1,3) • Answer these questions pertaining to the following equation: Mg(SO4) .7H2O -----> Mg(SO4) + H2O a. What is the chemical formula of the hydrate? b. What is the chemical formula for the anhydrous salt? c. What is the mole ratio of salt to water in the hydrate? d. What is the percent composition of water in the hydrate?

  6. Infinite Campus Update • Hydrate Lab: today, May 3rd • Lab Report-final draft: by Monday, May 7th • Stoichiometry Quiz: Monday, May 7th

  7. Infinite Campus Update • Hydrate Lab: today, May 3rd • Famous Scientist Rough Draft: by Monday, May 7th • Stoichiometry Quiz: Monday, May 7th

  8. Infinite Campus Update • Lab Report-final draft: by Monday, May 7th • Stoichiometry Quiz: Monday, May 7th

  9. Infinite Campus Update • Hydrate Lab : posted in IC • Lab Report-final draft: by Monday, May 7th • Stoichiometry Quiz: Monday, May 7th

  10. Stochiometry ObjectivesChapter 12 I can explain why it is important to balance chemical equations. 2. I can convert between substances in a balanced chemical equation using mole conversions.

  11. Balancing and Interpreting Chemical Equations N2 + H2 ----------> NH3 1. What type of chemical reaction is this? Balance the chemical equation. What does this balanced chemical equation tell you?

  12. Balancing and Interpreting Chemical Equations N2 + 3H2 ----------> 2NH3 1. a. According to the equation how many moles of NH3 is produced? b. How many moles of N2 are needed to produce 8.0 moles of NH3?

  13. Stoichiometry (1, 2nd) H2O ----------> H2 + O2 1. What type of reaction is this? 2. Balance the chemical equation if needed. 3. Interpret the chemical equation using moles? 4. If you start with 100 moles of H2O how many moles of H2 would be produced?

  14. Stoichiometry N2 + 3H2 ----------> 2NH3 Converting between substances in a balanced chemical equation using mole conversions.

  15. Bell Ringer: Stoichiometry • N2H4 + O2 -----> N2 + H2O • Balance the equation. • How many moles of N2H4 (rocket fuel) are present in the chemical equation? • If 5.6 moles of rocket fuel reacted with oxygen how many moles of nitrogen and water do you predict would be produced? • If 13.8 grams of water were produced how much rocket fuel in grams would have been used up?

  16. Bell Ringer: Stoichiometry N2H4 + O2 -----> N2 + H2O Balance the equation. How many moles of N2H4 (rocket fuel) are present in the chemical equation? If 5.6 moles of rocket fuel reacted with oxygen how many moles of nitrogen and water do you predict would be produced?

  17. Bell Ringer: Stoichiometry N2H4 + O2 -----> N2 + 2H2O If 13.8 grams of water were produced how much rocket fuel in grams would have been used up?

  18. Stoichiometry:

  19. Balancing and Interpreting Chemical Equations N2 + H2 ----------> NH3 1. What type of chemical reaction is this? Balance the chemical equation. What does this balanced chemical equation tell you?

  20. Stoichiometry N2 + 3H2 ----------> 2NH3 Stoichiometry: Converting between substances in a balanced chemical equation using mole conversions.

  21. Balancing and Interpreting Chemical Equations N2 + 3H2 ----------> 2NH3 1. a. According to the equation how many moles of NH3 is produced? b. How many moles of N2 are needed to produce 8.0 moles of NH3?

  22. Mole-Mole Stoichiometry Conversions A -----> B + C Convert from moles of substance A to moles of substance B. Moles of given substance Moles of wanted substance mole given to mole wanted ratio (balanced equation) One step conversion: Convert from moles of given substance to moles of wanted substance using the balanced equation.

  23. Stoichiometry:Mole to Mole Conversions

  24. Stoichiometry Problems: C3H8 + 5O2 -------> 3 CO2 + 4H2O How many grams of CO2 are produced when 6.2 grams of C3H8 combusts with oxygen?

  25. Mass to Mass Stoichiometry Conversions A -----> B + C Convert from grams of substance A to grams of substance B. Mass of given substance Moles of given substance Moles of wanted substance Mass of wanted substance • mass to mol of given mol given to mol wanted mol to mass of wanted • (molar mass conversion) (balanced equation) (molar mass conversion) • Three Step Conversion: • Convert grams of given to moles using the molar mass conversion. (1 mole = molar mass of given) • Convert moles of given to moles of wanted using • the balanced equation. • 3.Convert moles of wanted to grams using the molar mass conversion.(1 mole = molar mass of wanted)

  26. Stoichiometry:Mass to Mass Conversions

  27. Stoichiometry:Mass to Mass Conversions

  28. Stoichiometry HCl + Mg -------> MgCl2 + H2 • What type of reactions is this? • Balance the equation if needed. • If 6.8 moles of Mg react with 7.5 moles of HCl, how many moles of MgCl2 would be produced?

  29. Limiting Reagent Demonstration Lab Purpose: Illustrate the concept of a limiting reactant in a chemical reaction. Procedures: Add different amounts of magnesium strips to 13mL of 1.0 M hydrochloric acid. Data: What did you observe from the demonstration? Conclusion: What is the limiting and excess reactant in this reaction?

  30. Stoichiometry: Limiting Reactants • Limiting Reactant: • Excess Reactant: en.wikipedia.org

  31. Stoichiometry: Limiting Reactants • Limiting Reactant: completely consumed • Excess Reactant: partially consumed en.wikipedia.org

  32. Stoichiometry: Limiting Reactant HCl + Mg -------> MgCl2 + H2 • What type of reactions is this? • Balance equation if needed. • If 6.8 moles of Mg react with 7.5 moles of HCl, how many moles of MgCl2 and H2 would be produced?

  33. Stoichiometry: Limiting vs. Reactant • Limiting Reactant: Al Theoretical Yield of AlCl3: 3.0 moles • Limiting Reactant: C2H4 Theoretical yield of H2O: 5.4 moles • Limiting Reactant: N2 Theoretical yield of NH3: 34 g

  34. Stoichiometry: Percent Yield % Yield of Product: Accuracy of product formation in the lab. % Yield of product:actual yield x 100 theoretical yield • Theoretical yield of AlCl3: 3.0 moles Actual yield from lab of AlCl3: 2.8 moles Calculate % yield of AlCl3:

  35. Stoichiometry: Percent Yield 4. Theoretical Yield of AlCl3: 3.0 moles Actual yield from lab of AlCl3: 2.8 mole % Yield of AlCl3:93% 5. Theoretical yield of H2O: 5.4 moles Actual yield from lab of H2O: 4.9 moles % Yield of H2O: 91% • Theoretical yield of NH3: 34 g Actual yield from lab of NH3: 31.5 g % yield of NH3: 92.6%

  36. Bell Ringer: Limiting Reactants and % Yield C2H2 + O2 --- CO2 + H2O 1. Balance the equation if needed. • If 2.40 moles of C2H2 reacts with 7.40 moles of O2how many grams of water can be produced? • What is the limiting reactant? • Use limiting reactant to calculate theoretical yield of H2O in grams. • If the actual yield of H2O in the lab was 40.1 grams, calculate what the % yield of H2O would be.

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