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STOICHIOMETRY PRACTICE

STOICHIOMETRY PRACTICE . 1. When solid aluminum chloride is heated at high temperatures, solid aluminum and chlorine gas are produced. a. Write and balance the reaction that occurs. b. Identify the reaction type.

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STOICHIOMETRY PRACTICE

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  1. STOICHIOMETRY PRACTICE

  2. 1. When solid aluminum chloride is heated at high temperatures, solid aluminum and chlorine gas are produced. • a. Write and balance the reaction that occurs. • b. Identify the reaction type.

  3. 1. When solid aluminum chloride is heated at high temperatures, solid aluminum and chlorine gas are produced. • a. Write and balance the reaction that occurs. 2AlCl3 → 2Al + 3Cl2 • b. Identify the reaction type. • Decomposition

  4. c. What mass of aluminum chloride must decompose in order to form 10.25g of aluminum?

  5. c. What mass of aluminum chloride must decompose in order to form 10.25g of aluminum? 10.25g Al 1 mole Al 2 moles AlCl3 132 g AlCl3 = 50.1 g AlCl3 27 g Al 2 mole Al 1 mole AlCl3

  6. d. What mass of aluminum will be produced if 13.5g of chlorine are produced?

  7. d. What mass of aluminum will be produced if 13.5g of chlorine are produced? 13.5 g Cl2 1mole Cl2 2moles Al 27g Al = 3.5 g Al 70 g Cl2 3 moles Cl2 1mole

  8. e. What mass of aluminum will be produced if 20.5g of chlorine are produced?

  9. e. What mass of aluminum will be produced if 20.5g of chlorine are produced? 20.5g Cl2 1 mole Cl2 2moles Al 27g Al = 5.3 g Al 70 g Cl2 3moles Cl2 1mole Al

  10. f. How many atoms of aluminum will be produced if 20.5g of chlorine are produced?

  11. f. How many atoms of aluminum will be produced if 20.5g of chlorine are produced? 20.5g Cl2 1 mole Cl2 2moles Al 6.02 x 1023= 1.2 x 1023 atoms Al 70 g Cl2 3moles Cl2 1mole Al

  12. g. What mass of chlorine will be produced if 5.00g of aluminum chloride decompose?

  13. g. What mass of chlorine will be produced if 5.00g of aluminum chloride decompose? • 5.00g AlCl3 1mole AlCl3 3moles Cl2 70g Cl2 = 4.0 g Cl2 132g AlCl3 2 moles AlCl3 1mole Cl2

  14. 2. When flourine is bubbled through a hydrobromic acid solution, bromine and hydrofluoric acid are formed. • a. Write the balanced equation for the reaction. • b. What type of reaction is this?

  15. 2. When flourine is bubbled through a hydrobromic acid solution, bromine and hydrofluoric acid are formed. • a. Write the balanced equation for the reaction. • F2 + 2HBr → Br2 + 2HF • b. What type of reaction is this? • Single replacement

  16. b. What mass of bromine will be formed if 25.0g of fluorine react with excess hydrofluoric acid?

  17. b. What mass of bromine will be formed if 25.0g of fluorine react with excess hydrofluoric acid? 25.0 g F2 1mole F2 1mole Br2 160 g Br2 = 105.2g Br2 38 g F2 1mole F2 1mole Br2

  18. c. What mass of hydrobromic acid is needed to react with 2.8L of fluorine gas at STP?

  19. c. What mass of hydrobromic acid is needed to react with 2.8L of fluorine gas at STP? • 2.8L F2 1mole F2 2moles HBr 80g HBr = 20g HBr 22.4 L F2 1moleF2 1moleHBr

  20. e. What mass of hydrofluoric acid reacts if 16.5g of bromine form?

  21. e. What mass of hydrofluoric acid reacts if 16.5g of bromine form? • 16.5g Br2 1moleBr2 2moles HF 20g HF = 4.1gHF 160g Br2 1mole Br2 1mole HF

  22. 3. Iron reacts with sulfuric acid to form iron(III) sulfate and hydrogen gas. • a. Write the balanced reaction below. b. What type of reaction is this?

  23. 3. Iron reacts with sulfuric acid to form iron(III) sulfate and hydrogen gas. • a. Write the balanced reaction below. • 2Fe + 3H2SO4 → Fe2(SO4)3 + 3H2 • b. What type of reaction is this? • Single Replacement

  24. c. What mass of iron is needed to react with 10.5g of sulfuric acid?

  25. c. What mass of iron is needed to react with 10.5g of sulfuric acid? 10.5 g H2SO4 1 mol H2SO4 2 moles Fe 56 g = 4 g Fe 98 g 3 moles H2SO4

  26. d. What mass of iron(III) sulfate will be formed if 5.5g of iron react with excess sulfuric acid?

  27. d. What mass of iron(III) sulfate will be formed if 5.5g of iron react with excess sulfuric acid? 5.5g Fe 1mol Fe 1mol Fe2(SO4)3 400 g = 19.6 g Fe2(SO4)3 56 g 2mole Fe 1mol Fe2(SO4)3

  28. What volume of hydrogen gas, at STP, will be formed if 10.0g of iron(III) sulfate is formed?

  29. What volume of hydrogen gas, at STP, will be formed if 10.0g of iron(III) sulfate is formed? 10.0g Fe2(SO4)3 1mole Fe2(SO4)3 3molesH2 22.4L = 1.68 L H2 400 g 1mole Fe2(SO4)3 1molesH2

  30. 4. When solid calcium nitride is heated at high temperatures, solid calcium and nitrogen gas are produced. • a. Write and balance the reaction that occurs. • b. Identify the reaction type.

  31. 4. When solid calcium nitride is heated at high temperatures, solid calcium and nitrogen gas are produced. • a. Write and balance the reaction that occurs. Ca3N2 → 3Ca + N2 • b. Identify the reaction type. • Decomposition

  32. c. What mass of calcium nitride must decompose in order to form 10.25g of calcium?

  33. c. What mass of calcium nitride must decompose in order to form 10.25g of calcium? 10.25g Ca 1mol Ca 1mol Ca3N2 148 g = 12.6 g Ca3N2 40g 3mol Ca 1mol Ca3N2

  34. d. What mass of calcium will be produced if 13.5g of nitrogen are produced?

  35. d. What mass of calcium will be produced if 13.5g of nitrogen are produced? 13.5g N2 1mol N2 3mols Ca 40g = 57.9 g Ca 28g 1mol N2 1mol Ca

  36. e. What volume of nitrogen, assuming the reaction is at STP, will be produced if 5.00g of calcium nitride decompose?

  37. e. What volume of nitrogen, assuming the reaction is at STP, will be produced if 5.00g of calcium nitride decompose? 5.00g Ca3N2 1mol Ca3N2 1mol N2 22.4L = .76 L N2 148 g 1mol Ca3N2 1mol N2

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