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Ch12.1 - Stoichiometry

Ch12.1 - Stoichiometry. N 2(g) + H 2(g) NH 3(g). Ch12.1 - Stoichiometry. 1 N 2(g) + 3 H 2(g) 2 NH 3(g) 1 mole reacts with 3 moles to produce 2 moles Masses: 2 N @ 14.0 = 28.0 g/mol 2 H @ 1.0 = 2.0 g/mol 1 N @ 14.0 = 14.0 3 H @ 1.0 = 3.0

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Ch12.1 - Stoichiometry

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  1. Ch12.1 - Stoichiometry • N2(g) + H2(g) NH3(g)

  2. Ch12.1 - Stoichiometry • 1N2(g) + 3H2(g)2NH3(g) • 1 mole reacts with 3 moles to produce 2 moles • Masses: • 2 N @ 14.0 = 28.0 g/mol • 2 H @ 1.0 = 2.0 g/mol • 1 N @ 14.0 = 14.0 • 3 H @ 1.0 = 3.0 • 17.0 g/mol How many moles of NH3 produced? - 2 mol of N2 react? - 1½ mol of H2 react? - 28 g of N2 react?

  3. Ex1) Calculate the # of moles of nitrogen required to make 7.24 moles of ammonia. N2 + 3 H2 2 NH3 HW#1) Given 4 Al + 3 O2 2 Al2O3 How many moles of Al are needed to form 3.7 mol of Al2O3? b) How many moles of O2 are required to react completely with 14.8 moles of Al?

  4. Ex1) Calculate the # of moles of nitrogen required to make 7.24 moles of ammonia. N2 + 3 H2 2 NH3 ? moles 7.24 moles 7.24 moles NH3 1 moles N2 2moles NH3 = 3.62 moles N2 HW#1) Given 4 Al + 3 O2 2 Al2O3 ? Mol 3.7 mol How many moles of Al are needed to form 3.7 mol of Al2O3? 3.7 mol Al2O3 4 mol Al 2 mol Al2O3 = 7.4 mol Al b) How many moles of O2 are required to react completely with 14.8 moles of Al? 14.8 mol Al 3 mol O2 4 mol Al = 11.1 mol O2

  5. Mass – Mass Calcs Ex2) Calculate the # of grams of NH3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N2(g) + 3 H2(g) 2 NH3(g) Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH3 needed for the reaction? N2(g) + 3 H2(g) 2 NH3(g)

  6. Mass – Mass Calcs Ex2) Calculate the # of grams of NH3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N2(g) + 3 H2(g) 2 NH3(g) 5.40 H2 1 mol H2 2 mol NH2 17.0g NH3 2.0 g H2 3 mol H2 1 mol NH3 = 30.6g NH3 Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH3 needed for the reaction? N2(g) + 3 H2(g) 2 NH3(g) 30.6g NH3 1 mol NH3 1 mol N2 28.0g N2 17.0 g NH3 2 mol NH3 1 mol N2 = 25.2g N2

  7. HW#2) CaC2(s) + H2O C2H2(g) + Ca(OH)2(aq) a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced?

  8. HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq) a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O 1 mol CaC2 18.0g H2O 2 mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced?

  9. HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq) a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O 1 mol CaC2 18.0g H2O 2 mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? 5.00g CaC2 1 mol CaC2 1 mol C2H2 26.0g C2H2 52.1g CaC2 1 mol CaC2 1 mol C2H2 = 2.49g C2H2 c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced? CH 12 HW#1 1-3

  10. HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq) a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O 1 mol CaC2 18.0g H2O 2 mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? 5.00g CaC2 1 mol CaC2 1 mol C2H2 26.0g C2H2 52.1g CaC2 1 mol CaC2 1 mol C2H2 = 2.49g C2H2 c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced? .89 mol C2H2 1 mol Ca(OH)2 74.1g Ca(OH)2 1 mol C2H2 1 mol Ca(OH)2 = 66.0g Ca(OH)2 CH 12 HW#1 1-3

  11. Ch12 HW#1 1-3 3) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : H2O: b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O

  12. Ch12 HW#1 1-3 3) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO2 44.0g CO2 26.0 g C2H2 2 mol C2H2 1 mol CO2 = 176 g CO2 H2O: b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O

  13. Ch12 HW#1 1-3 3) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO2 44.0g CO2 26.0 g C2H2 2 mol C2H2 1 mol CO2 = 176 g CO2 H2O: 52.0g C2H2 1 mol C2H2 2 mol H2O 18.0g H2O 26.0 g C2H2 2 mol C2H2 1 mol H2O = 36.0g H2O b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O

  14. Ch12 HW#1 1-3 3) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO2 44.0g CO2 26.0 g C2H2 2 mol C2H2 1 mol CO2 = 176 g CO2 H2O: 52.0g C2H2 1 mol C2H2 2 mol H2O 18.0g H2O 26.0 g C2H2 2 mol C2H2 1 mol H2O = 36.0g H2O b) How many grams O2 to burn 52.0g C2H2? 52.0g C2H2 1 mol C2H2 5 mol O2 32.0g O2 26.0 g C2H2 2 mol C2H2 1 mol O2 = 160g O2 c) 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O 52.0g + 160g = 176g + 36g

  15. Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 5) Glucose (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose?

  16. Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 2 Al + 6 HCl 2 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose?

  17. Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 2 Al + 6 HCl 2 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose? C6H12O6 + 6 O2 6 CO2 + 6 H2O .25mol ?mol .25mol C6H12O6 6molHCl 1mol CHO = 1.5mol O2

  18. 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation:Li3N + 3 H2O NH3 + 3 LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine?

  19. 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation:Li3N + 3 H2O NH3 + 3 LiOH .38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH 35.0g Li3N 1mol Li3N 1mol LiOH = .78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine?

  20. 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation:Li3N + 3 H2O NH3 + 3 LiOH .38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH 35.0g Li3N 1mol Li3N 1mol LiOH = .78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine? Cl2 + 2 NaI 2 NaCl + I2 .29g NaI 1 molNaI2 mol NaCl 58.5g NaCl 150.0g NaI2 mol NaI1 mol NaCl = .112g NaCl

  21. 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C4H10 + 13 O2 8 CO2 + 10 H2O 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O3 + 3 C 2 Sb + 3 CO

  22. 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C4H10 + 13 O2 8 CO2 + 10 H2O 0.85g C4H10 1mol C4H10 8mol CO2 44.0g CO2 58.0g C4H10 2mol C4H10 1mol CO2 = _____g CO2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O3 + 3 C 2 Sb + 3 CO

  23. 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C4H10 + 13 O2 8 CO2 + 10 H2O 0.85g C4H10 1mol C4H10 8mol CO2 44.0g CO2 58.0g C4H10 2mol C4H10 1mol CO2 = _____g CO2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O3 + 3 C 2 Sb + 3 CO .46g Sb2O3 1 mol Sb2O3 2 mol Sb 121.8g Sb 291.6g Sb2O3 1 mol Sb2O3 1 mol Sb = .38g Sb

  24. 10) What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77g of water? H2O2 H2O + O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

  25. 10) What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77g of water? H2O2 H2O + O2 0.77g H2O 1 mol H2O 2 mol H2O2 34.0g H2O2 18.0g H2O 2 mol H2O 1 mol H2O2 = ____g H2O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

  26. 10) What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77g of water? H2O2 H2O + O2 0.77g H2O 1 mol H2O 2 mol H2O2 34.0g H2O2 18.0g H2O 2 mol H2O 1 mol H2O2 = ____g H2O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide? CO + O2 CO2 0.69 CO2 1 mol CO2 2 mol CO 28.0g CO 44.0g CO2 2 mol CO2 1 mol CO = 0.44g CO

  27. 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC2 + H2O Ca(OH)2 + C2H2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? __O3 __O2

  28. 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC2 + 2 H2O Ca(OH)2 + C2H2 .64g H2O 1 mol H2O 1 mol Ca(OH)2 74.1g Ca(OH)2 18.0 g H2O 2 mol H2O 1 mol Ca(OH)2 = 1.32g Ca(OH)2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? __O3 __O2

  29. 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC2 + 2 H2O Ca(OH)2 + C2H2 .64g H2O 1 mol H2O 1 mol Ca(OH)2 74.1g Ca(OH)2 18.0 g H2O 2 mol H2O 1 mol Ca(OH)2 = 1.32g Ca(OH)2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? 2 O3 3 O2 .87g O2 1 mol O2 2 mol O3 48.0g O3 32.0g O2 3 mol O2 1 mol O3 = .87g O3

  30. Ch12.3 – More Stoichiometry Ex1) How many molecules of oxygen are produced when 29.2g of water is decomposed? Ex2) Assuming STP, how many liters of oxygen are needed to produce 19.8 L of SO3? Ex3) How many mls of nitrogen dioxide are produced when 3.4 ml of oxygen react with an excess of nitrogen monoxide? Assume STP.

  31. Ch12.3 – More Stoichiometry Ex1) How many molecules of oxygen are produced when 29.2g of water is decomposed? 2 H2O2 H2(g) + O2(g) Ex2) Assuming STP, how many liters of oxygen are needed to produce 19.8 L of SO3? 2 SO2 + O2 2 SO3 Ex3) How many mls of nitrogen dioxide are produced when 3.4 ml of oxygen react with an excess of nitrogen monoxide? Assume STP. O2 + 2 NO 2 NO2 Ch12 HW#3 14

  32. Lab 12.1 Quantitative Analysis Data Analysis 1) Mass of Fe lost by nails: Δmass = Fe(before) – Fe(after) = ____ g Fe 2) Moles of Fe: Δmass of Fe = g Fe 1 mole Fe 55.8g Fe = ___ mol Fe 3) Mass of Cu produced: (mass of beaker + product) – (mass of beaker) = ___ g Cu 4) Moles of Cu: Mass Cu produced = g Cu 1 mol Cu 63.5 g Cu = ___ mol Cu 5) Mole Ratio: ___ mol Fe ___ mol Cu ___Fe + ___CuCl2 ___FeCl3 + ___Cu

  33. Lab12.1 – Mass – Mass Conversions - lab due in 2 days - Ch12 HW#3 due at beginning of period

  34. Ch12 HW#3 14 Sn(s) + 2 HF(g) SnF2 + H2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x1024 molecules ?g a) b) c)

  35. Ch12 HW#3 14 Sn(s) + 2 HF(g) SnF2 + H2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x1024 molecules ?g 9.40L H2 1 mol H2 2 mol HF 22.4L HF 22.4L H2 1 mol H2 1 mol HF = 18.8L b) c)

  36. Ch12 HW#3 14 Sn(s) + 2 HF(g) SnF2 + H2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x1024 molecules ?g 9.40L H2 1 mol H2 2 mol HF 22.4L HF 22.4L H2 1 mol H2 1 mol HF = 18.8L 20.0 L HF 1 mol HF 1 mol H2 6.02x1023 molecules H2 22.4L HF 2 mol HF 1 mol H2 = 2.69x1023 molecules c)

  37. Ch12 HW#3 14 • Sn(s) + 2 HF(g) SnF2 + H2(g) • a) ? L 9.40 L • b) 20.0 L ? molecules • c) 7.42x1024 molecules ?g • 9.40L H2 1 mol H2 2 mol HF 22.4L HF • 22.4L H2 1 mol H2 1 mol HF = 18.8L • 20.0 L HF 1 mol HF 1 mol H2 6.02x1023 molecules H2 • 22.4L HF 2 mol HF 1 mol H2 • = 2.69x1023 molecules • 7.42x1024 • molecules HF 1 mol HF 1 mol SnF2 156.7g SnF2 • 6.02x1023 2 mol HF 1 mol SnF2 • molecules HF = 967g SnF2

  38. Ch12 HW#4 15 – 20 15. 20.0g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. How many liters would the hydrogen gas occupy at STP? 16. If 30.2 of aluminum react with HCL to produce aluminum chloride and hydrogen gas, how many liters of hydrogen are produced at STP?

  39. Ch12 HW#4 15 – 20 15. 20.0g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. How many liters would the hydrogen gas occupy at STP? K + H2O KOH + H2 16. If 30.2 of aluminum react with HCL to produce aluminum chloride and hydrogen gas, how many liters of hydrogen are produced at STP? Al + HCl AlCl3 + 3 H2

  40. 17. How many liters of HCL are produced by the reaction of 5.7L of hydrogen with an equal amount of chlorine? 18. How many liters of hydrogen are required to react with 0.45 mol of oxygen to produce water?

  41. 17. How many liters of HCL are produced by the reaction of 5.7L of hydrogen with an equal amount of chlorine? H2 + Cl2HCl 18. How many liters of hydrogen are required to react with 0.45 mol of oxygen to produce water? H2 + O2 H2O Ch12 HW#4 19,20 for HW

  42. 19. How many liters of SO2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O2 SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl2 ZnCl2

  43. 19. How many liters of SO2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O2 SO2 26.9L O2 1 mol O2 1 molSO2 22.4L SO2 22.4L O2 1 mol O2 1 mol SO2 = 26.9L SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl2 ZnCl2

  44. 19. How many liters of SO2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O2 SO2 26.9L O2 1 mol O2 1 molSO2 22.4L SO2 22.4L O2 1 mol O2 1 mol SO2 = 26.9L SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl2 ZnCl2 16.8L Cl2 1 mol Cl2 1 mol ZnCl2 136.4g ZnCl2 22.4L Cl2 1 mol Cl2 1 mol ZnCl2 = 102.3g ZnCl2

  45. Ch12 Mid Chapter Review 1. In Lab12.1 you reacted 2 iron nails with copper (II) chloride. If the nails massed at 4.25g, and there was enough CuCl2 to completely dissolve the nails, what mass of copper would be produced? ___Fe + ___CuCl2 ___Cu + ___FeCl3 2. In ch11, magnesium reacted with carbon dioxide to produce magnesium oxide, carbon, and lots of bright light! How many molecules of carbon dioxide are required to react with 2.50g of Mg?

  46. 3. If lead wasn’t so dangerous for the environment, we would decompose 3.00g of PbCO3.Pb(OH)2 to obtain CO2. What volume should be produced? 2 PbCO3.Pb(OH)2 3PbO + H2O + 2 CO2

  47. Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl2 2 FeCl3 + 3 Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg + CO2 2 MgO + C

  48. Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl2 2 FeCl3 + 3 Cu 1.00g Fe 1 mol Fe 3 mol Cu 63.5g Cu 55.8g Fe 2 mol Fe 1 mol Cu = 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg + CO2 2 MgO + C

  49. Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl2 2 FeCl3 + 3 Cu 1.00g Fe 1 mol Fe 3 mol Cu 63.5g Cu 55.8g Fe 2 mol Fe 1 mol Cu = 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg + CO2 2 MgO + C 12.04x1023 6.02x1023 atoms Mg 1 mol Mg 1 mol CO2 molecules CO2 6.02x1023 2 mol CO2 1 mol CO2 = 6.02x1023 atoms Mg molecules CO2

  50. 3. What volumes of CO2 should be produced if 4.00 g of lead carbonate decompose? 2PbCO3 Pb(OH)3 3 PbO + H2O + 2 CO2

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