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The balanced equation of 4Al + 3O 2 → 2Al 2 O 3 can be interpreted by saying that 1 mol of Al:

The balanced equation of 4Al + 3O 2 → 2Al 2 O 3 can be interpreted by saying that 1 mol of Al:. 8.1. Reacts with 3 mol of O 2 Produces 1 mol of Al 2 O 3 Produces 0 . 5 mol Al 2 O 3 Reacts with 2 mol of O 2 Cannot react with O 2.

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The balanced equation of 4Al + 3O 2 → 2Al 2 O 3 can be interpreted by saying that 1 mol of Al:

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  1. The balanced equation of 4Al + 3O2→ 2Al2O3 can be interpreted by saying that 1 mol of Al: 8.1 Reacts with 3 mol of O2 Produces 1 mol of Al2O3 Produces 0.5 mol Al2O3 Reacts with 2 mol of O2 Cannot react with O2

  2. The balanced equation of 4Al + 3O2→ 2Al2O3 can be interpreted by saying that 1 mol of Al: 8.1 Reacts with 3 mol of O2 Produces 1 mol of Al2O3 Produces 0.5 mol Al2O3 Reacts with 2 mol of O2 Cannot react with O2

  3. How many moles of oxygen are needed to produce 6 mol of Fe2O3 in the following equation: 4Fe + 3O2→ 2Fe2O3? 8.2 3 1 6 9 18

  4. How many moles of oxygen are needed to produce 6 mol of Fe2O3 in the following equation:4Fe + 3O2→ 2Fe2O3? 8.2 3 1 6 9 18

  5. How many moles of gaseous oxygen are required for the complete combustion of 4.0 mol of butane (C4H10)? 8.3 4.0 8.0 13 26 52

  6. How many moles of gaseous oxygen are required for the complete combustion of 4.0 mol of butane (C4H10)? 8.3 4.0 8.0 13 26 52

  7. How many grams of oxygen are required to completely burn 5.90 g of C3H8in the following unbalanced equation: C3H8(g) + O2(g) → CO2(g) + H2O(g)? 8.4 5.90 g 21.4 g 4.28 g 10.7 g 29.5 g

  8. How many grams of oxygen are required to completely burn 5.90 g of C3H8in the following unbalanced equation: C3H8(g) + O2(g) → CO2(g) + H2O(g)? 8.4 5.90 g 21.4 g 4.28 g 10.7 g 29.5 g

  9. How many grams of aluminum sulfate are produced from 2.67 mol sulfuric acid in the following unbalanced equation: Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)? 8.5 305 g 457 g 272 g 914 g 342 g

  10. How many grams of aluminum sulfate are produced from 2.67 mol sulfuric acid in the following unbalanced equation: Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)? 8.5 305 g 457 g 272 g 914 g 342 g

  11. How many moles of phosphorus are required to produce 15.5 g P4O6 in the following equation:4P(s) + 3O2(g) → P4O6(s)? 8.6 34.9 mol 0.0703 mol 4.00 mol 2.18 mol 0.282 mol

  12. How many moles of phosphorus are required to produce 15.5 g P4O6 in the following equation:4P(s) + 3O2(g) → P4O6(s)? 8.6 34.9 mol 0.0703 mol 4.00 mol 2.18 mol 0.282 mol

  13. How many moles of oxygen gas are produced from the following decomposition of 3.0 mol of Al2O3, assuming a 85% yield: 2Al2O3→ 4Al + 3O2? 8.7 4.5 mol 3.8 mol 5.3 mol 3.0 mol 4.2 mol

  14. How many moles of oxygen gas are produced from the following decomposition of 3.0 mol of Al2O3, assuming a 85% yield: 2Al2O3→ 4Al + 3O2 ? 8.7 4.5 mol 3.8 mol 5.3 mol 3.0 mol 4.2 mol

  15. How many kg of methane (CH4) are produced from 25.0 kg of hydrogen in the following catalytic methanation: 3H2 + CO → CH4+ H2O? 8.8 115 kg 74.3 kg 134 kg 25.0 kg 66.2 kg

  16. How many kg of methane (CH4) are produced from 25.0 kg of hydrogen in the following catalytic methanation: 3H2 + CO → CH4+ H2O? 8.8 115 kg 74.3 kg 134 kg 25.0 kg 66.2 kg

  17. How many moles of water are produced from the combustion of 3.5 mol of hydrogen and 5.2 mol of oxygen? 8.9 7.0 mol 5.2 mol 3.5 mol 10. mol 1.8 mol

  18. How many moles of water are produced from the combustion of 3.5 mol of hydrogen and 5.2 mol of oxygen? 8.9 7.0 mol 5.2 mol 3.5 mol 10. mol 1.8 mol

  19. How many grams of NO are produced from the oxidation of 14.5 g of NH3 by 12.2 g of O2 in the following equation: 4NH3 + 5O2→ 4NO + 6H2O? 8.10 0.305 g 25.5 g 18.3 g 9.15 g 0.851 g

  20. How many grams of NO are produced from the oxidation of 14.5 g of NH3 by 12.2 g of O2 in the following equation: 4NH3 + 5O2→ 4NO + 6H2O? 8.10 0.305 g 25.5 g 18.3 g 9.15 g 0.851 g

  21. How many grams of the excess reagent are left over after the reaction of 4.36 g of Al and 8.50 g HCl in the following unbalanced equation:Al + HCl → AlCl3 + H2? 8.11 2.26 g 4.14 g 2.3 g 21.5 g 10.4 g

  22. How many grams of the excess reagent are left over after the reaction of 4.36 g of Al and 8.50 g HCl in the following unbalanced equation:Al + HCl → AlCl3 + H2? 8.11 2.26 g 4.14 g 2.3 g 21.5 g 10.4 g

  23. How many molecules of water are produced from the combustion of 2.56 mol of octane in the following equation:2C8H18+ 25O2→ 16CO2 + 18H2O? 8.12 1.08 x 1025 2.77 x 1025 2.56 x 1025 1.39 x 1025 6.02 x 1023

  24. How many molecules of water are produced from the combustion of 2.56 mol of octane in the following equation:2C8H18+ 25O2→ 16CO2 + 18H2O? 8.12 1.08 x 1025 2.77 x 1025 2.56 x 1025 1.39 x 1025 6.02 x 1023

  25. How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation: 2H2O2→ 2H2+ O2? 8.13 8.75 x 1024 7.74 x 1022 1.55 x 1022 5.27 x 1024 6.02 x 1023

  26. How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation: 2H2O2→ 2H2+ O2? 8.13 8.75 x 1024 7.74 x 1022 1.55 x 1022 5.27 x 1024 6.02 x 1023

  27. How many molecules of ammonia are produced from 7.54 x 1025 molecules of hydrogen in the following equation: 3H2 + N2→ 2NH3? 8.14 2 molecules 7.54 x 1025 molecules 5.03 x 1025 molecules 1.51 x 1026 molecules 6.02 x 1023 molecules

  28. How many molecules of ammonia are produced from 7.54 x 1025 molecules of hydrogen in the following equation: 3H2 + N2→ 2NH3? 8.14 2 molecules 7.54 x 1025 molecules 5.03 x 1025 molecules 1.51 x 1026 molecules 6.02 x 1023 molecules

  29. How many molecules of CO2 are produced from the combustion of 2 molecules of C8H18 and 5 molecules of O2? (Hint: This is a tricky question.) 8.15 1.93 x 1024 molecules 16 molecules 9.63 x 1024molecules 3 molecules 3.2 x 1024molecules

  30. How many molecules of CO2 are produced from the combustion of 2 molecules of C8H18 and 5 molecules of O2? (Hint: This is a tricky question.) 8.15 1.93 x 1024 molecules 16 molecules 9.63 x 1024molecules 3 molecules 3.2 x 1024molecules

  31. What is the theoretical yield of acetic acid when 22.5 g of methanol reacts with 32.0 g of carbon monoxide in the following equation:CH3OH + CO → HC2H3O2? 8.16 24.2 g 32.0 g 42.2 g 68.6 g 84.4 g

  32. What is the theoretical yield of acetic acid when 22.5 g of methanol reacts with 32.0 g of carbon monoxide in the following equation:CH3OH + CO → HC2H3O2? 8.16 24.2 g 32.0 g 42.2 g 68.6 g 84.4 g

  33. What is the theoretical yield of SO3 from the combustion of 3.00 mol of S and 6.00 mol of O2? 8.17 3.00 g 320. g 2.00 g 4.00 g 240. g

  34. What is the theoretical yield of SO3 from the combustion of 3.00 mol of S and 6.00 mol of O2? 8.17 3.00 g 320. g 2.00 g 4.00 g 240. g

  35. What is the theoretical yield of MgO from the combustion of 5.25 x 1023 atoms of Mg and 4.69 x 1023 molecules of O2? 8.18 35.1 g 2.17 x 1025g 31.4 g 3.78 x 1025g 62.8 g

  36. What is the theoretical yield of MgO from the combustion of 5.25 x 1023 atoms of Mg and 4.69 x 1023 molecules of O2? 8.18 35.1 g 2.17 x 1025g 31.4 g 3.78 x 1025g 62.8 g

  37. Which reactant is in excess from the reaction of 35.0 g of hydrogen with 276 g of oxygen to form water? 8.19 H O O2 H2 H2O

  38. Which reactant is in excess from the reaction of 35.0 g of hydrogen with 276 g of oxygen to form water? 8.19 H O O2 H2 H2O

  39. Which of the following statements is NOT correct about the limiting reactant in a reaction? 8.20 It has the lowest mass. Its coefficient in the balanced equation is the smallest one. It has the highest mass. It doesn’t react completely. All of the above

  40. Which of the following statements is NOT correct about the limiting reactant in a reaction? 8.20 It has the lowest mass. Its coefficient in the balanced equation is the smallest one. It has the highest mass. It doesn’t react completely. All of the above

  41. In the combustion of a sample of methane, the theoretical yield is 28.9 g CO2. When a chemistry student performed the experiment, the yield was 26.4 g CO2. What is the percent yield of their reaction by the student? 8.21 100. % 91.3 % 109 % 85.2 % 55.9 %

  42. In the combustion of a sample of methane, the theoretical yield is 28.9 g CO2. When a chemistry student performed the experiment, the yield was 26.4 g CO2. What is the percent yield of their reaction by the student? 8.21 100. % 91.3 % 109 % 85.2 % 55.9 %

  43. An experiment had a percent yield of 91.8% and a calculated theoretical yield of 28.2 g. How many grams were actually produced? 8.22 25.9 g 2.50 g 92.0 g 28.5 g 30.7 g

  44. An experiment had a percent yield of 91.8% and a calculated theoretical yield of 28.2 g. How many grams were actually produced? 8.22 25.9 g 2.50 g 92.0 g 28.5 g 30.7 g

  45. What is the limiting reactant for the reaction between 18.2 g of K and 8.38 g of water in the following unbalanced reaction:K + H2O → KOH + H2? 8.23 K H2O KOH H2 Both are used up at the same time.

  46. What is the limiting reactant for the reaction between 18.2 g of K and 8.38 g of water in the following unbalanced reaction:K + H2O → KOH + H2? 8.23 K H2O KOH H2 Both are used up at the same time.

  47. 5.0 kg of hydrogen is reacted with 31 kg of oxygen. The experiment yields 28 kg of water. Calculate the percent yield of the reaction. 8.24 40. % 63 % 80. % 90. % 161%

  48. 5.0 kg of hydrogen is reacted with 31 kg of oxygen. The experiment yields 28 kg of water. Calculate the percent yield of the reaction. 8.24 40. % 63 % 80. % 90. % 161%

  49. 4.25 mol of Cl2 are reacted with 1.49 mol NaOH. 12.5 g of NaClO3 are produced. Calculate the percent yield of the following reaction: 3Cl2 + 6 NaOH → 5 NaCl + NaClO3 + 3H2O. 8.25 28.1% 47.3% 79.9% 82.8% 91.2%

  50. 4.25 mol of Cl2 are reacted with 1.49 mol NaOH. 12.5 g of NaClO3 are produced. Calculate the percent yield of the following reaction: 3Cl2 + 6 NaOH → 5 NaCl + NaClO3 + 3H2O. 8.25 28.1% 47.3% 79.9% 82.8% 91.2%

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