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Last night’s homework:

Last night’s homework:. Problems 4-6 on page 282 Questions 7-11 on page 283. Write chemical equations for each of the following reactions. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.

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Last night’s homework:

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  1. Last night’s homework: Problems 4-6 on page 282 Questions 7-11 on page 283

  2. Write chemical equations for each of the following reactions.

  3. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.

  4. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.

  5. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3 + NaCl

  6. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3 + NaCl

  7. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3 + NaCl

  8. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3 + NaCl

  9. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3+ NaCl

  10. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3+ NaCl

  11. In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride. FeCl3 + NaOH→ Fe(OH)3 + NaCl

  12. FeCl3 + NaOH → Fe(OH)3 + NaCl

  13. Fe Cl Na O H Fe Cl Na O H FeCl3 + NaOH→ Fe(OH)3 + NaCl

  14. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 1 Na 1 O 3 H 3 FeCl3 + NaOH→ Fe(OH)3 + NaCl

  15. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 1 Na 1 O 3 H 3 FeCl3 + NaOH→ Fe(OH)3 + NaCl

  16. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 1 Na 1 O 3 H 3 FeCl3 + NaOH→ Fe(OH)3 + 3NaCl

  17. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl3 Na 3 O 3 H 3 FeCl3 + NaOH→ Fe(OH)3 + 3NaCl

  18. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 3 Na 3 O 3 H 3 FeCl3 + NaOH→ Fe(OH)3 + 3NaCl

  19. Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 3 Na 3 O 3 H 3 FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

  20. Fe 1 Cl 3 Na 3 O 3 H 3 Fe 1 Cl 3 Na 3 O 3 H 3 FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

  21. Fe 1 Cl 3 Na 3 O 3 H 3 Fe 1 Cl 3 Na 3 O 3 H 3 FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

  22. 5. Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas.

  23. 5. Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas. CS2 + O2→ CO2 + SO2

  24. CS2 + O2→ CO2 + SO2

  25. C O S C O S CS2 + O2→ CO2 + SO2

  26. C 1 O 2 S 2 C 1 O 4 S 1 CS2 + O2→ CO2 + SO2

  27. C 1 O 2 S 2 C 1 O 4 S 1 CS2 + O2→ CO2 + 2SO2

  28. C 1 O 2 S 2 C 1 O 6 S 2 CS2 + O2→ CO2 + 2SO2

  29. C 1 O 2 S 2 C 1 O 6 S 2 CS2 + 3O2→ CO2 + 2SO2

  30. C 1 O 6 S 2 C 1 O 6 S 2 CS2 + 3O2→ CO2 + 2SO2

  31. C 1 O 6 S 2 C 1 O 6 S 2 CS2 + 3O2→ CO2 + 2SO2

  32. 6. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas and aqueous zinc sulfate.

  33. 6. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas and aqueous zinc sulfate. Zn+ H2SO4→ H2 + ZnSO4

  34. Zn H S O Zn H S O Zn+ H2SO4→ H2 + ZnSO4

  35. Zn 1 H 2 S 1 O 4 Zn 1 H 2 S 1 O 4 Zn+ H2SO4→ H2 + ZnSO4

  36. List three types of evidence that a chemical reaction has occurred.

  37. List three types of evidence that a chemical reaction has occurred. Changes in: • Temperature • Color Appearance of: • Odor • Gas bubbles • Solid precipitate

  38. 8. Compare and contrast a skeleton equation and a chemical equation.

  39. 8. Compare and contrast a skeleton equation and a chemical equation. Both show formulas of reactants and products. Chemical equation also shows relative amounts.

  40. 9. Why is it important that a chemical equation be balanced?

  41. 9. Why is it important that a chemical equation be balanced? Mass is neither created nor destroyed.

  42. 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula?

  43. 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula? No

  44. 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula? No H2O → H2 + O2

  45. 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula? No H2O → H2 + O2 H2O2 → H2 + O2

  46. 11. Why is it important that to reduce the coefficients in a balanced equation to the lowest possible whole-number ratio?

  47. 11. Why is it important that to reduce the coefficients in a balanced equation to the lowest possible whole-number ratio? Clearly shows the relative amounts. .

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