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

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

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

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

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

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

11. FeCl3 + NaOH → Fe(OH)3 + NaCl
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. FeCl3 + NaOH → Fe(OH)3 + NaCl

14. FeCl3 + NaOH → Fe(OH)3 + NaCl

15. FeCl3 + NaOH → Fe(OH)3 + NaCl

16. FeCl3 + NaOH → Fe(OH)3 + 3NaCl

17. FeCl3 + NaOH → Fe(OH)3 + 3NaCl

18. FeCl3 + NaOH → Fe(OH)3 + 3NaCl

19. FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

20. FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

21. 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. CS2 + O2 → CO2 + SO2 C O S C O S

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

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

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

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

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

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

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

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

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

37. Changes in: Temperature Color Appearance of: Odor Gas bubbles
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. Both show formulas of reactants and products.
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. Mass is neither created nor destroyed.
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. . Clearly shows the relative amounts.
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. .