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

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Presentation on theme: "Last night’s homework: Problems 4-6 on page 282 Questions 7-11 on page 283."— Presentation transcript:

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

4

5 FeCl 3 + NaOH → Fe(OH) 3 + NaCl

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

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

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

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

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

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

12

13 Fe Cl Na O H Fe Cl Na O H

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

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

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

17 FeCl 3 + NaOH → Fe(OH) 3 + 3NaCl Fe 1 Cl 3 Na 1 O 1 H 1 Fe 1 Cl 3 Na 3 O 3 H 3

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

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

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

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

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

23 CS 2 + O 2 → CO 2 + SO 2

24

25 COSCOS COSCOS

26 C 1 O 4 S 1 C 1 O 2 S 2

27 CS 2 + O 2 → CO 2 + 2SO 2 C 1 O 4 S 1 C 1 O 2 S 2

28 CS 2 + O 2 → CO 2 + 2SO 2 C 1 O 6 S 2 C 1 O 2 S 2

29 CS 2 + 3O 2 → CO 2 + 2SO 2 C 1 O 6 S 2 C 1 O 2 S 2

30 CS 2 + 3O 2 → CO 2 + 2SO 2 C 1 O 6 S 2 C 1 O 6 S 2

31 CS 2 + 3O 2 → CO 2 + 2SO 2 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 Zn + H 2 SO 4 → H 2 + ZnSO 4

34 Zn H S O Zn H S O

35 Zn + H 2 SO 4 → H 2 + ZnSO 4 Zn 1 H 2 S 1 O 4 Zn 1 H 2 S 1 O 4

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

37 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. 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.

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

43 No

44 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula? No H 2 O → H 2 + O 2

45 10. When balancing a chemical equation, can you adjust the number that is subscripted to a substance formula? No H 2 O → H 2 + O 2 H 2 O 2 → H 2 + O 2

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..


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