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Ch.5 Classification & Balancing of Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Chemical Reaction: Chemical Change
Law of Conservation of Mass
Balancing Chemical Equations (Simplified)
Solubility Rules
Molecular Equations
Types of Chemical Reactions
Complete Ionic Equations
Calculate Oxidation Numbers
Redox Reactions
Spontaneous Redox Reactions
Balancing Redox Reactions: Acidic Solutions
Balancing Redox Reactions: Basic Solutions
Balancing Redox Reactions (Simplified)
Galvanic Cell (Simplified)

Concept #1: Galvanic Cell (Voltaic Cell)

Example #1: The purpose of a galvanic cell is to: 

a) Purify solids              b) Allow for only oxidation          

c) Generate electricity      d) To consume electricity

Example #2: How many electrons are transferred between the zinc and copper electrodes in the galvanic cell? 

a) 1                  b) 2                  c) 3                      d) 4

Concept #2: Electrolytic Cell

Example #3: : Identify the location within an electrolytic cell where the loss of electrons will occur. 

a) Cathode      b) Anode        c) Salt Bridge        d) Electrode       e) Voltmeter 

Concept #3: Understanding Electrolytic Cell

Example #4: Which of the following is true about an electrolytic cell?

a) It changes chemical energy into electrical energy.

b) It uses a positive cathode. 

c) It uses an electrical current to make a nonspontaneous reaction go.

d) All of the above.

Practice: Which of the following statements is true for a salt bridge?

Practice: Which of the following statements is TRUE for a voltaic cell, but FALSE for an electrolytic cell?

I. The flow of electrons is spontaneous.
II. Oxidation occurs at the anode.
III. Electrons flow from the anode to the cathode.

Practice: What is the balanced half reaction that occurs at the anode in the overall cell reaction of a voltaic cell?

3 MnO4(aq) + 5 Fe(s) → 3 Mn2+(aq) + 5 Fe3+(aq)