Oxidation reduction reduction reactions.....help please?!

Question

1. What is the difference between an oxidizing agent and a reducing agent?

2. When first learning to balance equations, we learned that the number of atoms of each element in the products and reactants must be equivalent. What are some additional factors that must be taken into account when balancing equations for redox reactions?

3. What are half reactions?

4. What two aspects of the half-reaction equations must be balanced?

5. For the equation Ag NO3 - --> Ag NO

(Note: This reaction takes place in an acidic solution.)

Step 1: What substance is reduced?

Step 2: What substance is oxidized?

Step 3: What is the half reaction for oxidation?

Step 4: What is the half reaction for reduction?

Step 5: What is the net balanced equation?

Step 6: What is the reduced equation?

Answer 1

Do your own homework and pay attention in class please.

Answer 2

1. An oxidizing agent is a substance that oxidizes another species. The agent itself is reduced. Similarly, a reducing agent reduces another species; the agent itself is oxidized.

2. The number of electrons on both sides of the equation must balance as does the total charge.

3. A half-reaction shows either the oxidation or reduction process in a reaction.

4. See #2

5. Something is not right with this reaction.