1. Balance the following half cell reaction:

1. MnO4- = Mn+2(acid)

2.  Zn = Zn+2

3.  NO3- = NH3 (acid)

4.  ClO3- = Cl-    (basic)

5. VO+2 = V+2 (acidic)

6.  Cr2O7-2= Cr+3(acidic)

Balance the following reactions.

1.  Fe+3 + Sn+2 = Fe+2 + Sn+4

2.  Cr2O7-2 + V+2 = Cr+3 + VO+2 (acidic)

3.  Cl2 = Cl- + ClO3-(basic)

4.  Cu  + NO3- = NO + Cu+2 (acidic)

5.  P2O5 + H2O = H3PO4

6. MnO4- + V+2= Mn+2 + VO2+1(acidic)
 
 

3. 22.5 ml of 0.16 N MnO4- = ___________wt of Fe (Fe+2/Fe+3).

4. 1.67 g of KMnO4 dissolved to make 360 ml of solution = _____________ N

5.Indicate the equivalent weight of each of the following substances that were weighed out.
 

Substance weighed out. Reaction:  Equivalent Weight
I2 I2 to I-
Fe(NH4)2(SO4)2(H2O)6 Fe+2 to Fe+3
Na2S2O3 S2O3-2 to S4O6-2
Na2C2O4 C2O4-2 to CO2

6. IO4- + 8 H+ + __________e- = I- + 4 H2O

a) 1 b) 5 c) 6 d) 7 e) 8

 7 What is the standard potential for a galvanic cell based on the reaction:
 
 

5 VO+2 + MnO4- + 11 H2O = 5 V(OH)4+ + Mn+2 + 2 H+
 
 

Could this reaction be used to analyze a sample for vanadium? Is the reaction spontaneous? How do you know?
 
 

8. 22.5 ml of 0.16 N MnO4-= ___________eq of Sn (Sn+2=Sn+4)

9. Draw how the physical construction of a cell that has a short hand representation would look:

Zn| Zn+2(aq) || Br2(l),Br-(aq)|C(graphite)

Indicate the direction of flow of the electrons in the wire and the flow of the ions in the salt bridge. Calculate the standard potential of the cell.