Chemistry 30

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Redox Reactions & Electrochemistry Practice

Practice Set 3: Balancing Redox Reactions

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  1. Balance the following redox reactions using the oxidation number method.

a. SnCl2 + HgCl2 → SnCl4 + HgCl

       
balance for electrons
   

 

initial

 

final

change

 

Coefficient

 

Total e-

Sn

 

   

×

 

=

 

Hg

 

   

×

 

=

 

Answer:

 

b. HNO3 + H2S → NO + S + H2O

       
balance for electrons

   

 

initial

 

final

change

 

Coefficient

 

Total e-

N

 

   

×

 

=

 

S

 

   

×

 

=

 

Answer:

 

c. NaClO + H2S → NaCl + H2SO4

       
balance for electrons

   

 

initial

 

final

change

 

Coefficient

 

Total
e-

Cl

 

   

×

 

=

 

S

 

   

×

 

=

 

Answer:

 

d. CdS + I2 + HCl → CdCl2 + HI + S

Because one of the atoms undergoing oxidation or reduction has a subscript (I2) we will account for the number of atoms of each element when preparing our summary chart:

               
balance for electrons

   

 

initial

 

final

change

 

no. atoms

 

No.
e -

 

Coefficient

 

Total e-

S

 

   

 

 

 

 

×

 

=

 

I

 

   

×


(in I2)

=

 

×

 

=

 

Answer:

 

e. I2 + HNO3 → HIO3 + NO2 + H2O

Once again, because one of the atoms undergoing oxidation or reduction has a subscript (I2) we will account for the number of atoms of each element when preparing our summary chart:

               
balance for electrons

   

 

initial

 

final

change

 

no. atoms

 

No.
e -

 

Coefficient

 

Total
e -

I

 

   

×


(in I2)

 

 

×

 

=

 

N

 

   

 

 

=

 

×

 

=

 

Answer:

 

f. MnO4- + H+ + Cl- → Mn2+ + Cl2 + H2O

    Make your own summary chart

  1. Balance the following half-reactions for both atoms and electrons by adding the appropriate number of electrons to the correct side of the equation. Also identify each as either an oxidation or reduction.
    Add electrons to the equation Oxidation
or
Reduction?
a. Pb2+ → Pb    
b. Cl2 → Cl-    
c. Fe3+ → Fe2+    
d. N2O + H2O → NO + H+    
  1. Break each equation into two half-reactions. Identify each half-reaction as oxidation or reduction.
a. Cu + 2 H+ → Cu2+ + H2  
    oxidation
    reduction
b. 2 Al + 3 S → Al2S3  
    oxidation
    reduction
  1. Balance the following equations using the half-reaction method.

a. Na + Br2 → NaBr

Step 1

Step 2

Step 3

Write the two balanced half-reactions, removing any spectator ions:

Balance for electrons

Add the half-reactions, replacing any spectator ions that were removed and/or recombining compounds

space

space

space

 

 

space

spaceadd together:

 

reform compound:

b. Zn + S → ZnS

Step 1

Step 2

Step 3

Write the two balanced half-reactions, removing any spectator ions:

Balance for electrons

Add the half-reactions, replacing any spectator ions that were removed and/or recombining compounds

     
     

added together:

 

reform compound:

c. Ag + Cr2O72- + H+ → Ag+ + Cr3+ + H2O

For each half-reaction, remember to balance for atoms first, then add electrons to balance for charge.

Step 1

Step 2

Step 3

Write the two balanced half-reactions, removing any spectator ions:

Balance electrons

Add the half-reactions, replacing any spectator ions that were removed and/or recombining compounds

   
   
added together:  

reform compound:

   

Check Answers

Return to Notes

 

Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 22-May-2006