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- 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
- 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.
Make your own summary chart
Add electrons to the equation | Oxidation or Reduction? |
||
a. | Pb2+ → Pb | ||
b. | Cl2 → Cl- | ||
c. | Fe3+ → Fe2+ | ||
d. | N2O + H2O → NO + H+ |
- 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
- 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
add 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: