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Balancing Oxidation-Reduction Equations
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Co2+ (aq) + Al(s) e)
Using the activity series provided, write the net ionic chemical equations for the following reactions. If no reaction occurs, simply write NR
2+ 0
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best reducing agents
best oxidizing agents
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Co2+ (aq) + Al(s)
Using the activity series provided, write the net ionic chemical equations for the following reactions. If no reaction occurs, simply write NR
2+ 0
Co (s) + Al3+ (aq)0 3+
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oxidation-reduction reactions
Co2+(aq) + Al(s) + Al3+(aq)Co (s)
Al 3+(aq) + 3e- Al(s) oxidation
Co(s)+ 2e- Co2+(aq)reduction
the number of electrons lost has to be equal to the number of electrons gained.
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oxidation-reduction reactions
Co2+(aq) + Al(s) + Al3+(aq)Co (s)
Al 3+(aq) + 3e- Al(s) oxidation
Co(s)+ 2e- Co2+(aq)reduction
the of electrons lost has to be equal to the number of electrons gained.
2( )
3( )
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oxidation-reduction reactions
Co2+(aq) + Al(s) + Al3+(aq)Co (s)
2Al 3+(aq) + 6e-
3Co(s)+ 6e-
Al(s) oxidation
Co2+(aq)reduction
the of electrons lost has to be equal to the number of electrons gained.
2
3
2( )
3( )
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3Co (s) + 2Al3+ (aq) 3Co2+ (aq) + 2Al(s)
2Al 3+(aq) + 6e- Al(s) oxidation
3Co(s)+ 6e- Co2+(aq)reduction
2
3
oxidation-reduction reactions
Adding the half reactions to gather gives us the overall redox reaction.
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Example
is this a redox reaction?
KMnO4 + FeSO4
*All species are (aq)
K2SO4 MnSO4Fe2(SO4 )3+ +
7+ 2+
3+ 2+
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Example
KMnO4 + FeSO4
*All species are (aq)
K2SO4 MnSO4Fe2(SO4 )3+ +
Balance the following equation ?
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Half-Reaction Method in Acid
1. Write the unbalanced equation in ionic form.
2. Separate the equation into two half-reactions.
3. Balance each half reaction (except for O and H).
5. Balance the charges by adding electrons.
4. In acid solution, balance O by adding H2O and H by adding H+
6. Add the half reactions
7. Check to make sure atoms and charges are balanced
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Example
Balance the following equation for the reaction in acid solution. *
KMnO4 + FeSO4
*All species are (aq)
K2SO4 MnSO4Fe2(SO4 )3+ +
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Example
Balance the following equation for the reaction in acid solution. *
MnO4- + Fe2+ Mn2+ + Fe3+
*All species are (aq)
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1. Write the unbalanced equation in ionic form.
MnO4- + Fe2+ Mn2+ + Fe3+
2. Separate the equation into two half-reactions
Fe2+ Fe3+
MnO4- Mn2+
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3. Balance each half reaction (except for O and H).
4. In acid solution, balance O by adding H2O and H by adding H+
Fe2+ Fe3+
MnO4- Mn2+8H++ 4H2O+
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5. Balance the charges by adding electrons.
Fe2+ Fe3+ + 1e-
MnO4- Mn2+8H++ 4H2O++ 5e-
5 x
1 x
You need the same number of electrons on both sides of the equation.
(
( )
)
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5. Balance the charges by adding electrons.
5Fe2+ 5Fe3+ + 5e-
MnO4- Mn2+8H++ 4H2O++ 5e-
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5Fe2+ 5Fe3+ + 5e-
MnO4- Mn2+8H++ 4H2O++ 5e-
MnO4-
Mn2+
8H++
4H2O ++
+ 5Fe2+
5Fe3+
6. Add the half reactions
This is the balanced equation
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Example
Balance the following equation for the reaction in basic solution. *
*All species are (aq)
HS- + NO3- S + NO2
-
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Half-Reaction Method in Base
1. Use the half-reaction method as specified for acidic solutions to obtain the final balanced equation as if H+ ions were present.
2. Add the number of OH- ions to both sides of the equation to turn the remaining H+ ions to H2O
3. Eliminate waters that appear on both sides of the equation.
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Example
Balance the following equation for the reaction in basic solution. *
*All species are (aq)
HS- S + H+
2H+ + + H2O
+ 2e-
2e- +
HS- + NO3- S + NO2
-
NO3- NO2
-
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Example
Balance the following equation for the reaction in basic solution. *
HS- S
NO3- NO2
-H+ + + H2O
HS- + NO3- S + NO2
-
NO3-H+ +HS- + NO2
- + H2O+ SOH- + + OH-
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Example
Balance the following equation for the reaction in basic solution. *
HS- S
NO3- NO2
-H+ + + H2O
HS- + NO3- S + NO2
-
NO3-H+ +HS- + NO2
- + H2O+ SOH- + + OH-
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Example
Balance the following equation for the reaction in basic solution. *
HS- S
NO3- NO2
-H+ + + H2O
HS- + NO3- S + NO2
-
NO3-HS- + NO2
- + H2O+ S + OH-H2O +
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Example
Balance the following equation for the reaction in basic solution. *
HS- + NO3- S + NO2
-
NO3-HS- + NO2
- + S + OH-
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Cr2O72- (aq) + I- (aq) a)
Complete and balance the following equations, and identify the oxidizing and reducing agents:
Cr3+ (aq) + IO3- (aq)
I2 (s) + OCl- (aq) b) IO3- (aq) + Cl- (aq)
As2O3 (s) + NO3- (aq) c) H3 AsO4 (aq) + N2O3 (aq)
acidic solution
acidic solution
acidic solution
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MnO4- (s) + Br- (aq) d) MnO2 (s) + BrO3- (aq)
BrO3- (s) + N2H4 (g) e) Br- (aq) + N2 (g)
NO2- (aq) + Al (s) f) NH4+ (aq) + AlO2- (g)
basic solution
acidic solution
basic solution
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1. Write the unbalanced equation in ionic form.
2. Separate the equation into two half-reactions.
3. Balance each half reaction (except for O and H).
6. Balance the charge in the half reaction by adding electrons.
4. In acid solution, balance O by adding H2O
8. Add the half reactions (canceling anything that is redundant)
9 Check to make sure atoms and charges are balanced
Half-Reaction Method in Acid
5. In acid solution, balance H by adding H+
7. multiply by half reactions by an integer to make the electrons lost equal to the electrons gained
Half-Reaction Method in base
2. Eliminate waters that appear on both sides of the equation.
1. Use the acid method, then add the number of OH- ions to both sides of the equation to turn the remaining H+ ions to H2O
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Cr2O72- (aq) + I- (aq)
a)
Cr3+ (aq) + IO3- (aq)
I- IO3-
Cr2O72- Cr3+
+ 6H+ + 6e-3H2O +
+ 7H2O 214H+ + 6 e- +
8H+ + I- + Cr2O72-
IO3- + 2Cr3+ + 4H2O
4
Complete and balance the following equations, and identify the oxidizing and reducing agents:
acidic solution
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2H+ + 2 e- + 5 551010
5 ( )
I2 IO3-
OCl- Cl-
+ 12H+ + 10e-6H2O +
+ H2O
H2O + I2 + 5OCl-
2IO3- + 5Cl- + 2H+
I2 (s) + OCl- (aq)
b)
IO3- (aq) + Cl- (aq)
2
Complete and balance the following equations, and identify the oxidizing and reducing agents:
acidic solution
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As2O3 H3 AsO4
NO3- N2O3
+ 4H+ + 4e-5H2O +
+ 3H2O 6H+ + 4 e- +
2
As2O3 (s) + NO3- (aq)
c)
H3 AsO4 (aq) + N2O3 (aq)
2
2H+ + 2H2O + 2NO3-
2H3 AsO4 + N2O3
+ As2O3
Complete and balance the following equations, and identify the oxidizing and reducing agents:
acidic solution
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+ 2OH-
2OH- +
+ 6e-
3 e- + 2 ( )
MnO4- (s) + Br- (aq)
d)
MnO2 (s) + BrO3- (aq)
MnO4- MnO2
Br- BrO3-
+ 2H2O 4H+ +
+ 6H+ 3H2O +
2H+ + Br- + 2MnO4-
BrO3- + 2 MnO2 + H2O
6 8 2 2 4
H2O + Br- + 2MnO4-
BrO3- + 2 MnO2 + 2OH-
Complete and balance the following equations, and identify the oxidizing and reducing agents:
basic solution
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BrO3- (s) + N2H4 (g)
e)
Br- (aq) + N2 (g)
Complete and balance the following equations, and identify the oxidizing and reducing agents:
acidic solution
N2H4 N2 + 4H+ + 4e-
BrO3- Br- + 3H2O 6H+ + 6 e- +
3 ( )
2 ( )
12123 3
12 12 2 2 6
3N2H4 + 2BrO3- 2Br- + 3N2 + 6H2O
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NO2- (aq) + Al (s)
f)
NH4+ (aq) + AlO2- (g)
Complete and balance the following equations, and identify the oxidizing and reducing agents:
basic solution
NO2- NH4+
Al AlO2-
+ 2H2O 8H+ + 6 e- +
2H2O + + 4H+ + 3e- 2 ( )4 2 2 8 6
2BrO3- + NH4+2H2O + + 2Al AlO2-
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2 ( )
5 ( )
+ 4H2O 8H+ + 5 e- +
+ 2e-
MnO4- (s) + Br- (aq) Mn2+(aq) + Br2 (aq)
MnO4- Mn2+
Br- Br2
16H+ + 10 Br- + 2 MnO4-
5 Br2 + 2 Mn2+ + 8 H2O
Complete and balance the following equations, and identify the oxidizing and reducing agents:
acid solution
2
10 16 2 2 8
10 5 10
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NH4NO3 (s) + Zn (s) ZnO (s) + 2H2O (g) + N2 (g)
problems 34-37 refer to the chemical reaction below
which atom is acting as the oxidizing agent?
What is the oxidation state of zinc ion at the end of the reaction?
Which element is reduced during the reaction reaction?
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Example
Balance the following equation for the reaction in acid solution. *
HNO3(aq) + H3PO3(aq) NO(g ) + H3PO4aq) + H2O(l)
![Page 39: Balancing Oxidation-Reduction Equations - Mister Chemistry](https://reader031.vdocuments.us/reader031/viewer/2022012412/616ba8edbc07744a212c07f9/html5/thumbnails/39.jpg)
1. Write the unbalanced equation in ionic form.
2. Separate the equation into two half-reactions
NO3- NO
H3PO3 H3PO4
H+ (aq) NO3- (aq) + H3PO3(aq) NO(g )
+ H3PO4aq) + H2O(l)
![Page 40: Balancing Oxidation-Reduction Equations - Mister Chemistry](https://reader031.vdocuments.us/reader031/viewer/2022012412/616ba8edbc07744a212c07f9/html5/thumbnails/40.jpg)
3. Balance each half reaction (except for O and H).
4. In acid solution, balance O by adding H2O and H by adding H+
NO3- NO
H3PO3 H3PO4
+ 2H2O4H+ +
H2O + + 2H+
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5. Balance the charges by adding electrons.
NO3- NO +
H3PO3 H3PO4
2H2O4H+ +
H2O + + 2H+
3e- +
+ 2e-
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5. Balance the charges by adding electrons.
NO3- NO +
H3PO3 H3PO4
2H2O4H+ +
H2O + + 2H+
3e- +
+ 2e-
2 x
3 x
(
( )
)
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5. Balance the charges by adding electrons.
2NO3- 2NO +
3H3PO3 3H3PO4
4H2O8H+ +
3H2O + + 6H+
6e- +
+ 6e-
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6. Add the half reactions
2NO3- 2NO +
3H3PO3 3H3PO4
4H2O8H+ +
3H2O + + 6H+
6e- +
+ 6e-
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6. Add the half reactions
2NO3- 2NO +
3H3PO3 3H3PO4
4H2O2H+ +
3H2O + + 6H+
6e- +
+ 6e-
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6. Add the half reactions
2NO3- 2NO +
3H3PO3 3H3PO4
H2O2H+ +
3H2O + + 6H+
6e- +
+ 6e-
2NO3-2H+ + 3H3PO3+
2NO + H2O + 3H3PO4
![Page 47: Balancing Oxidation-Reduction Equations - Mister Chemistry](https://reader031.vdocuments.us/reader031/viewer/2022012412/616ba8edbc07744a212c07f9/html5/thumbnails/47.jpg)
6. Add the half reactions
2NO3 +-2H+ + 3H3PO3 2NO + H2O + 3H3PO4
This is the balanced equation
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Example
Balance the following equation for the reaction in acid solution. *
Fe(s) + HCl(aq) HFeCl4(aq) + H2 (aq )
H+ H2
Fe HFeCl44Cl- +H+ +
22e- +
+ 3e-( )2
( )3
![Page 49: Balancing Oxidation-Reduction Equations - Mister Chemistry](https://reader031.vdocuments.us/reader031/viewer/2022012412/616ba8edbc07744a212c07f9/html5/thumbnails/49.jpg)
Example
Balance the following equation for the reaction in acid solution. *
Fe(s) + HCl(aq) HFeCl4(aq) + H2 (aq )
H+ 3H2
2Fe 2HFeCl48Cl- +2H+ +
66e- +
+ 6e-
![Page 50: Balancing Oxidation-Reduction Equations - Mister Chemistry](https://reader031.vdocuments.us/reader031/viewer/2022012412/616ba8edbc07744a212c07f9/html5/thumbnails/50.jpg)
Example
H+ 3H2
2Fe 2HFeCl48Cl- +2H+ +
66e- +
+ 6e-
+ 3H22Fe 2HFeCl48Cl- +8H+ +
+ 3H22Fe 2HFeCl48HCl +or
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