Balancing Redox Reactions
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Balancing Redox Reactions. AlI 3. I 2 (s) + Al (s) . 3. 2. 2. +7. +3. +2. +4. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2. 2. 2 O 2. 4 H 2 O. HELP. 4 OH -. MnO 4 -.  Mn 2+. MnO 4 -.  Mn 2+. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2.

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Balancing Redox Reactions

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Balancing redox reactions

Balancing Redox Reactions

AlI3

I2 (s) + Al (s) 

3

2

2

+7

+3

+2

+4

MnO4- + C2O42- Mn2+ + CO2

MnO4- + C2O42- Mn2+ + CO2

2

2 O2

4 H2O

HELP

4 OH-


Balancing redox reactions

MnO4-

 Mn2+

MnO4-

 Mn2+

MnO4- + C2O42- Mn2+ + CO2

1. Break it into two half-reactions

MnO4-

 Mn2+

 CO2

C2O42-

2. Balance redox active species

3. Balance oxygen

using H2O

+ H2O

4


Balancing redox reactions

MnO4-

 Mn2+

MnO4-

MnO4-

 Mn2+

 Mn2+

+ H2O

+ H2O

4

4

8

H+ +

+7

+2

4. Balance hydrogen

using H+

8

H+ +

5. Balance charge

using e-

5

e- +

This is a balanced half-reaction

electrons are a ________

reactant

MnO4- is _______ electrons

gaining

MnO4- is being _______

reduced

Where do the e- come from?


Balancing redox reactions

C2O42-

 CO2

C2O42-

C2O42-

C2O42-

C2O42-

 CO2

 CO2

 CO2

 CO2

2

2

2

2. Balance redox active species

2

3. Balance oxygen

using H2O

4. Balance hydrogen

using H+

5. Balance charge

using e-

+ e-

2


Balancing redox reactions

+3

+4

C2O42-

 CO2

2

+ e-

2

This is a balanced half-reaction

electrons are a ________

product

C2O42- is _______ electrons

losing

C2O42- is being _______

oxidized

Now combine the two half-reactions


Balancing redox reactions

(

)

(

)

+ e-

2

C2O42-

 CO2

2

MnO4-

 Mn2+

+ H2O

4

8

H+ +

2

5

e- +

5

16H+

+ 8H2O

+ 10CO2

+ 2MnO4-

+ 5C2O42-

2Mn2+

stoichiometry

additional product, H2O

additional reactant, acid


Balancing redox reactions

Ag+ (aq)

Ag (s)

+ C6H12O7 (aq)

+ C6H12O6 (aq)

Ag+

Ag (s)

C6H12O6

C6H12O7


Balancing redox reactions

Ag+ + C6H12O6 Ag (s) + C6H12O7

Ag+

+ e-

Ag (s)

balance mass

balance oxygen

H2O

balance hydrogen

H+

balance charge

e-


Balancing redox reactions

H2O +

C6H12O6

C6H12O7

+ H+

2

+ e-

2

balance mass

balance oxygen

H2O

balance hydrogen

H+

balance charge

e-


Balancing redox reactions

(

)

+ H+

2

H2O +

C6H12O6

C6H12O7

+ H+

2

+ e-

2

2

Ag+

+ e-

Ag (s)

H2O +

C6H12O6

+ 2Ag+

C6H12O7

+ 2Ag (s)

Ag+

reduced

Ag+

oxidizing agent

C6H12O6

oxidized

C6H12O6

reducing agent

C

C

+

3+


Balancing redox reactions

(

)

2

H2O

2

2

OH-

OH-

+2

+

H2O

H2O

H2O +

C6H12O6

C6H12O7

+ H+

2

+ e-

2

2

Ag+

+ e-

Ag (s)

H2O +

C6H12O6

+ 2Ag+

C6H12O7

+ H+

2

+ 2Ag (s)

2

OH-

2

OH-

This reaction takes place in a basic solution

OH-

1

+H2O+

C6H12O6

+2Ag+

C6H12O7

+2Ag (s)

+ C6H12O6

+2Ag+

C6H12O7

+2Ag (s)


Balancing redox reactions

CNO-

MnO2

CN-

MnO4-

CNO-

MnO2

CN-

MnO4-

CNO- (aq)

+ MnO2 (s)

CN-(aq)

+ MnO4- (aq)

separate half-reactions

CNO-

MnO2

CN-

MnO4-

balance mass

balance oxygen

H2O+

+ H2O

2


Balancing redox reactions

CNO-

MnO2

H2O+

CN-

MnO4-

+ H2O

2

(

)

CNO-

H2O+

CN-

+ H+

2

(

)

4

MnO2

MnO4-

+ H+

+ H2O

2

CNO-

MnO2

H2O+

CN-

MnO4-

+ H2O

2

balance hydrogen

+ H+

2

+ H+

4

balance charge

3

+ e-

2

2

3

e-+

3 CN-

+2 MnO4-

+ 2 H+

3 CNO-

+ 2 MnO2

+ H2O


Balancing redox reactions

3 CN-

+2 MnO4-

+ 2 H+

3 CNO-

+ 2 MnO2

+ H2O

OH-

2

OH-

2

add OH-

make the solutions basic

3 CN-

+ 2 MnO4-

+H2O

3 CNO-

+ 2 MnO2

+ 2 OH-


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