Presentation is loading. Please wait.

Presentation is loading. Please wait.

HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI

Published byЭлла Алеева Modified over 5 years ago

Similar presentations

Presentation on theme: "HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI"— Presentation transcript:

1 HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI3 +7 +3 +2
+4 MnO4- + C2O42-  Mn2+ + CO2 MnO C2O42-  Mn CO2 2 2 O2 4 H2O HELP 4 OH-

2 MnO4- + C2O42-  Mn2+ + CO2 1. Break it into two half-reactions MnO4-  Mn2+ C2O42-  CO2 2. Balance redox active species MnO4-  Mn2+ 3. Balance oxygen using H2O MnO4-  Mn2+ + H2O 4

3 +7 +2 MnO4-  Mn2+ 4. Balance hydrogen using H+ 8 H+ + MnO4-  Mn2+ + H2O 4 5. Balance charge using e- 5 e- + MnO4-  Mn2+ + H2O 4 H+ + 8 This is a balanced half-reaction electrons are a ________ reactant MnO4- is _______ electrons gaining MnO4- is being _______ reduced Where do the e- come from?

4 C2O42-  CO2 2. Balance redox active species C2O42-  CO2 2 3. Balance oxygen using H2O C2O42-  CO2 2 4. Balance hydrogen using H+ C2O42-  CO2 2 5. Balance charge using e- C2O42-  CO2 2 + e- 2

5 +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

6 2 ( ) 5 e- + MnO4-  Mn2+ + H2O 4 H+ + 8 5 ( ) 2 + e- C2O42-  CO2 16H+ + 2MnO4- + 5C2O42- 2Mn2+ + 8H2O + 10CO2 stoichiometry additional product, H2O additional reactant, acid

7 Ag+ (aq) + C6H12O6 (aq) Ag (s) + C6H12O7 (aq) Ag+ Ag (s) C6H12O6 C6H12O7

8 Ag+ + C6H12O6  Ag (s) + C6H12O7 Ag+ + e- Ag (s) balance mass balance oxygen H2O balance hydrogen H+ balance charge e-

9 H2O + C6H12O6 C6H12O7 + H+ 2 + e- 2 balance mass balance oxygen H2O balance hydrogen H+ balance charge e-

10 H2O + C6H12O6 C6H12O7 + H+ 2 + e- 2 ( ) 2 Ag+ + e- Ag (s) H2O + C6H12O6 + 2Ag+ C6H12O7 + H+ 2 + 2Ag (s) Ag+ reduced Ag+ oxidizing agent C6H12O6 oxidized C6H12O6 reducing agent C C + 3+

11 H2O + C6H12O6 C6H12O7 + H+ 2 + e- 2 2 ( ) Ag+ + e- Ag (s) H2O + C6H12O6 + 2Ag+ C6H12O7 + H+ 2 + 2Ag (s) 2 OH- 2 OH- H2O 2 This reaction takes place in a basic solution OH- 1 OH- 2 +H2O+ C6H12O6 +2Ag+ C6H12O7 +2Ag (s) H2O +2 OH- 2 + C6H12O6 +2Ag+ C6H12O7 +2Ag (s) H2O +

12 CN-(aq) + MnO4- (aq) CNO- (aq) + MnO2 (s) separate half-reactions CN- CNO- MnO4- MnO2 balance mass CN- CNO- MnO4- MnO2 balance oxygen H2O+ CN- CNO- MnO4- MnO2 + H2O 2

13 H2O+ CN- CNO- MnO4- MnO2 + H2O 2 balance hydrogen CN- CNO- H2O+ + H+ 2 MnO4- MnO2 + H2O 2 + H+ 4 balance charge 3 ( ) CN- CNO- H2O+ + H+ 2 + e- 2 ( ) 2 3 e-+ MnO4- MnO2 + H2O 2 + H+ 4 3 CN- +2 MnO4- + 2 H+ 3 CNO- + 2 MnO2 + H2O

14 3 CN- +2 MnO4- + 2 H+ 3 CNO- + 2 MnO2 + H2O OH- 2 OH- 2 make the solutions basic add OH- 3 CN- + 2 MnO4- + H2O 3 CNO- + 2 MnO2 + 2 OH-

Download ppt "HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI"

Similar presentations

Balancing Redox rx Steps to balancing in an acidic solution. 1.Write half-reactions without including electrons. 2.Balance the number of all atoms except.

Balancing Redox rx Steps to balancing in an acidic solution. 1.Write half-reactions without including electrons. 2.Balance the number of all atoms except.
Chapter 4B: Balancing Redox Reactions

Chapter 4B: Balancing Redox Reactions
Redox Reactions Atom 1 Atom 2 Gives electrons This atom Oxidizes itself (loses electrons) It’s the reducing agent This atom Reduces itself (gains electrons)

Redox Reactions Atom 1 Atom 2 Gives electrons This atom Oxidizes itself (loses electrons) It’s the reducing agent This atom Reduces itself (gains electrons)
Copyright Sautter 2003. REVIEW OF ELECTROCHEMISTRY All electrochemical reactions involve oxidation and reduction. Oxidation means the loss of electrons.

Copyright Sautter REVIEW OF ELECTROCHEMISTRY All electrochemical reactions involve oxidation and reduction. Oxidation means the loss of electrons.
Electrochemical Reactions Redox reaction: electrons transferred from one species to another Oxidation ≡ loss of electrons Reduction ≡ gain of electrons.

Electrochemical Reactions Redox reaction: electrons transferred from one species to another Oxidation ≡ loss of electrons Reduction ≡ gain of electrons.
1/2 reactions AP style. What are 1/2 reactions Reactions in aqueous solutions can be complicated and hard to balance. Our solution… break the one reaction.

1/2 reactions AP style. What are 1/2 reactions Reactions in aqueous solutions can be complicated and hard to balance. Our solution… break the one reaction.
Balance Redox Equations: Half Reaction concentrate on electrons, balance each ½ rx. separately Ex: Cr 2 O 7 2- (aq) + Cl - (aq)  Cr 3+ (aq) + Cl 2 (g)

Balance Redox Equations: Half Reaction concentrate on electrons, balance each ½ rx. separately Ex: Cr 2 O 7 2- (aq) + Cl - (aq)  Cr 3+ (aq) + Cl 2 (g)
Pg 646 - 651. Balancing Redox Reaction  Can use “old” way: Ag (s) + Fe(NO3)3 (aq)  Fe (s) + AgNO3 (aq)  But what if we have a reaction that looks like.

Pg Balancing Redox Reaction  Can use “old” way: Ag (s) + Fe(NO3)3 (aq)  Fe (s) + AgNO3 (aq)  But what if we have a reaction that looks like.
Chapter 20 Redox Reactions. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species to another. Many real life.

Chapter 20 Redox Reactions. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species to another. Many real life.
Half-reactions show the oxidation or reduction reaction separated. Cu (s) + 2 AgNO 3(aq) → Cu(NO 3 ) 2(aq) + 2 Ag (s) Oxidation:Cu → Cu 2+ + 2e – Reduction:Ag.

Half-reactions show the oxidation or reduction reaction separated. Cu (s) + 2 AgNO 3(aq) → Cu(NO 3 ) 2(aq) + 2 Ag (s) Oxidation:Cu → Cu e – Reduction:Ag.
OXIDATION REDUCTION REACTIONS. Rules for Assigning Oxidation States The oxidation number corresponds to the number of electrons, e -, that an atom loses,

OXIDATION REDUCTION REACTIONS. Rules for Assigning Oxidation States The oxidation number corresponds to the number of electrons, e -, that an atom loses,
Reduction-Oxidation Reactions Redox Reactions

Reduction-Oxidation Reactions Redox Reactions
Half Reactions. Balancing Oxidation-Reduction Equations Perhaps the easiest way to balance the equation of an oxidation-reduction reaction is via the.

Half Reactions. Balancing Oxidation-Reduction Equations Perhaps the easiest way to balance the equation of an oxidation-reduction reaction is via the.
10.3 The Half-Reaction Method for Balancing Equations SCH4U1 Dec 8 th, 2009.

10.3 The Half-Reaction Method for Balancing Equations SCH4U1 Dec 8 th, 2009.
half reaction method for balancing in an acid or base

half reaction method for balancing in an acid or base
Electrochemistry AP Chemistry. During oxidation-reduction (redox) reactions, the oxidation states of two substances change. oxidation = reduction = loss.

Electrochemistry AP Chemistry. During oxidation-reduction (redox) reactions, the oxidation states of two substances change. oxidation = reduction = loss.
Balancing Redox Reactions Chem 12. Application of oxidation numbers: Oxidation = an increase in oxidation number Reduction = a decrease in oxidation number.

Balancing Redox Reactions Chem 12. Application of oxidation numbers: Oxidation = an increase in oxidation number Reduction = a decrease in oxidation number.
Balancing Redox Reactions. Half Reaction Method 1.Write the formula equation if it is not given. Then write the ionic equation. Formula eq: H 2 S + HNO.

Balancing Redox Reactions. Half Reaction Method 1.Write the formula equation if it is not given. Then write the ionic equation. Formula eq: H 2 S + HNO.
Oxidation-Reduction Reactions Chapter 4 Section 9 & 10 e-

Oxidation-Reduction Reactions Chapter 4 Section 9 & 10 e-
Electrochemistry © 2009, Prentice-Hall, Inc. Balancing Oxidation-Reduction Equations Perhaps the easiest way to balance the equation of an oxidation-reduction.

Electrochemistry © 2009, Prentice-Hall, Inc. Balancing Oxidation-Reduction Equations Perhaps the easiest way to balance the equation of an oxidation-reduction.

Similar presentations

Ads by Google