oxidation half reaction --------------------------------- reduction half reaction
Mn^2+(aq) ------>MnO2(s) --------------------- H2O2(aq) --------> H2O(l)
Mn^2+(aq) +2H2O(l)------>MnO2(s) -------------- H2O2(aq) --------> H2O(l) + H2O(l)
Mn^2+(aq) +2H2O(l)+4OH^-(aq)------>MnO2(s) +4H2O(l) --- H2O2(aq) +2H2O(l)--------> 2H2O(l) + 2OH^- (aq)
Mn^2+(aq) +2H2O(l)+4OH^- (aq) ------>MnO2(s) +4H2O(l) +2e^- -------- H2O2(aq) +2H2O(l) +2e^---> 2H2O(l) + 2OH^- (aq)
Mn^2+(aq) +2H2O(l)+4OH^- (aq) ------>MnO2(s) +4H2O(l) +2e^-
H2O2(aq) +2H2O(l) +2e^---> 2H2O(l) + 2OH^- (aq)
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Mn^2+ (aq) + H2O2(aq) + 2OH^- (aq) ------> MnO2(s) + 2H2O(l)
oxidation half reaction --------------------------------- reduction half reaction
Cl2(g)-----> 2ClO3^- (aq) --------------------- Cl2(g) ---------> 2Cl^- (aq)
Cl2(g)+ 6H2O(l) -----> 2ClO3^- (aq) --------------------- Cl2(g) ---------> 2Cl^- (aq)
Cl2(g)+ 6H2O(l) + 12OH^- (aq) -----> 2ClO3^- (aq) + 12H2O(l)------- Cl2(g) ---------> 2Cl^- (aq)
Cl2(g)+ 6H2O(l) + 12OH^- (aq) -----> 2ClO3^- (aq) + 12H2O(l)+10e^- ------- Cl2(g) +2e^- ---------> 2Cl^- (aq)
Cl2(g)+ 6H2O(l) + 12OH^- (aq) -----> 2ClO3^- (aq) + 12H2O(l)+10e^-
5Cl2(g) +10e^- ---------> 10Cl^- (aq)
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6Cl2(g) + 12OH^- (aq) -----------> 2ClO3^- (aq) + 10Cl^- (aq) + 6H2O(l)
19.37 Balance the following oxidation-reduction equations The reactions occur in basic solution a. Mn + H2O...
Balance the following oxidation-reduction equations. The reactions occur in acidic solution. (Use the lowest possible coefficients. Omit states of matter. Add H20 or H to any side of the reaction if it is needed.) a. Pb + Bi0,- + PbO2+ BiS+ Pb + BiO3 + PbO2 + Bi9+ + b. Cr,0,? + Fe2+ + Cr+ + Fe3+ | Cr₂O₂ ² + | Fe²+ + + Fel- c. MnO, +1“ + Mn2+ + Cl2 MnO2 + Cl + Mn + Cl2...
Homework -Chapter 19-Electrochemistry 19.as Balance the folowing odation-reduction equations The reactions occur in acidic solution CrO C,o Cr CO a Mn + NO, MnO, + HNO, c.
2. Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method a. Cu(s) + NO, (aa)Cu2 (aa) NOGg) h. Cr,0, (aa) C (a) Cr (a)C2(g) c. Pb(s) + PbO2(s) + H2S04(aq) PbSO,(s) d. Mn(a) NaBio,()Bi (aa) + Mn04 (aq)
balance the following oxidation reduction reaction in basic solution NO3- + Pb —-> NO + Pb 2+ Balance basic oxidation-reduction reactions Question Balance the following oxidation-reduction reaction in basic solution. NO; + Pb → NO + Pb2+ Provide your answer below: No; + Pb+ 4,0-Ono + Pb2+ + oH-
118 HNO: Mn + H2O + NO MnO2 + H + Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 4. PbO2 + Mn?' + SO42- + H P bSO4 + MnO4 + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 5._HNO: + Cr2O72- + H → Cr + NO + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 6. Mn?+ CIO, MnO2 + CIO Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent:...
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
Chemical equations of reduction–oxidation (redox) reactions can be quite nontrivial to balance. To do so, you begin with balancing the number of electrons some particles lose in oxidation and other particles gain in reduction. Consider a reaction between potassium permanganateKMnO4 andhydrochloricacidHCl(aq), which can be used in a lab to produce chlorine gas Cl2. In this reaction, a MnO− 4 ion is reduced to a Mn2+ ion by getting electrons from Cl− and losing its oxygen atoms to bind with H+...
Balance the following oxidation-reduction equation. The reactions occur in acidic or basic aqueous solution, as indicated. a. Co2+ + H2S +Co+Ss (acidic) O Co2+ +8H2S + 2Co + S8 + 16H+ O8Co2+ + 8H,8 + 8Co+Sg + 16+ Co2+ + 8H2S + 2Co + S8 b. S + Bry + SO 2 + Br” (basic) OS? + 4Br2 + 80H 8Br + SO4 + 4H2O O $2 + 4Br2 + 4H20 +8Br” + SO4 + 8H+ Os + 4Br2 +...
Balance each of the following half-reactions, assuming that they occur in basic solution. H2O(l)→H2(g)
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...