Question

Balance the following overall reactions showing the half reactions as well as the balanced overall reactions:...

Balance the following overall reactions showing the half reactions as well as the balanced overall reactions:

a. CH3OH + O2 ----> CO2 + H2O (@ high pH)

b. HS- + MnO4- -----> S(s) + MnO2 (s) (@ high pH)

c. IO3- (iodate) + I- (iodade) ----> I2 (iodine) (@ low pH)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Balance the reactions in acid using the half-reactions method. (could you also explain this process in...
Balance the reactions in acid using the half-reactions method. (could you also explain this process in words please. Thank you) a. MnO2 + BiO3– → MnO4– + Bi3+ b. CH3CH2OH + Cr2O72– → CH3COOH + Cr3+ c. NO3– + I2 → IO3– + NO2–
Balance each of the following redox reactions using the half-reaction method. a. ClO2–(aq) --> ClO2(g) +...
Balance each of the following redox reactions using the half-reaction method. a. ClO2–(aq) --> ClO2(g) + Cl–(aq) b. O2(g) + Sb(s) --> H2O2(aq) + SbO2–(aq) c. MnO4–(aq) + SO2(g) -->Mn2+(aq) + HSO4–(aq) d. CO(g) + I2O5(s) --> CO2(g) + I2(aq)
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) U4+ (aq) →...
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) U4+ (aq) → UO22+ (aq) (ii) (acid solution) Rh2+ (aq) → Rh2O3 (s) (iii) (base solution) MnO2 (s) → MnO4– (aq) (iv) (base solution) PuO3 (s) → Pu(OH)4 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Use half-reactions to balance the following equation in acidic solution: Fe2+ + IO3- = Fe3+ +...
Use half-reactions to balance the following equation in acidic solution: Fe2+ + IO3- = Fe3+ + I2
Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the...
Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the proper coefficient for each of the species involved in the overall reaction. Water molecules and protons are not shown in the half-reactions, but may be needed in the overall reaction. I2 (s) → I- (aq) ξo = 0.54 V VO2+ (aq) → VO2+ (aq) ξo = 1.00 V VO2+ (aq) I2 (s) VO2+ (aq) I- (aq) H+ (aq) H2O (l)
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) O2(g) + Pb(s) → H2O(l) + Pb2+(aq) (b) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq) (c) Cl2(g) + Cr3+(aq) → Cl −(aq) + Cr2O72−(aq) (d) F2(g) + Mn2+(aq) → F −(aq) + MnO4−(aq)
1 a. The reaction between aluminum and iodine has this overall electrochemical cell: Al(s)| Al3+(aq)|| I2(aq),I-1(aq)|...
1 a. The reaction between aluminum and iodine has this overall electrochemical cell: Al(s)| Al3+(aq)|| I2(aq),I-1(aq)| Pt(s) Balance each of the two half-cell reactions and put them together to obtain the balanced overall reaction. Identify the oxidation and reduction half-cells, as well as the cathode and anode. b. Refer to the attached table of standard reduction potentials. Determine the standard potential (EO) for the overall reaction. Show all units. Is the reaction spontaneous? How can you tell? c. Write the...
Hi, the following problem I'm working on is: The hydroperoxide ion HO2- (aq) reacts with permanganate...
Hi, the following problem I'm working on is: The hydroperoxide ion HO2- (aq) reacts with permanganate ion MnO4- (aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution. I know the beginning equation is: HO2^-(aq) + MNO4^-(aq) ---> MnO2(s) +O2(g) and that I have to write half rxns for each one. I also know the answer ends up being: H2O(l) + 2MnO4- (aq) +3HO2-(aq) --->...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo =...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo = 0.34 V MnO4 - (aq) + 4 H+ (aq) + 3 e- -----> MnO2 (s) + 2 H2O (l) Eo = 1.68 V A. What is the standard cell potential for a voltaic cell comprised of these two half reactions? B. What is the equilibrium constant for this reaction at 25 oC? C. How is the magnitude of the equilibrium constant consistent with a...
Balance each of the following by the ion-electron method. All are in acidic solution. Do not...
Balance each of the following by the ion-electron method. All are in acidic solution. Do not include states.             Mn2+ + BiO3¯ + H+   ____    MnO4¯ + Bi3+ + H2O             IO3¯ + SO2 + H2O _____ I2 + SO42¯ + H+             Se + BrO3¯ + H2O ________ H2SeO3 + Br¯             P4+ HClO + H2O ________ H3PO4 + Cl¯ + H+             Al + Cr2O72¯ + H+ ______ Al3+ + Cr3+ + H2O             ClO3¯ + I¯ +...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT