Question

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–

Homework Answers

Answer #1

a)

Mn in MnO2 has oxidation state of +4

Mn in MnO4- has oxidation state of +7

So, Mn in MnO2 is oxidised to MnO4-

Bi in BiO3 has oxidation state of +6

Bi in Bi+3 has oxidation state of +3

So, Bi in BiO3 is reduced to Bi+3

Reduction half cell:

1 BiO3 + 3e- --> 1 Bi+3

Oxidation half cell:

1 MnO2 --> 1 MnO4- + 3e-

Number of electrons is same in both half reactions.

So, balancing of electrons is not required. It's already balanced

Lets combine both the reactions.

1 BiO3 + 1 MnO2 --> 1 Bi+3 + 1 MnO4-

Balance Oxygen by adding water

1 BiO3 + 1 MnO2 --> 1 Bi+3 + 1 MnO4- + 1 H2O

Balance Hydrogen by adding H+

1 BiO3 + 1 MnO2 + 2 H+ --> 1 Bi+3 + 1 MnO4- + 1 H2O

This is balanced chemical equation in acidic medium

BiO3 + MnO2 + 2 H+ --> Bi+3 + MnO4- + H2O

I am allowed to answer only 1 question at a time

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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¯ +...
Balance each redox reaction in basic solution using the half reaction method. (Please provide step by...
Balance each redox reaction in basic solution using the half reaction method. (Please provide step by step solution because I'm lost in this area) O2 + Cr3+ → H2O2 + Cr2O72- Te + NO3- → TeO32- + N2O4 IO3-+Re→ReO4- +IO- Pb2++IO3-→ PbO2 +I2 Cr2O72- + Hg → Hg2+ + Cr3+
Balance the following half-reactions (Express your answer as a balanced half-reaction. Identify all of the phases...
Balance the following half-reactions (Express your answer as a balanced half-reaction. Identify all of the phases in your answer.): (basic) Cr2O72−(aq)⟶Cr3+(aq) (acidic) CrO42−(aq)⟶Cr(OH)4−(aq) (basic) Bi3+(aq)⟶BiO3−(aq) (acidic) ClO−(aq)⟶Cl−(aq)
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)
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): NO3– + I–...
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): NO3– + I– → NO + I2 (b) (acid solution): Cr2O72– + Fe2+ → Cr3+ + Fe3+ (c) (basic solution): Au(s) + CN– + O2 (g) → Au(CN)2–
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)
(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.
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)
Balance the following redox equation in basic solution using the half-reactions method. H2O2 + Cr3+ =...
Balance the following redox equation in basic solution using the half-reactions method. H2O2 + Cr3+ = CrO42- + H2O
In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing...
In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing agent and the reducing agent in each reaction. a. ??(?) + ??3 −(??) → ?? 2+(??) + ??(?) b. ??2?7 2−(??) + ?? −(??) → ?? 3+(??) + ??2 (?) c. ??2 2+(??) + ??(?) → ? 4+(??) + ???4 2− d. ??2 (??) → ???3 −(??) + ?? −(??) This was how the question was given.