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Lena [83]
3 years ago
8

When the following oxidation–reduction reaction in acidic solution is balanced, what is the lowest whole-number coefficient for

  H2O, and on which side of the balanced equation should it appear?
MnO4–(aq)+Br–(aq)→Mn2+(aq)+Br2(l)

Select one:

a. 1, reactant side

b. 2, product side

c. 8, product side

d. 16, reactant side

e. 4, product side
Chemistry
1 answer:
Svet_ta [14]3 years ago
3 0

Answer:

c. 8, product side

Explanation:

In order to balance a redox reaction we use the ion-electron method, which has the following steps:

Step 1: identify oxidation and reduction half-reaction.

Oxidation: MnO₄⁻(aq) → Mn²⁺(aq)

Reduction: Br⁻(aq) → Br₂(l)

Step 2: perform the mass balance adding H⁺ and H₂O where necessary

8 H⁺(aq) + MnO₄⁻(aq) → Mn²⁺(aq) + 4 H₂O(l)

2 Br⁻(aq) → Br₂(l)

Step 3: perform the electrical balance adding electrons where necessary.

8 H⁺(aq) + MnO₄⁻(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l)

2 Br⁻(aq) → Br₂(l) + 2 e⁻

Step 4: multiply both half-reactions by numbers that secure that the number of electrons gained and lost are the same.

2 × (8 H⁺(aq) + MnO₄⁻(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l))

5 × (2 Br⁻(aq) → Br₂(l) + 2 e⁻)

Step 5: add both half-reactions side to side.

16 H⁺(aq) + 2 MnO₄⁻(aq) + 10 e⁻ + 10 Br⁻(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 Br₂(l) + 10 e⁻

16 H⁺(aq) + 2 MnO₄⁻(aq) + 10 Br⁻(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 Br₂(l)

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c.  It's an electrolytic cell, because it's a nonspontaneous reaction.

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a. By the notation given, first is represented the oxidation reaction and then the reduction reaction, so they are:

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Mg²⁺(aq) + 2e⁻ ⇄ Mg(s) (reduction)

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The number of electrons must be the same, so the oxidation reaction is multiplied by 2, and the reduction reaction by 3.

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