A chemist designs a galvanic cell that uses these two half-reactions:

half-reaction standard reduction potential

MnO4⁻ (aq) + 8H⁺ (aq) + 5e⁻ → Mn (aq) ²⁺ + 4H2O (l) E⁰red = + 1.51V

Fe³⁺ (aq) + e⁻ → Fe²⁺ (aq) E⁰red = + 0.771V

Answer the following questions about this cell.

(a) Write a balanced equation for the half-reaction that happens at the cathode.

(b) Write a balanced equation for the half-reaction that that happens at the anode.

(c) Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Question

Chemistry

Yasmin Graham

30 November, 01:09

A chemist designs a galvanic cell that uses these two half-reactions:

half-reaction standard reduction potential

MnO4⁻ (aq) + 8H⁺ (aq) + 5e⁻ → Mn (aq) ²⁺ + 4H2O (l) E⁰red = + 1.51V

Fe³⁺ (aq) + e⁻ → Fe²⁺ (aq) E⁰red = + 0.771V

Answer the following questions about this cell.

(a) Write a balanced equation for the half-reaction that happens at the cathode.

(b) Write a balanced equation for the half-reaction that that happens at the anode.

(c) Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

+1

Answers (1)

Know the Answer?

Harold Lozano · Answer 1

MnO4⁻ (aq) + 8H⁺ (aq) + 5Fe³⁺ (aq) →Mn (aq) ²⁺ + 4H2O (l) + 5Fe²⁺ (aq)

Explanation:

a)

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

b)

5Fe³⁺ (aq) + 5e⁻ → 5Fe²⁺ (aq)

c)

MnO4⁻ (aq) + 8H⁺ (aq) + 5Fe³⁺ (aq) →Mn (aq) ²⁺ + 4H2O (l) + 5Fe²⁺ (aq)