Based on the reduction potentials you measured, answer the following 1. Calculat

Question

Based on the reduction potentials you measured, answer the following 1. Calculate the potential for the electrochemical cell shown below? Pt|Fe^3+ (aq)|Fe^2+ (aq)||Ag^+(aq)|Ag(s) 2. Will metallic zinc precipitate out of a Zn(NO_3)_2 solution if metallic copper is added? Explain. 3. Which of the following would be the strongest reducing agents under standard conditions: Zn(s), Cu(s), Br^- (aq), Fe^2+ (aq), Cl^- (aq) 4. Why could the cell potential for the Cl_2(g) | 2Cl^- (aq) || Ag^+ (aq) | Ag(s) cell not be determined?

Explanation / Answer

1. Potential for the given cell,

Eo = Ecathode - Eanode

     = 0.80 - 0.77

     = 0.03 V

2. No metallic Zn would not precipitate out of solution when metallic Cu is added as the reduction potential of Cu is lower than the Zn and hence Cu will have greater tendency to get reduced than Zn in solution.

3. Among all Zn has the most negative standard reduction potential, hence this would be the strongest reducing agent.

4. In the given cell, Ag+ would react with the formed Cl- in solution and precipitate out. Thus making the system not homogeneous and hence the cell potential is not measurable.

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