Consider the following cell:Pt (s) | H₂ (8,1 atm)| H* (aq, a = 1)| Fe³ (aq), Fe²+ (aq) | Pt(s)(i)Write the overall cell reaction.(ii)If the cell potential is 0.712 V, and given that Fe3+ (aq) + e→ Fe2+ (aq)E° = 0.771 V, what is the ratio of Fe2+ (aq) to Fe3+ (aq) at 298.15 K?(iii) Calculate the fraction of the total iron present as Fe3+ (aq) at cellpotentials of 0.650, 0.700, 0.750, 0.771, 0.800 and 0.900 V.

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Answered: Consider the following cell: Pt (s) |…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 105QRT

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Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
Consider the following galvanic cell reaction at 25 oC, 4 Cr2+(aq) + O2(g) + 4 H3O+(aq) → 4 Cr3+(aq) + 6 H2O(l). Which of thefollowing statements best describes what would happen to the cell potential if the concentration of Cr2+ is increased?(a) The cell potential would become less positive.(b) The cell potential would become more positive.(c) The cell potential would remain the same.(d) It is impossible to tell.

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