Open Question
Calculate ΔG°_rxn and E°_cell for a redox reaction with n = 2 that has an equilibrium constant of K = 25 (at 25 °C).
Ch.19 - Electrochemistry
Chapter 19, Problem 74
A voltaic cell employs the redox reaction: 2 Fe3+(aq) + 3 Mg(s) → 2 Fe(s) + 3 Mg2+(aq). Calculate the cell potential at 25 °C under each set of conditions. a. standard conditions. b. [Fe3+] = 1.0 × 10^-3 M; [Mg2+] = 2.50 M. c. [Fe3+] = 2.00 M; [Mg2+] = 1.5 × 10^-3 M.
Verified step by step guidance1
<insert step 1: Identify the half-reactions and their standard reduction potentials.>
<insert step 2: Calculate the standard cell potential (E°cell) using the standard reduction potentials.>
<insert step 3: Use the Nernst equation to calculate the cell potential under non-standard conditions.>
<insert step 4: For part b, substitute the given concentrations into the Nernst equation and solve for the cell potential.>
<insert step 5: For part c, substitute the given concentrations into the Nernst equation and solve for the cell potential.>
Related Practice
Open Question
Calculate ΔG°rxn and E°cell for a redox reaction with n = 3 that has an equilibrium constant of K = 0.050 (at 25 °C).
Textbook Question
A voltaic cell employs the following redox reaction: Sn2+(aq) + Mn(s) → Sn(s) + Mn2+(aq) Calculate the cell potential at 25 °C under each set of conditions. c. [Sn2+] = 2.00 M; [Mn2+] = 0.0100 M
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Textbook Question
An electrochemical cell is based on these two half-reactions:
Ox: Pb(s) → Pb2+(aq, 0.10 M) + 2 e–
Red: MnO4–(aq, 1.50 M) + 4 H+(aq, 2.0 M) + 3 e– → MnO2(s) + 2 H2O(l)
Calculate the cell potential at 25 °C.
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Textbook Question
An electrochemical cell is based on these two half-reactions:
Ox: Sn(s) → Sn2+(aq, 2.00 M) + 2 e–
Red: ClO2(g, 0.100 atm) + e– → ClO2–(aq, 2.00 M)
Calculate the cell potential at 25 °C.
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Textbook Question
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. a. What is the initial cell potential?
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