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3. You decide to assemble an electrochemical cell based on the half reactions Mg2+ / Mg(s) and Ni²+ / Ni(s). a. Write the equation for the product favored reaction that occurs in the cell. b. Calculate E for this product-favored reaction at 25 °C. C. What is the better reducing agent, Mg or Ni?

3. You decide to assemble an electrochemical cell based on the half reactions Mg2+ / Mg(s) and Ni²+ / Ni(s). a. Write the equation for the product favored reaction that occurs in the cell. b. Calculate E for this product-favored reaction at 25 °C. C. What is the better reducing agent, Mg or Ni?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 36E: Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution...
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Question: Please help guide me through this! Also, E° (Volts) for Mg²+ (aq) + 2 e -> Mg (s) is -2.37 V. Ni²+ (aq) + 2 e -> Ni (s) is -0.25 V.
3. You decide to assemble an electrochemical cell based on the half reactions Mg2+ / Mg(s) and Ni²+ / Ni(s). a. Write the equation for the product favored reaction that occurs in the cell. b. Calculate E for this product-favored reaction at 25 °C. What is the better reducing agent, Mg or Ni? d. Calculate Ecell for this reaction at 25 °C, [Ni²+] = 0.10 M and [Mg2+] = 0.90 M. (the Nernst equation, E=E - (RT/nF) In Q C. e. Do electrons flow from the Mg electrode to the Ni electrode or vice-versa? f. If a salt bridge containing NaNO3 connects the two half cells, in which direction do the nitrate ions move? g. Calculate AG for this cell at 25 °C when [Ni²+] = 0.10 M and [Mg2+] = 0.90 M. h. Calculate AG for this cell at 25 °C when [Ni2+] = 1.0 M and [Mg2+] = 1.0 M. i. Compare the magnitude of your AG answers in parts g and h, above. Is this reaction becoming more spontaneous or less spontaneous? Explain this observation using Le Chatelier's Principle.
Transcribed Image Text:3. You decide to assemble an electrochemical cell based on the half reactions Mg2+ / Mg(s) and Ni²+ / Ni(s). a. Write the equation for the product favored reaction that occurs in the cell. b. Calculate E for this product-favored reaction at 25 °C. What is the better reducing agent, Mg or Ni? d. Calculate Ecell for this reaction at 25 °C, [Ni²+] = 0.10 M and [Mg2+] = 0.90 M. (the Nernst equation, E=E - (RT/nF) In Q C. e. Do electrons flow from the Mg electrode to the Ni electrode or vice-versa? f. If a salt bridge containing NaNO3 connects the two half cells, in which direction do the nitrate ions move? g. Calculate AG for this cell at 25 °C when [Ni²+] = 0.10 M and [Mg2+] = 0.90 M. h. Calculate AG for this cell at 25 °C when [Ni2+] = 1.0 M and [Mg2+] = 1.0 M. i. Compare the magnitude of your AG answers in parts g and h, above. Is this reaction becoming more spontaneous or less spontaneous? Explain this observation using Le Chatelier's Principle.
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