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QUESTION 11 The following 5 questions refer to the redox reaction shown below at 298K : Sn (s) + CuSO4 (s) → SnSO4 (aq) + Cu (s) write the electrode half reactions. Anode: Sn (s) +2e Sn2+ (aq); cathode: Cu (s) +2e Anode: Cu (s) +2e → Cu2+ (aq); cathode: Sn (s) +2e Anode: Sn (s) - 2e Sn2+( QUESTION 12 - Anode: Cu²+ (aq) +2e → Cu (s); cathode: Sn²+ (aq) +2e O Pt | Sn(s), Sn²+ (aq) || Cu2+ (aq), Cu(s) | Pt O Sn²+ (aq) | Sn(s) ||Cu(s) | Cu²+ (aq) QUESTION 13 → Sn(s) | Sn2+ (aq) || Cu²+ (aq) | Cu(s) Cu²+ (aq) › Sn²+ (aq) +(aq); cathode: Cu2+ (aq) +2e O 0.197 -0.197 Continue with the last question, the corresponding cell notation is O Sn(s) | Cu2+ (aq) || Sn²+ (aq) | Cu(s) → Sn (s) - Cu (s) Continue with the last two questions, calculate stand cell potential Eºcell. 0.477 -0.477

QUESTION 11 The following 5 questions refer to the redox reaction shown below at 298K : Sn (s) + CuSO4 (s) → SnSO4 (aq) + Cu (s) write the electrode half reactions. Anode: Sn (s) +2e Sn2+ (aq); cathode: Cu (s) +2e Anode: Cu (s) +2e → Cu2+ (aq); cathode: Sn (s) +2e Anode: Sn (s) - 2e Sn2+( QUESTION 12 - Anode: Cu²+ (aq) +2e → Cu (s); cathode: Sn²+ (aq) +2e O Pt | Sn(s), Sn²+ (aq) || Cu2+ (aq), Cu(s) | Pt O Sn²+ (aq) | Sn(s) ||Cu(s) | Cu²+ (aq) QUESTION 13 → Sn(s) | Sn2+ (aq) || Cu²+ (aq) | Cu(s) Cu²+ (aq) › Sn²+ (aq) +(aq); cathode: Cu2+ (aq) +2e O 0.197 -0.197 Continue with the last question, the corresponding cell notation is O Sn(s) | Cu2+ (aq) || Sn²+ (aq) | Cu(s) → Sn (s) - Cu (s) Continue with the last two questions, calculate stand cell potential Eºcell. 0.477 -0.477

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...
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QUESTION 14 Continue with the last three questions, calculate the equilibrium constants K of the redox reactions at 25°C. 4.6 x 1016 1.04 0.04 1.4 x 1016 QUESTION 15 Continue with the last question, based on your calculation, which direction does the reaction proceed spontaneously under the reaction condition? O Toward product cannot be determined. O The reaction is in equlibrium O Toward reactant
Transcribed Image Text:QUESTION 14 Continue with the last three questions, calculate the equilibrium constants K of the redox reactions at 25°C. 4.6 x 1016 1.04 0.04 1.4 x 1016 QUESTION 15 Continue with the last question, based on your calculation, which direction does the reaction proceed spontaneously under the reaction condition? O Toward product cannot be determined. O The reaction is in equlibrium O Toward reactant
QUESTION 11 The following 5 questions refer to the redox reaction shown below at 298K : Sn (s) + CuSO4 (s) → SnSO4 (aq) + Cu (s) write the electrode half reactions. Anode: Sn (s) +2e Sn2+ (aq); cathode: Cu (s) +2e Anode: Cu (s) +2e → Cu2+ (aq); cathode: Sn (s) +2e QUESTION 12 - Anode: Cu²+ (aq) +2e → Cu (s); cathode: Sn²+ (aq) +2e Anode: Sn (s) - 2e Sn2+ (aq); cathode: Cu²+ (aq) +2e O Pt | Sn(s), Sn²+ (aq) || Cu2+ (aq), Cu(s) | Pt O Sn²+ (aq) | Sn(s) ||Cu(s) | Cu²+ (aq) Sn(s) | Sn2+ (aq) || Cu²+ (aq) | Cu(s) QUESTION 13 → Continue with the last question, the corresponding cell notation is O Sn(s) | Cu2+ (aq) || Sn²+ (aq) | Cu(s) Cu2+ (aq) Sn²+ (aq) O 0.197 -0.197 → Sn (s) Cu (s) Continue with the last two questions, calculate stand cell potential Eºcell. 0.477 -0.477
Transcribed Image Text:QUESTION 11 The following 5 questions refer to the redox reaction shown below at 298K : Sn (s) + CuSO4 (s) → SnSO4 (aq) + Cu (s) write the electrode half reactions. Anode: Sn (s) +2e Sn2+ (aq); cathode: Cu (s) +2e Anode: Cu (s) +2e → Cu2+ (aq); cathode: Sn (s) +2e QUESTION 12 - Anode: Cu²+ (aq) +2e → Cu (s); cathode: Sn²+ (aq) +2e Anode: Sn (s) - 2e Sn2+ (aq); cathode: Cu²+ (aq) +2e O Pt | Sn(s), Sn²+ (aq) || Cu2+ (aq), Cu(s) | Pt O Sn²+ (aq) | Sn(s) ||Cu(s) | Cu²+ (aq) Sn(s) | Sn2+ (aq) || Cu²+ (aq) | Cu(s) QUESTION 13 → Continue with the last question, the corresponding cell notation is O Sn(s) | Cu2+ (aq) || Sn²+ (aq) | Cu(s) Cu2+ (aq) Sn²+ (aq) O 0.197 -0.197 → Sn (s) Cu (s) Continue with the last two questions, calculate stand cell potential Eºcell. 0.477 -0.477
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