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Consider the following half-reactions: Half-reaction E° (M) Ag*(aq) + e Ni2*(aq) + 2e Zn2*(aq) + 2e Ag(s) 0.799V Ni(s) -0.250V Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is:

Consider the following half-reactions: Half-reaction E° (M) Ag*(aq) + e Ni2*(aq) + 2e Zn2*(aq) + 2e Ag(s) 0.799V Ni(s) -0.250V Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is:

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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b)

Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e Ni2+(aq) + 2e Zn2*(aq) + 2e → Ag(s) 0.799V → Ni(s) -0.250V → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Ag*(aq) oxidize Zn(s) to Zn2+(aq)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.
Transcribed Image Text:Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e Ni2+(aq) + 2e Zn2*(aq) + 2e → Ag(s) 0.799V → Ni(s) -0.250V → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Ag*(aq) oxidize Zn(s) to Zn2+(aq)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 5.47x10-4 M and the Mn²+ concentration is 1.18 M ? Hg2+(aq) + Mn(s)→ Hg(1) + Mn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Transcribed Image Text:What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 5.47x10-4 M and the Mn²+ concentration is 1.18 M ? Hg2+(aq) + Mn(s)→ Hg(1) + Mn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
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