Phineas was running a voltaic cell constructed with a Ni(s)|Ni2*(aq) half-cell and a K(s)|K*(aq) cell. The observed potential of Ecell is 2.71 V. Using the Nernst equation calculate the concentration of Ni2+ if 0.559M of K* is present. K+(aq) + e¯ → K(s) E°= -2.93 Ni²++2e- → Ni E° = -0.23 O 1.01 O 0.563 O 0.681 O 0.715
Phineas was running a voltaic cell constructed with a Ni(s)|Ni2*(aq) half-cell and a K(s)|K*(aq) cell. The observed potential of Ecell is 2.71 V. Using the Nernst equation calculate the concentration of Ni2+ if 0.559M of K* is present. K+(aq) + e¯ → K(s) E°= -2.93 Ni²++2e- → Ni E° = -0.23 O 1.01 O 0.563 O 0.681 O 0.715
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.4: Standard Electrochemical Potentials
Problem 1RC
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![Phineas was running a voltaic cell constructed with a Ni(s)|Ni²*(aq) half-cell and a K(s)|K*(aq) cell.
The observed potential of Ecell is 2.71 V. Using the Nernst equation calculate the concentration of
Ni2+ if 0.559M of K* is present.
K+(aq) + e¯ → K(s) E°= -2.93
Ni2++2e- → Ni E° = -0.23
O 1.01
O 0.563
O 0.681
O 0.715](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61f2bd8c-527a-479e-9deb-09c663979694%2F2e4b8656-1517-4910-99f7-9889930ff645%2Fpz8sv6wh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Phineas was running a voltaic cell constructed with a Ni(s)|Ni²*(aq) half-cell and a K(s)|K*(aq) cell.
The observed potential of Ecell is 2.71 V. Using the Nernst equation calculate the concentration of
Ni2+ if 0.559M of K* is present.
K+(aq) + e¯ → K(s) E°= -2.93
Ni2++2e- → Ni E° = -0.23
O 1.01
O 0.563
O 0.681
O 0.715
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