Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is oxidized to Cr³+ (aq) at a platinum electrode and a cathode where Ag* (aq) is reduced to Ag (s). Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is oxidized to Cr³+ (aq) at a platinum electrode and a cathode where Ag* (aq) is reduced to Ag (s). Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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
Section19.5: Electrochemical Cells Under Nonstandard Conditions
Problem 19.7CYU: The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to...
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Transcribed Image Text:Write the cell notation for an electrochemical cell consisting of an anode where Cr²+ (aq) is oxidized to Cr³+ (aq) at a platinum electrode and a cathode where Ag* (aq) is
reduced to Ag (s). Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Transcribed Image Text:Write the cell notation for an electrochemical cell consisting of an anode where Cr²+ (aq) is oxidized to Cr³+ (aq) at a platinum electrode and a cathode where Ag* (aq) is
reduced to Ag (s). Assume all aqueous solutions have a concentration of 1 mol/L.
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