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What voltage would have been observed if you had switched the position of the electrodes but not the solutions for any of the electrochemical cells? Clearly explain your answer, include what would happen in each cell.

What voltage would have been observed if you had switched the position of the electrodes but not the solutions for any of the electrochemical cells? Clearly explain your answer, include what would happen in each cell.

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 26E: Determine the overall reaction and its standard cell potential at 25 C for the reaction involving...
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What voltage would have been observed if you had switched the position of the electrodes but not the solutions for any of the electrochemical cells? Clearly explain your answer, include what would happen in each cell.

Cell 3 List the combination of half-cells used (electrode and solution used in each half cell). 2+ Fe²+ + 2e > Fe Pb→ Pb²+ + 2e E = -0.44V E = -0.13v Write the balanced net ionic equation for the spontaneous reaction. 2+ 2+ Pb + Fe²² → Pb²+ + Fe Observed Voltage 6.031v Calculated Eº for cell 0.3lv (spontaneous cell) Cell 4 List the combination of half-cells used (electrode and solution used in each half cell). Fe Fe²+ 2e €²=-0.44 v 2+ Ni²+ + 2e → Ni € = -0.25v E° = -0.44 ve(-0.13v) E = -0.31v Write the balanced net ionic equation for the spontaneous reaction. Fe+Ni2+ →Fe + Ni Observed Voltage +.200 v (spontaneous cell) Calculated Eº for cell (). 19 v Eº = -0.25v - (-0.44×) € -0.19 Cell 5 List the combination of half-cells used (electrode and solution used in each half cell). Write the balanced net ionic equation for the spontaneous reaction.
Transcribed Image Text:Cell 3 List the combination of half-cells used (electrode and solution used in each half cell). 2+ Fe²+ + 2e > Fe Pb→ Pb²+ + 2e E = -0.44V E = -0.13v Write the balanced net ionic equation for the spontaneous reaction. 2+ 2+ Pb + Fe²² → Pb²+ + Fe Observed Voltage 6.031v Calculated Eº for cell 0.3lv (spontaneous cell) Cell 4 List the combination of half-cells used (electrode and solution used in each half cell). Fe Fe²+ 2e €²=-0.44 v 2+ Ni²+ + 2e → Ni € = -0.25v E° = -0.44 ve(-0.13v) E = -0.31v Write the balanced net ionic equation for the spontaneous reaction. Fe+Ni2+ →Fe + Ni Observed Voltage +.200 v (spontaneous cell) Calculated Eº for cell (). 19 v Eº = -0.25v - (-0.44×) € -0.19 Cell 5 List the combination of half-cells used (electrode and solution used in each half cell). Write the balanced net ionic equation for the spontaneous reaction.
9 8 10 6 7 In-Lab Guidelines (This is a guide to the information that you should be observing while in the laboratory. Record this information in the Laboratory Notebook. Turn in the duplicate pages of your observations to your Instructor before you leave the laboratory period.) Electrochemical Cells NAME: INSTRUCTOR: 5 Cell # Laboratory 12 Electrochemistry Determination of Avogadro's Number and Faraday's Constant 4 3 1 2 Cathode Red Probe Electrode Си Pb Fe Anode Black Probe Solution Electrode Solution Ni DATE: Cu(NO3)2) Zn Pb(NO3) Cu Fe(NO₂)₂ Pb Ni(NO₂) Fe SECTION: Voltage Zn(N03)₂ +.859 Cathode Cu Cu(NO₂.379 Cu Fe Pb(NO3)₂ +.031 Fe(NO3)2 +.200 bservations: (any observations made during the experiment, spills, disconnects, wrong utions, wrong electrodes, etc.)
Transcribed Image Text:9 8 10 6 7 In-Lab Guidelines (This is a guide to the information that you should be observing while in the laboratory. Record this information in the Laboratory Notebook. Turn in the duplicate pages of your observations to your Instructor before you leave the laboratory period.) Electrochemical Cells NAME: INSTRUCTOR: 5 Cell # Laboratory 12 Electrochemistry Determination of Avogadro's Number and Faraday's Constant 4 3 1 2 Cathode Red Probe Electrode Си Pb Fe Anode Black Probe Solution Electrode Solution Ni DATE: Cu(NO3)2) Zn Pb(NO3) Cu Fe(NO₂)₂ Pb Ni(NO₂) Fe SECTION: Voltage Zn(N03)₂ +.859 Cathode Cu Cu(NO₂.379 Cu Fe Pb(NO3)₂ +.031 Fe(NO3)2 +.200 bservations: (any observations made during the experiment, spills, disconnects, wrong utions, wrong electrodes, etc.)
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