This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — here are the answers for question 51: Step 1: Understand the concept of a reference electrode. When a new reference electrode is used, its standard potential is set to 0.00 V. The potentials of all other half-cells are then adjusted relative to this new reference. The formula for the new potential (E'_new) is: E'_new = E^_original - E^_reference In this case, iron (Fe(s) / Fe^2+(aq)) is the reference electrode, and its original standard potential is E^_reference = +0.44 V (from the given table). Step 2: Calculate the new potential for each half-cell. For Al(s) / Al^3+(aq): E'_Al = (-1.66 V) - (+0.44 V) = -2.10 V For Zn(s) / Zn^2+(aq): E'_Zn = (-0.76 V) - (+0.44 V) = -1.20 V For Fe(s) / Fe^2+(aq): E'_Fe = (+0.44 V) - (+0.44 V) = 0.00 V For Ni(s) / Ni^2+(aq): E'_Ni = (+0.25 V) - (+0.44 V) = -0.19 V Step 3: Present the rewritten E^ values in a table. The rewritten E^ values using iron as a reference electrode are: |l|c|c| Half-cell & E^ / Volts & Using iron \\ Al(s) / Al^3+(aq) & -1.66 & -2.10 \\ Zn(s) / Zn^2+(aq) & -0.76 & -1.20 \\ Fe(s) / Fe^2+(aq) & 0.44 & 0.00 \\ Ni(s) / Ni^2+(aq) & 0.25 & -0.19 \\ Got more? Send 'em!