Multiple Choice
Which equation is used to calculate the theoretical cell potential (E^ext{cell}) under standard conditions for a galvanic cell?
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20. Electrochemistry
Cell Potential: Standard
Multiple Choice
Predict whether the following reaction will occur as written based on the calculated Eºcell.
Ag+ (aq) + Au (s) → Ag (s) + Au3+ (aq)
Standard Reduction Potentials
Ag+(aq) + e– → Ag (s) E°red = + 0.80 V
Au3+ (aq) + 3 e– → Au (s) E°red = + 1.50 V
A
+0.70 V
B
+2.30 V
C
-0.70 V
D
-2.30 V
Verified step by step guidance1
Identify the half-reactions involved in the given redox reaction. The oxidation half-reaction is Au (s) → Au3+ (aq) + 3 e–, and the reduction half-reaction is Ag+ (aq) + e– → Ag (s).
Determine the standard reduction potentials for each half-reaction from the provided data: E°red for Ag+ (aq) + e– → Ag (s) is +0.80 V, and E°red for Au3+ (aq) + 3 e– → Au (s) is +1.50 V.
Reverse the oxidation half-reaction to find its oxidation potential: Au (s) → Au3+ (aq) + 3 e–. The oxidation potential is the negative of the reduction potential, so E°ox = -1.50 V.
Calculate the standard cell potential (E°cell) using the formula: E°cell = E°red (reduction) + E°ox (oxidation). Substitute the values: E°cell = +0.80 V + (-1.50 V).
Evaluate the sign of E°cell. If E°cell is positive, the reaction is spontaneous as written. If E°cell is negative, the reaction is non-spontaneous as written.
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