Electrode Electrolyte Determination Given A Redox Reaction

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Electrode Electrolyte Determination Given A Redox Reaction

Figure 15.7 is a conceptual sketch of the construction of a galvanic cell based on the following spontaneous reaction:

3Fe(s) + 2Au^{3+} --------> 3Fe^{2+} + 2Au(s)

(a) Determine electrodes A and B, and electrolytes A and B in figure 15.7.

(b) What is the sign of the change in enthalpy for this reaction?

**The strings**:

S_{7}P_{5}A_{52} (Change - Chemical Change)
**The math**:

Pj Problem of Interest is of type *change* (chemical change). This problem is also an *identity* problem because we are determining the identities of the electrodes and electrolytes from the given redox reaction. However, the Pj Problem of Interest is cast as of type *change* because of the underlying chemical reaction in which the electrodes and electrolytes are participants.

The half-reactions of the cell are as follows:

Half-reaction at the anode:

Fe(s) -------> Fe^{2+} + 2e^{-} oxidation reaction.

Half-reaction at the cathode:

Au^{3+} + 3e^{-} -------> Au(s) reduction reaction

So, Electrode A (the anode) is an iron electrode and electrolyte A is a solution containing Fe^{2+} ions (e.g FeSO_{4})

So, Electrode B (the cathode) is a gold electrode and electrolyte B is a solution containing A^{3+} ions (e.g. AuCl_{3})

The reaction is spontaneous, the enthalpy change ΔH is negative.

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