For a Cobalt-Silver cell with the given diagram, we’re asked to write the net cell equation and to calculate E°cell and ΔG°rxn at 25 °C.
The cell diagram of the process is:
Co(s) | Co2+ (aq, 0.0155 M) || Ag+ (aq, 1.50 M) | Ag(s)
Where
Co(s) is the left-hand electrode
Co2+ is the left-hand cation in the aqueous electrolyte
Ag+ is the right-hand cation in the aqueous electrolyte
Ag is the right-hand electrode
There are two ways to identify the Cathode and Anode:
A B C
Co(s) | Co2+ (aq, 0.0155 M) || Ag+ (aq, 1.50 M) | Ag(s)
We answer the problem in 5 steps:
Step 1: Balance the charges: add electrons to the more positive side (or less negative side)
Step 2: Balance electrons on the two half-reactions.
For the following electrochemical cell
Co(s) | Co2+ (aq, 0.0155 M) || Ag+ (aq, 1.50 M) | Ag(s)
Write the net cell equation. Phases are optional. Do not include the concentrations.
Calculate the following values at 25.0°C using standard potentials as needed.
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