Respuesta :
Start by writing a simplified reaction sequence between the two elements. For this, we need some electric potential values, which you can find in a table. Adjust based on the source that you are given, because they will differ just a little.
For the reactions, using a reductions table:
Cr3+ + 3e- —> Cd0 E=-0.74
Ag+ + e- —> Ag0. E=0.8
Because Ag+ has a larger E value, the Ag+ will oxidize Cd0 in the following reaction:
3Ag+ + Cr0 —> 3Ag0 + Cd3+
(Notice that three Ag’s are used to work for the transfer of three electrons.)
At the anode, the item in solution is oxidized so that electrons are left behind. This means that the reaction occurring at the anode is the Chromium reaction, and it looks like this:
Cr0(s) —> Cr3+(aq) + 3e-
For the reactions, using a reductions table:
Cr3+ + 3e- —> Cd0 E=-0.74
Ag+ + e- —> Ag0. E=0.8
Because Ag+ has a larger E value, the Ag+ will oxidize Cd0 in the following reaction:
3Ag+ + Cr0 —> 3Ag0 + Cd3+
(Notice that three Ag’s are used to work for the transfer of three electrons.)
At the anode, the item in solution is oxidized so that electrons are left behind. This means that the reaction occurring at the anode is the Chromium reaction, and it looks like this:
Cr0(s) —> Cr3+(aq) + 3e-
The half-cell reaction that takes place at the anode has been oxidation of chromium. It has been given as [tex]\rm Cr^0\;(s)\;\rightarrow\;Cr^3^+\;(aq)\;+\;3\;e^-[/tex].
A voltaic cell has been defined as the electrochemical cell that has been using the chemical energy to produce electrical energy. The chemical reaction in the cell results in the production of electrical energy.
Half-cell reaction at Anode
The anode has been the negatively charged electrode in the electrochemical cell, where the loss of electrons by the chemical takes place.
Thus, anode has been the site for oxidation in the voltaic cell.
The chromium-silver cell has, one of the element oxidized, and the other being reduced. The element with higher oxidation potential reduces.
In silver and chromium, the action potential of silver has been higher than chromium. Thus, silver has been reduced, and chromium has been oxidized. Thus, the oxidation of chromium occur at the anode in the voltaic cell.
The chemical reaction for the oxidation of chromium has been:
[tex]\rm Cr^0\;(s)\;\rightarrow\;Cr^3^+\;(aq)\;+\;3\;e^-[/tex]
Learn more about voltaic cell, here:
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