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7/27/2019 Galvanic and Electrolytic Cells
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Galvanic and Electrolytic Cells
lectrochemistry and electrochemical cells were introduced in our unit on diabetes monitoring. You can review that
ere. Electrochemical cells are in a circuit that allows the transfer of electrons through it. The cell includes:
an anode, the electrode where oxidation takes place a cathode, the electrode where reduction takes place an electrolyte, to allow conduction of ions within the solution in each half cell a salt bridge orsemipermeable membrane, to allow conduction of ions between half cells the external circuit that connects the two electrodes includes wires, a load, and meters
Galvanic Cells
n electrochemical cell that releases energy is called a galvanic cell. The electrochemical reaction has a negative vaf the Gibbs free energy and a positive cell potential difference.
elow is a galvanic cell in which the reaction between A+
and B is exothermic, with a G of -10 kJ/mol under
andard conditions and a value ofE0
of 0.10 V.
Hydrogen Electrode and Half Reactions
We havetablesthat show reduction half reactions. How are these obtained?
n electrochemical reaction in an electrochemical cell requires both a reduction half reaction and an oxidation half
http://butane.chem.uiuc.edu/pshapley/genchem2/B9/1.htmlhttp://butane.chem.uiuc.edu/pshapley/genchem2/B9/1.htmlhttp://butane.chem.uiuc.edu/pshapley/genchem2/Tables.html#nhttp://butane.chem.uiuc.edu/pshapley/genchem2/Tables.html#nhttp://butane.chem.uiuc.edu/pshapley/genchem2/Tables.html#nhttp://butane.chem.uiuc.edu/pshapley/genchem2/Tables.html#nhttp://butane.chem.uiuc.edu/pshapley/genchem2/B9/1.html7/27/2019 Galvanic and Electrolytic Cells
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eaction. A voltmeter in the circuit shows the total cell voltage (Etot = Ered + Eox). We can determine a half cell potenty measuring the voltage of a cell that includes that half cell along with a standard half cell of known potential.
he accepted standard electrode is the hydrogen electrode. This consists of a half cell with an unreactive metal electr
2(g) at 1 atmosphere pressure, and a 1 M aqueous solution of acid.
n the reduction mode:
2H+
+ 2e-
H2
Ered = 0.00 V
n the oxidation mode:
H2 2H+
+ 2e-
Ered = 0.00 V
ou can see here that the potential of a half cell in which Cu+2
is reduced to Cu is 0.34 V.
reductionCu
+2+ 2e
-Cu
Ered = x
oxidationH2 2H
++ 2e
-
Eox = 0.00 V
netCu
+2
+ H2 Cu + 2H+
Etot = 0.34 V
lectrolytic Cells
n electrolytic cell has an endothermic chemical reaction. The reaction is not spontaneous so a power source is requi
nergy is stored in an electrochemical cell. That energy can be released when the cell is allowed to run in a galvanic
mode.
7/27/2019 Galvanic and Electrolytic Cells
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bove right is the galvanic cell that we saw previously. The molecules A and B+
are produced and energy is released
he electrode on the left side of the cell is the cathode because A+
is reduced to A at that electrode.
bove left is the same cell in an electrolytic mode. An energy source causes the reaction to go in the direction oppos
the spontaneous direction. Now, A+
and B are produced. The electrode on the right is the cathode because B+
is
educed to B there.
Professor Patricia Shapley, University of Illinois, 2012