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Summary Electrochemistry
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12 chemistry Electrochemistry
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Introduction to ElectrochemistryIn this session, we will be discussing electrochemistry and coordination chemistry.
Electrochemistry deals with the conversion of chemical energy into electrical energy and vice
versa. There are two types of electrochemical cells, galvanic and electrolytic cells. Galvanic cells
involve spontaneous reactions, while electrolytic cells require an external power source to drive
the reaction. We will be discussing the working of galvanic cells and the importance of salt
bridges in maintaining electrical neutrality.
Galvanic Cells
Galvanic cells involve redox reactions that produce electrical energy. The anode undergoes
oxidation, while the cathode undergoes reduction. The direction of electron flow is from the
anode to the cathode. The overall reaction in a galvanic cell is spontaneous, and the cell
potential can be calculated using the reduction potentials of each half-cell.
Electrolytic Cells
Electrolytic cells require an external power source to drive the reaction. The cathode undergoes
reduction, while the anode undergoes oxidation. The direction of electron flow is from the
cathode to the anode. The overall reaction in an electrolytic cell is non-spontaneous, and the cell
potential must be greater than zero for the reaction to occur.
Salt Bridges
Salt bridges are used in electrochemical cells to maintain electrical neutrality. The salt bridge
contains an inert electrolyte that allows ions to flow between the two half-cells, preventing a
buildup of charge. Common inert electrolytes used in salt bridges include ammonium nitrate,
potassium nitrate, ammonium chloride, and potassium chloride.
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