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Design an electrochemical cell that produces an optimal energy output. -…
Design an electrochemical cell that produces an optimal energy output.
An electrochemical cell is a device that generates electricity from the chemical reactions that occur within it, or consume electrical energy in order to enable chemical reactions. These devices are capable of converting chemical energy into electrical energy.
Generally consist of a cathode and an anode.
Made up of two "half cells" that are connected by a salt bridge.
There are two types of salt bridge - a glass tube filled with an electrolyte, or a porous filter paper soaked in an electrolyte
Types of electrolytes:
Sodium Chloride
Potassium Chloride
Potassium Nitrate
What determines how effective an electrolyte is?
Ion mobility - both the cation and the anions require similar electrical mobility to maintain electrical neutrality of the two half cells.
Availability - the electrolyte cannot be difficult to procure or highly expensive.
Types of electrochemical cells:
Galvanic (Voltaic) Cells
Changes chemical energy into electrical energy.
Cathode has a positive charge and anode has a negative charge.
Within the context of the deconstruction practical, the electrochemical cell requires an electrical energy output, thus a galvanic cell will be constructed.
Facilitates a spontaneous redox reaction
Electrolytic Cells
Changes electrical energy into chemical energy.
Cathode has a negative charge and anode has a positive charge.
Requires external voltage.
Facilitates a non-spontaneous redox reaction