All Flashcards
Compare and contrast Galvanic and Electrolytic Cells.
Galvanic: Spontaneous, produces electricity, positive E° | Electrolytic: Non-spontaneous, requires external power, negative E°
Compare the electron flow in galvanic vs. electrolytic cells.
Galvanic: Electrons flow spontaneously from anode to cathode. | Electrolytic: Electrons are forced to flow from anode to cathode by an external power source.
Compare the spontaneity of Galvanic and Electrolytic cells.
Galvanic: Spontaneous redox reactions occur. | Electrolytic: Non-spontaneous redox reactions are forced to occur.
What are the general steps to solve electrolysis problems using Faraday's Law?
- Convert time to seconds and calculate total charge (Coulombs). 2. Convert Coulombs to moles of electrons using Faraday's constant. 3. Use stoichiometry to convert from moles of electrons to moles of substance. 4. Convert moles of substance to grams using molar mass.
Define electrolytic cell.
A cell that uses an external power source to drive a non-spontaneous redox reaction.
Define anode.
The electrode where oxidation occurs.
Define cathode.
The electrode where reduction occurs.
Define Faraday's constant.
The charge of one mole of electrons, approximately 96485 Coulombs.
Define Faraday's Law.
The law stating that the amount of substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the cell.
Define galvanic cell.
An electrochemical cell that generates electricity through spontaneous redox reactions.