zuai-logo

What are the general steps to solve electrolysis problems using Faraday's Law?

  1. 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.

All Flashcards

What are the general steps to solve electrolysis problems using Faraday's Law?
1. 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.
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 is the effect of applying an external voltage greater than the absolute value of the negative E<sub>cell</sub> in an electrolytic cell?
The non-spontaneous reaction is forced to occur.
What is the effect of passing a current through a solution of metal ions during electrolysis?
The metal ions are reduced at the cathode, depositing the metal.