Electrochemistry Quiz

Study Notes

In an electrochemical cell, a salt bridge is used to connect the two half-cells, allowing the transfer of ions and maintaining electrical neutrality.
The electrolyte used in the salt bridge is typically KCl.

The Nernst equation relates the reduction potential of an electrochemical reaction to the standard electrode potential, temperature, and activities (or concentrations) of the chemical species involved.
The equation is 𝐸 = 𝐸∘ - 𝑅𝑇𝑛𝐹 ln⁡𝑄, where 𝐸 is the electrode potential, 𝐸∘ is the standard electrode potential, 𝑅 is the gas constant, 𝑇 is the temperature, 𝑛 is the number of moles of electrons, 𝐹 is the Faraday constant, and 𝑄 is the reaction quotient.

The amount of substance deposited at the electrode is proportional to the charge passed through the electrolyte.
Faraday's first law of electrolysis states that the amount of chemical change or substance deposited at an electrode during electrolysis is directly proportional to the quantity of electricity (charge) passed through the electrolyte.

A galvanic cell, also known as a voltaic cell, is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell.
A Daniel cell consists of a zinc electrode in zinc sulfate solution and a copper electrode in copper sulfate solution, connected by a salt bridge.

Electrode potential is not a colligative property.
Colligative properties include vapor pressure lowering, boiling point elevation, and osmotic pressure.