5 Questions
Explain the difference between galvanic and electrolytic cells and provide an example of each type of cell in action.
Galvanic cells convert chemical energy into electrical energy through spontaneous redox reactions, such as a battery powering a device. Electrolytic cells, on the other hand, use electrical energy to drive non-spontaneous reactions, such as electroplating.
Define resistivity, conductivity, and molar conductivity of ionic solutions and explain their significance in electrochemistry.
Resistivity (ρ) is a measure of a material's ability to resist the flow of electric current, while conductivity (κ) measures its ability to conduct electric current. Molar conductivity (Λm) quantifies the ability of a given volume of a solution to carry a charge, and these properties are critical in understanding the behavior of ionic solutions in electrochemical processes.
What is the Nernst equation used for, and how does it relate to the emf of a galvanic cell?
The Nernst equation is used to calculate the emf (electromotive force) of a galvanic cell under non-standard conditions. It relates the cell potential to the activities of the chemical species involved in the redox reaction.
Discuss the construction and functioning of primary and secondary batteries, as well as fuel cells.
Primary batteries are non-rechargeable and convert chemical energy into electrical energy, while secondary batteries are rechargeable and can convert electrical energy back into chemical energy. Fuel cells utilize chemical energy from a fuel and an oxidant to produce electrical energy.
Explain the process of corrosion and its relation to electrochemistry.
Corrosion is an electrochemical process where a metal deteriorates due to chemical reactions with its environment. It involves the transfer of electrons between the metal and its surroundings, making it a key aspect of electrochemistry.
Test your knowledge about electrochemical cells, Nernst equation, standard potential, Gibbs energy of cell reaction, resistivity, conductivity, and molar conductivity of ionic solutions.
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