Electrolysis
Electrolysis is a process in which electricity is used to split water into hydrogen and oxygen gases. When a direct current flows through water, oxygen appears at the positive electrode (anode), and hydrogen is released at the negative electrode (cathode). Typically, twice as much hydrogen is produced as oxygen by volume. Because pure water does not conduct electricity well, substances like salt are often added, though this is less environmentally friendly. Using a proton exchange membrane (PEM), hydrogen can be extracted from pure water, because the membrane allows necessary particle movement between anodes and cathodes.
Related
Summarize the key steps shown in the video for water electrolysis
Explain the roles of anode and cathode in the video demonstration
List the materials and setup used in the video for the electrolysis cell
Compare PEM electrolysis vs simple saltwater electrolysis shown
Describe safety concerns and byproducts mentioned in the video.
Electrolysis needs a conducting liquid with free-moving ions (electrolyte).
Positive ions (cations) are attracted to the cathode, while negative ions (anions) are attracted to the anode.
The process causes chemical changes due to the movement and reactions of ions at the electrodes.
Increasing the concentration of the electrolyte or the voltage increases the rate of ion flow and, therefore, the rate of electrolysis.