Research

Below are the chemical equations that were used in the energy production proof here. It proves how much Voltage, or activation energy, to allow the reaction to go.

2 H₂O(l) --> 2 H₂(g) + O₂(g)

2 H2O + 2 e- --> H2 + 2 OH-			Eored = -0.83 V
2 H2O --> O2 + 4 H+ + 4 e-			Eoox = -1.23 V

http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch20/faraday.php

"Electrochemistry." Electrolytic Cells. Bodner Research Web, n.d. Web. 28 Apr. 2014.

Electrolysis cells

Below is a brief description of how the electrodes should work. One end will be hooked up to the positive end of the battery while the other to the negative end of the battery.

The electrolytic cell has two (usually inert) electrodes to pass the electric current into the electrolyte. The negative electrode is called the cathode and the positive electrode is called the anode. The inert electrodes are usually made of graphite or platinum wire. The reactions occur at the surface of the electrodes. The power supply is usually symbolized by a short fat line (negative) and a long thin line (positive)

http://ibchem.com/IB/ibnotes/full/red_htm/9.5.htm

"Electrolytic Cells." Oxidation and Reduction. IsisSoft Interactive, n.d. Web. 28 Apr. 2014.

Electrolysis Reaction Again

This is an important video to watch if one is not sure what electrolysis is about. In this particular experiment, graphite electrodes were used. We are undecided on the material of electrodes for our model.

The Splitting of Water

The link below describes and the picture to the right depicts English physicist William Nicholson and English surgeon Sir Anthony Carlisle completing and experiment wherein water is split into hydrogen and oxygen via platinum wires connected to one battery terminal each.  This was the first time electrolysis was used to produce gaseous hydrogen and oxygen.

http://www.sciencephoto.com/media/107877/view

Experiments on Electrolysis of Water

This website linked below is an overview of an experiment looking to improve the electrolysis processes of water. The errors that occur within there experimentation were related to corroding copper electrodes, slow process time for the reaction and discoloration in the water. With in their experiment they changed their copper electrodes to graphite rod electrodes to avoid the corrosion and discoloration of the water. For our project this got me thinking about the most efficient metal to use for the electrodes and what would be most environmentally friendly for open water in the ocean. Possible electrodes to be tested may contain copper, aluminum, steal, platinum, and graphite.  Also in their experiment they added 10% of sulfuric acid to increase the reaction time. This would not be most efficient for a submarine model because we would not want to put in foreign substances in the water. The question that arises is that will salt content in the water produce a similar effect to increase reaction time. This will be investigated further with chemical reactions and testings.

http://www.miniscience.com/projects/WaterElectrolise.htm

INC., MiniScience,. "Electrolysis of Water." Electrolysis of Water. N.p., n.d. Web. 11 Apr. 2014. <http://www.miniscience.com/projects/WaterElectrolise.htm

Electrolysis Reaction

This is an example of the electrolysis reaction. It states that the two test tubes contain hydrogen gas and oxygen gas separately. This is a great visual for the physical basic reaction.

Five Neat Things About Submarines 

This was the article that got myself (Jon) interested in hydrolysis in submarines. It also helped me understand what hydrolysis was and how I could explain it to my group members. This blog is an important resource for the design project.


http://markanthonygreen.blogspot.com/2010/03/five-neat-things-about-submarine-by.html

Green, Tony. "5 Neat Things about a Submarine." : Five Neat Things about a Submarine by. Blogspot, 20 Mar. 2010. Web. 07 Apr. 2014.