The Conclusion

The result of the electrolysis experiment was that no oxygen gas was produced, only hydrogen gas. This is because the chloride ions are oxidized in the reaction rather than the water oxidized to oxygen. Although the main goal of the project is not completed, the resulting hydrogen gas can be useful on multiple occasions. This will be discussed in the following sections. If this were to be scaled up for a full sized submarine, an extremely large amount of electric potential must be emitted to produce an adequate amount of products to be used. Also, the brine saltwater must be filtered to distilled water for oxygen gas to be produced. The amount of power that a nuclear submarine can emit makes electrolysis possible for breathable air. A nuclear submarine can produce about 150 standard cubic feet per hour of oxygen using electrolysis [7]. The tests showed that the reaction is not at all efficient and would need to be modified largely to become reasonable on large scale. 

Lab Number 9

The main issue at the moment is calculating the efficiency of the experiment. The problem is that a small amount of energy is being inputting into the system while a larger energy is being outputted. This is impossible since energy cannot be created. One solution is that the current could have been measured incorrectly. We will use another multimeter to measure the current to get an accurate reading to fix the calculations.

Lab Number 8

In today's lab, our group discussed the final report rough draft and what we can do to improve it. We broke down each section in the report and decided what information to add and remove. We also assigned roles to review and revise sections. The final construction will be completed next week as the materials will be purchased this weekend. We will run a few tests next week in larger scale with the finalized electrodes, copper. While constructing the final design, the last sections of the final project will be added. These will be equally distributed to each member of the group.

New Container

It was agreed upon in the group to shrink the system entirely. If we were to go large scale, and use the big plastic bin, an incredible amount of salt would be needed in order to have the solution to be just like saltwater. A smaller plastic bin with a lid was bought from a local hardware store. This will prove to be easier to operate with the system meaning a smaller amount of salt would be needed. The hole in the top of the lid needed to be machined in order for the alligator clamps to fit through. A 1/2 inch drill bit with the drill press was used at the machine shop to cut the lid.

The new and improved container. 

A larger hole was made for the alligator clamps to fit through.

Lab Number 7

In this lab, we were able to complete the efficiency experiment. Results and conclusions will be discussed at the end of this post.

Experiment setup:

Each reaction ran for an exact 60 seconds.

Copper

Aluminum

Oxygen gas actually visibly being produced on this electrode.

Steel

Titanium

 

Results

Conclusion

In each of the experiments, there is one common theme: there is actually no oxygen gas being created. This is the main goal of the design project and it seems that it cannot be done. In order for the reaction to go, there needs to be salt in the solution, however, this salt actually ionizes with the oxygen gas to create chlorine gas. The chlorine gas contaminates the water which is why it turns a greenish/yellow color. Overall, it was learned that the reaction cannot be done here to produce oxygen.

On the other hand, in each case a decent amount of hydrogen gas was produced. This can later be used in different reactions to not only produce oxygen, but possibly fire missiles or other possibilities. Hydrogen gas is extremely flammable and because of this trait, is useful for many reactions.

In conclusion, this was a extremely useful and important experiment. It took a while to complete, but all of the time spend was crucial for learning the experiment. We are happy that we have the knowledge that was learned from the efficiency experiment. 

Open Lab

On Wednesday, we were able to get lab time from 3pm-6pm. We set up the system using the steel electrode and a 1000 mL beaker. Sodium Chloride was added to the system as a catalyst to make the reaction go faster.

This is a picture of how the system looks. 

In this open lab period, we were able to experiment and learn about the reaction. Many small parts about the system went wrong from keeping the electrode in place, having water in the graduated cylinders, and the connections of the copper wire to the electrode. The lab time was needed to iron out these problems. Wednesday was a learning experience and allowed us to really learn about the reaction and how it works.

Sean stirring the salt in the water

A close up of the reaction.

On Thursday, Sean and Emily were able to get into the lab and continue the experiment. They learned that the connection between the copper wire and the electrode, although they were twisted on, were not solid and in result, hindered the reaction. They decided to use alligator clamps for a better connection and that improved the reaction tremendously.

Alligator clamps used

 This was a breakthrough in the experiment and allowed for the lab on Friday to go smoothly and for solid data to be recorded. In the Lab Week 7 post, the results of the experiment as well as conclusions will be discussed.

This is an example of how the experiment went. As it is seen, it is not the best setup for the reaction.

Lab Number 6

In week 6 lab, our group was able to go down into the Conservative Energy Laboratory and start with our experiment. The experiment wasn't exactly successful, but useful knowledge about the reaction and the process was gained.

We set up the experiment like this:

with one graduated cylinder on each stand and each clamps holding an electrode. It was soon found that this was an incorrect setup for the experiment but the reason why will be explained later. Copper wire was attached to the electrodes using electrical tape and was strung to each pole of the 6 volt battery. On a set time, the wires were applied to the battery and ... not much happened. After over a minute, all that was seen was minor bubbles. 

This indicated that the reaction started, but shortly afterward stopped. This was attempted multiple times but with each successive trial, there was no clear gas production volume. After help from Megan, we decided to add sodium chloride, or salt, to the solution to allow for a faster reaction. This did in fact help, as more bubbles were produced initially, but the reaction still did not continue. 

After scratching our heads and searching for possible answers, the solution struck us near the end of the lab time. We needed to complete the circuit not electrically, but chemically. This could be done in two ways. One being a salt bridge which maintains charge balance by allowing electrons to flow from anode to cathode and around the battery again. The reason why the reaction wasn't continuing was because the air was not able to transfer electrons throughout the two systems. By completing this circuit, the reaction should progress. 

An example salt bridge

The other way the reaction could continue is if we submerged the entire system in a salt-water solution. This makes the surrounding salt-water the salt bridge in which electrons could flow, therefor driving the reaction. 

Kind of like this, in a way.

The sodium chloride used would be a catalyst for the reaction, in result speeding it up. There is concern that chlorine gas would be produced, but this is a chance that we would have to take.  

With this knowledge, we will get into the lab on our own time this week to complete the experiment before lab Friday. This will be done to discover which electrode is the most efficient. 

Materials Came In

This week, a portion of our materials came in which were ordered from McMasterCarr.com. We received, all in one foot, 1/4 inch diameter dimensions, a steel rod, aluminum rod, copper rod, titanium rod and four graduated cylinders. The exact specifications are as listed:

• Low-Carbon Steel Rod
• Multipurpose 6061 Aluminum Rod
• High-Strength 182 Copper Rod
• Ultra-Corrosion-Resistant Titanium (Grade 2)
• 25 mL Plastic Graduated Cylinder, 6-5/8 inch tall (0.5 mL increments) 

Copper Rod

Titanium Rod

Graduated Cylinder

Since the rods came in each with a 12 inch length, they needed to be cut down to fit the 3 inch requirement. A metal cutting Band Saw was used at the Drexel Machine Shop.

The Band Saw in action

 Correct markings were made and the metals were carefully cut in half, then in half again. 

Examples of the measurement markings on the Titanium rods

After they were cut, a belt-fed sander was used to smooth the rough edges to prevent injury. 

Titanium Rod before

Titanium Rod after

The Band Saw cut all the metals with ease, except for the Titanium rod which took at least 10-15 minutes per cut (while other metals took 30-60 seconds). 

The Titanium rod took 15 minutes to cut per cut

Nevertheless, the rods were cut to the required length.

Finished Copper Rods

Finished Titanium Rods

Finished Steel Rods

Finished Aluminum Rod

Lab Number 5

Materials are on the way!

• Graduated cylinders are ordered
• Final electrode list has been made, needs to be finalized. 

• Type	Diameter (in)	Length (in)	Price
  Graduated Cylinder	1	7 7.0/8.0	$10.87
  Steel Unpolished	1.0/2.0	12	$3.06
  Aluminum Unpolished	1.0/2.0	12	$3.19
  Titanium	1.0/2.0	6	$20.11
  Copper Unpolished	1.0/2.0	12	$14.80

Once we get these materials in, we can proceed with our experiment (using the multimeter) and finalize which electrode will be used. Each electrode should be 1/4 inch in diameter and 3 inches long for the test and experiment. It is important that the surface area and connection to each electrode is identical throughout each pair. A challenge will be cutting each metal accurately.

The Final System

Once we physically get the materials, we will finalize on the size of the system. The material should be aluminum, but any easily malleable substance will be used. An acrylic window will be used to view the reaction. We have an idea to make this window accessible by using a latch. This will be challenging because when close, it needs to be water proof. A solution to this may be a rubber piece, but we are unsure at this point.    

Electrolysis of Water

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.

The Science behind Electrodes

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.

Better Video of Electrolysis Reaction

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.

Lab Number 4

What to do:

Once we find a cheap graduated cylinder that works for the project, we can then find the correct diameter for the electrodes. This then tells us how big the whole system would be, therefor allowing us to order the correct amount of materials and start construction. While construction is in process, an experiment for determining the most efficient voltage and electrode will be done to record data as well as concluding the selection of materials. Most of the other materials, such as copper wires, batteries, electrical tape and a fish tank are bought already. Time in a undergraduate lab with a borrowed voltmeter is needed for the experiment. The experiment should last at most 3 hours.

Electrodes:

It is concluded that these materials will be ordered when the size is known:

• stainless steel
• aluminum
• graphite
• iron
• copper

Electrolysis Reaction Proof

Creo Parametric Model

Shown below is a crude model of the final design of the system. The scaling of each part in the assembly is off but the rough basic shape is there. Also, the electrode placement is off but will be fixed in actual construction. Not shown is the outside circuitry which will switch system on and off.

Materials shown:

• Gold - 9v battery
• Green - attached to positive terminal
• Red - attached to negative terminal
• Blue Transparent - graduated cylinders
• Metallic - electrodes
• Aluminum - aluminum shell
• Glass - acrylic window

A look inside the system.

An outside look of the system.

A different angle.

Lab Number 3

Next Step:

• Creo model of system
• Electrode test
• determining what material the electrode should be made out of (steel, aluminum, copper, graphite)
• determining if an electrode will be used for better conduction
• determining an efficient, cost effective, and easily obtainable wire material
• Ordering submarine materials
• this includes the aluminum and acrylic
• any wires needed
• other electrical parts (switches)
• Researching Energy production
• by using enthalpy chemistry, the amount of energy the reaction produces can be determined. This is helpful to determine the efficiency of the reaction and thus how much voltage is created.
• This will be the most important next step

Construction of Prototype

Procedure:

Supplies for the design

For the first phase of our experimenting we are constructing a submarine prototype using a 2-L bottle. We cut a rectangular hole in the side of the bottle to access the interior. In our first design, we used electrical tape to tape two AAA batteries to the top of the bottle. We then took spare copper wires and electrical taped them to the positive and negative ends to the batteries. This totaled four copper wires. These were then lead into the water. The materials we used were a plastic bottle, copper wires, utility knife, electrical tape, 2 AAA batteries, and a 9-volt battery. 

The first design

Experiment 1:

This experiment was using the AAA battery setup. For some reason, either the batteries were not enough voltage (1.5 Volts each to total 3 Volts) or the connections to the poles was not solid enough. In result, nothing happened.

Experiment 2:

This experiment, we substituted the AAA batteries for a 9-volt battery. This reduced the wires from four to two. As shown in the video, the reaction was occurring. 

The electrolysis system

The 9-volt battery and copper wires

Conclusion:

We concluded from our experiment that there needs to be a higher voltage in order for the reaction to work better. This will help with our readings of the amount of volume of gas created. A new wire and possibly an electrode will be used to allow the reaction to run more efficiently. This will be either aluminum, graphite or any other metal that is more efficient (experiments will be ran). There is also an idea that a controlled amount of salt will be added to the water. This will allow the water to be even more conductive due to the extra ions in the water. 

Thoughts

After talking with Prof. Cairncross, we have found out our game plan. We will make a prototype submarine out of a 2-liter sprite bottle, basic copper wires, and two 9-volt batteries. This will allow us to see the reaction and take notes on what we can improve on. We already know that the material of the wires can be better, but copper wire is easy to get and cheap. We will watch the reaction go, and the plan is to use graduated cylinders to measure the volume of oxygen and hydrogen gas formed. This is an important step in the production process of the project.

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

Example of 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.

Lab Number 2

Thoughts

Problem: Copper wire will corrode when the electrolysis reaction occurs.

Solution: Replace copper wire with graphite or another conductor (tests provided) to allow for the reaction to proceed at ease.

• Two 12-volt batteries (or a bunch of 9 volt batteries) will be the basis of the energy for the electrolysis reaction. This should be sufficient enough for the reaction. 
• How big should the submarine be? 
• What materials should it be made out of?
• Aluminum Sheets
• Acrylic sheet for "window"
• How should the volume of gas be measured?
• What conductive material should the wires be made of to be the most efficient?
• Test reaction of each metal in the lab for greatest efficiency. 
• Reaction happens, gas volume measured, THEN what happens to the gas? How is it released?
• In progress

Five Neat Things About Submarines 

This was the article that got myself (Jon) interested in electrolysis in submarines. It also helped me understand what electrolysis 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.