Yeast Beasts in Action Lab Investigation

Some of the things that I observed was that for the soda, nothing extreme happened, like

I thought it would. The pressure started out by only changing a range from .1 to .2, so it

was not major. But all of a sudden the pressure changed, and it went up about one. Towards

the end of the testing session, there were bubbles starting to form in the soda. Maybe from the

building pressure. For the stomach antacid, the mixture remained the same, it was foggy

hydrogen peroxide. After we completed the test, the mixture became very bubbly and it was

stirring around. There was also a little amount of foam clinging on the sides of the glass testing

tube. The pressure for this was 100.70.

The one with the greatest yeast activity and pressure was the Diet Coke soda, which had the pressure of 102.7. I think that the carbonation in the soda had something to do with the pressure. Also the carbon dioxide was released inside, and it was trying the find a way to escape. The test that had to slowest yeast activity and pressure was the slim milk. The skim milk pressure was 100.58. Milk has a pH around 6.4 to 6.8, so it is not actually neutral. The soft drink has a pH 3.0 or lower and the stomach antacid has increased pH in your stomach. I did some research on hydrogen peroxide. I found out that it was a oxidizer, that it commonly found in bleach. Bleach, on the pH scale, is one of the most basic, at 12.5. Pure hydrogen peroxide has a pH of 6.2, which will make it a weak acid. So, it really depends on what it is mixed with it. So the basic and the acid will have a different reaction than a acid and acid reaction/pressure.

Some things that I concluded from my results of the experiment was that there the reaction between acids and bases are different, but they can both create very similar pressures, because they were so close. Some of things that went wrong is the experiment was turning the Diet Coke test. After we had added the two drops of yeast, we shook the mixture, but we did not start the test right after. This could have released some of the carbon dioxide, that could contributed to the pressure. Another action was that we had to retest a test, because the data was not collecting any of the pressure.

What can you conclude from the results of your experiment?

Conservation of Mass Lab Investigation

The combination of vinegar and baking soda will cause a very strong reaction. We did not need to shake up the solution in order for the reaction to occur. I researched the reaction between baking soda and vinegar. Baking soda is a pure chemical called sodium bicarbonate, which is the chemical formula of NaHCO3. Vinegar is a weak solution of acetic acid in water, approximately 5%. “The reaction between baking soda and vinegar is actually two reactions, an acid base reaction followed by a decomposition reaction. When the two ingredients are mixed, hydroge

n ions ( H+) from the vinegar react with the bicarbonate ions (HCO3- ) from the baking soda to form a new chemical called carbonic acid (H2CO3). The carbonic acid thus formed then immediately decomposes into carbon dioxide gas (CO2)and water (H2O). It's this carbon dioxide gas that can be seen bubbling and foaming as soon as you mix baking soda and vinegar together.”
Some of the observations I made were the Pop Rocks caused the soda to bubble, which caused the gas to be released. The balloon filled up a little, but it was not the reaction I was expecting. But once we shook the soda and Pop Rocks, the balloon started to fill fast. I also noticed that some of the Pop Rocks were sinking to the bottom, before the carbon dioxide was being released. It was mainly the larger chunks. For the vinegar and baking soda lab, there were bubbles forming in the liquid. The reaction started first away. There was no need to assist the “blowing up” of the balloon. A major difference from the different tests was the size of the balloon. Though we had to shake up the first one, the balloon was much larger than the one for the vinegar and baking soda.
A changing factor t

hat varied from lab table to table was the type of soda used. For my group, we used Coca Cola. After doing so research there are the amounts of carbonated water in the sodas we used today:

Sprite: 92.31%

Coke “Coca Cola”: 95.78%

Dr. Pepper: 96.17%
Because there are different levels, then the amount of carbon realized to create the gas, the ultimately lead to blowing up the balloon. The balloon was not filling up with gases, and thanks to Table 2, we discovered that if we shake the bottle gently, then the Pop Rocks will dissolve faster, which could realize the carbon dioxide. According to the manufactures of Pop Rocks, they contain sugar, lactose (milk sugar), corn syrup, and flavoring. All of the ingredients reach the boiling the point, and they are mixed with carbon dioxide gas under a 600 pound high pressure. I learned that the soda/Pop Rocks is actually not a chemical reaction, but a physical reaction. We had a few things wrong with our experiment. One of my group members accidentally brought in the wrong size empty bottle, only 16.9 FL oz. Some of the people in my group thought that it would be no big deal, but I said that the we needed to have the right size, because that could have been a huge difference. The balloons also there not the best quality. It was hard to put the Pop Rocks into the balloons. We there not able to put the whole package, like we there supposed to. I also tried to blow it up, it try to stretch out, so it could fit more inside, but it did not work. It also was difficult to stretch the balloon to fit it on the bottle opening, without spilling the Pop Rocks into the bottle. The balloons had a hard time filling up for the Pop Rock experiment.

Chemical Reactions and Heat Investigation

My hypothesis was correct. I had predicted that the heat would go the fastest, the room temperature went at a moderate rate, and the cold went had the slowest. The water molecules move faster at a higher temperatures, so they will bump the solute more often. When the water molecules hit, their polar ends attract to the solute's charged ends and they are pulled apart until completely diffused. There also is more space in between the molecules, so the solute can settle in there. Because there is more space, there is more room for the solute to expand and than dissolve. This is the opposite for cold, because the molecules move slower, so it does not dissolve as fast. The major difference between all three test trials, was manifestly the time it took to dissolve. The room temperature test took about 40 seconds to completely dissolve. The hot water test nearly cut this in half, so it was an outstanding 25 seconds. Finally, the cold water test took 1 minute and 55 seconds. Some of the similarities that I noticed between all three of the tests is that it reminded me of carbonated water/soda, because of the bubbles. Also the liquid became very cloudy, right after the tablet was dropped into the water. In every lab/experiment, there always is something that will skew the results. One of the things in our specific experiment would have to do with the temperature probe. In the time during the different sessions, the temperature probe did not have enough time to convert back to room temperature. We tried to weight it out as much as possible, but still was a few degrees off. In the end, this experiment was cool to see the reaction in different temperatures.

ChemThink: Chemical Reactions

1. C H E M I C A L R E A C T I O NS T U T O R I A L Q U EST I ON S

1. Starting materials in a chemical reaction are called reactants.




2. The ending materials in a chemical reaction are called products.




3. The arrow indicates a chemical reaction




4. All reactions have one thing in common: there is a chemical change.




5. Chemical reactions always involve a rearrangement.




6. In all reactions we still have all of the same atoms at the end that we had at the start.




7. In every reaction there can never be any missing atoms or new atoms.




8. Chemical reactions only rearrange the bonds in the atoms that are already there.




9. Let’s represent a reaction on paper. For example, hydrogen gas (H2) reacts with oxygen gas (O2) to form water

(H2O): H2 +O2 = H2O




If we use only the atoms shown, we’d have two atoms of H, and one atom of O as reactants. This would make one molecule of H20, but we'd have no oxygen atoms left. However, this reaction only makes H20.




Remember: reactions are not limited to 1 molecule each of reactants. We can use as many as we need to balance

the chemical equation.

A balanced chemical reaction shows:

a) What atoms are present before (in the reactants) and after (in the products)

b) How many of each reactant and product is present before and after.




10. So to make H2O from oxygen gas and hydrogen gas, the balanced equation would be:




2 H2 +2 O2 = 1 H20




Which is the same as:







# of atoms in Reactant	Element	# of atoms in Products
2	H	2
2	O	1




11. This idea is called the Law of Conservation of Mass.




12. There must be the same mass and the same number of atoms and after the reaction (in the products).




13. What is the balanced equation for this reaction? before the reaction (in the reactants)




2 Cu+ 1 O2 = 1 CuO




14. In the unbalanced equation there are:




Reactants>




Cu atoms 1




O atoms 2







Products>




Cu atoms 1




O atoms 1




15. To balance the equation, we have to add CuO molecules to the products, because this reaction doesn't make lone O atoms.




16. When we added a molecule of CuO, now the number of O atoms is balanced but the number of Cu atoms don’t match. Now we have to add more two Cu atoms to the reactants.




17. The balanced equation for this reaction is




2 Cu + 2 O = 2 CuO




This is the same thing as saying:




Reactants




# Cu atoms 2 = # Cu atoms 2




# O atoms 2 = # O atoms 2







Products




# Cu atoms 2 = # Cu atoms 2




# O atoms 2 = # O atoms 2




18. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.)




1 CH4 + 2 O2 = 2 H20 + 1 CO2







# of atoms in Reactants	Elements	# of atoms in the Products
1	C	1
4	H	2
2	O	3







19. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.)




1 N2 + 3 H2 = 2 NH3







# of atoms in Reactants	Elements	# of atoms in Products
2	N	1
2	H	3







1. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.)




2 KDIO3 -> 2 KCI + 3 O2




1. 













1. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.)




4 Al + 3 O2 -> 2 Al2O3







# of atoms in Reactants	Elements	# of atoms in Products
1	Al	2
2	O	3










SU M M A R Y




1) Chemical reactions always involve breaking bonds, making bonds, or both.




2) The Law of Conservation of Mass says that the same atoms must be present before and after the reaction.




3) To balance a chemical equation, you change the coefficients in front of each substance until there are the same number of each type of atom in both reactants and products.

Polymer Lab Group Investigation

We mixed glue, water, yellow food coloring, and ethanol. Then on the side, borax and the sodium silicate were combined. It is amazing how changing the order and ingredients could change the experiment all together. I mean, we used the similar amounts and the same ingredients, but they there ultimately added together, in the end. The result of our experiment looks like a cross between brains and scrambled eggs. I was not expecting this. I thought that by combining the two experiments, that it would be a fusion of the two end results: a hard core (for the sodium silicate experiment) and a “squishy” body (for the glue experiment.) I was shocked by the results of the lab. I thought that it was weird that the 75 mL of glue did not make the solution sticky, I thought it would. The borax did not dissolve all the way, which made the ending result feel grainy (we added 3 mL to start). I feel like we added too much.

The components and chemicals in the yellow food dye did not really effect the results, so to me, it was deemed unnecessary. It did however added to the effect that the solution looked like scrambled eggs. The solution mixture was very thin, and liquid based. I thought that by adding a tablespoon of Borax, that the solution would thicken. It did. We added another tablespoon (5 tablespoons total) because the solution was little a little runny. This was a little too much, because the borax would not dissolve. We stopped stirring, before the borax was able to. When we tried the rebound test, all the solution did was flop on the table. This happened for each of the trials, so the rebound was 0 cm. The first time we dropped it from 30 cm, there was a small explosion of borax and a small amount of ethanol.

We torn off a chunk, to see if maybe a smaller amount would at least get a rebound. It worked, but it only got to a few centimeters. We froze the smaller piece in a glass beaker, and with the larger one, we chilled it in the refrigerator. We removed the large solution 15 minutes after. There was a small round, but too small to be able to measure. I think that this was due to the heat the hands provide. One of the ways that heat escapes the body is through the hands, so the “chill” heated up. My fellow group members were playing with it in their hands, before the rebound test was completed. We took to the smaller piece out of the freezer, 20 minutes later. It had a surprising rebound, averaging 6-7 centimeters.

Sodium Silicate Polymer Investigation

I was not expecting the results of today's lab. I did not think that the ending results would look like a "bouncy ball." A major difference between today's lab and Tuesday's lab was the procedures leading up to the conclusion. For example, when we began to stir the different solutions, the glue/borax solution took a longer time to become a solid and interfuse together. When we stirred up the sodium and ethyl alcohol, the results where instantaneous. Another difference was the overall look and feel of the solutions. Obviously with the glue, the solution was sticky and a pure white coloring. The sodium silicate solution, was transparent. If the glue solution had to be described in an everyday item, it would have to be marshmallow jet puff or taffy, because they have very similar looks and textures. If the sodium silicate had to be described, it would be a bouncy ball, because of the heights it got to, the sound, and the texture of it. Also, each experiment where manifestly used to create different polymers, using different ingredients. It is harder to shape the glue solution because, due to evaporation, the moisture inside the ball started to escape. When I started to roll it into a ball, there was a sudden realize of liquid, from the inside of the ball. The sodium/alcohol just needed a little water and some elbow grease and walla, it was a perfect circular ball. A more chemical difference is that sodium silicate bonds with four oxygen bonds, whereas silicon only binds with 2 carbon atoms. One of the similarities would be that the atoms of each chemical had to combine, in order to create the bond. If they did not combine, then there would be two layers of the solution: both different. The combining ultimately lead to the fusion to create the final ball. Another similarity is between silicon and carbon. Both carbon and silicon make four chemical bonds and can be branched out into four different directions to make a long chains. They both can combine with each other and other elements, in order to create many great elements.

Some problems that we encountered was that we were not a to see exactly 3 mL, because the graduated cylinder did not go all the way down to that. We just estimated by pouring the liquid a little under the 5mL cut off. We also did not use of the of the sodium silicate/alcohol mixture. This could effect the mass of the ball, when we dropped it to record the rebound. The extra weight could have changed the height. Gravity and weight go hand in hand. It is a myth that says heavier things fall faster, but it can cause the ball to bounce higher. For question 6, a major difference between the group's balls, would be the size of them. The size is basically saying that the mixture of the solution would make more of the material used to create the balls. The ball we made was smaller than other groups. Another thing is that people had a difficult time trying to put the ball together. Because they were drowning it in water, the solution could a broken down. Their hands could have removed solution from the ball. You could see how much liquid that came out of the ball by using a container. If you rolled the solution into a your hands, do it above the container, so that the extra fluids drip out, and you are able to measure the amount. Silicone has the potential of replacing plastic.