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Wednesday, March 23, 2011

Yeast Pressure Investigation

Today we investigated yeast activity and air pressure in Yeast Beasts in Action. We wanted to know how yeast activity varied in acidic, neutral, and basic mixtures. In order to perform the investigation you need 1 teaspoon of yeast, 50mL of water, 2 beakers, 1 gas sensor, black rubber stopper, 3 test tubes, 1 test tube rack, soda, milk, antacids, Vernier software, laptop, LabQuest Mini, graduated cylinder, 3% hydrogen peroxide, and an eye dropper.

First we set up the Vernier software and connected all the sensors with the LabQuest Mini. Then we placed the three test tubes on the rack and labeled them A, N, and B. Then we measured out 3mL of hydrogen peroxide and poured it into each tube. Then we made our yeast solution by filling up one of the beakers with 50mL of water and 1 teaspoon of yeast and stirring. We used the eye dropper to add 2 drops of the yeast solution to Test Tube A. Then we added 3mL of the soda and put the rubber stopper on top. We then collected the data and recorded the highest pressure of Test Tube A. We waited after the 2 minute mark until the pressure started going down so that we could get a more accurate pressure amount. We repeated these steps for the next two tests, but we used milk and antacids for the mixtures.

My hypothesis was: If yeast breaks down and releases the gas of compounds, then the acidic mixture will have the highest pressure because the other two mixtures will have lower kPa.
The reason I thought that the neutral and basic would have low pressure was because the neutral mixture (milk) would be cold which (as concluded from a previous lab) causes a lower pressure and the antacids neutralize acidity, so I did not think that they would cause a high pressure.

My hypothesis was close, but was not exactly supported by the data. The chart below shows the results of the tests:

Basically, the Basic mixture ended up having the highest pressure at 128.3 kPa. The Acidic mixture was close with 122.13 kPa. Last was the Neutral mixture with 117.19 kPa.
Below are charts containing the pressure info for each mixture:
(The Acidic Mixture)
(The Basic Mixture)
(The Neutral Mixture)

Thursday, March 17, 2011

Law of Conservation of Mass Investigation

Today we investigated mass and weight in the Conservation of Mass Investigation. In order to complete the lab investigation we needed 1-2 packets of pop rocks, 2 balloons, 2 twenty ounce soda bottles (one empty, one full), 1 tsp. of baking soda, 50mL of vinegar, a funnel, graduated cylinder, and a plastic spoon. There were two tests to complete, the Pop Rocks test and the Baking Soda/Vinegar test. Our problem was: What will happen to the balloon when the Pop Rocks are dropped into the bottle? Our hypothesis was: If we put the balloon on the bottle and drop the Pop Rocks, then the balloon will inflate because of the carbon dioxide in the Pop Rocks that will be released.

We began with the Pop Rocks test by pouring out half a packet of Pop Rocks into one of the balloons. First we had to stretch the balloon to make it more flexible. Then once the balloon was filled we attached the balloon to the soda bottle, but we did it in a way so that the balloon was at the side of the bottle and we could control went to drop in the Pop Rocks. Like this:

Then we poured it into the bottle, and watched. Basically what happened was the balloon stuck upright, and the part of the balloon covering the opening in the bottle filled up slightly. The Pop Rocks fizzed and dissolved in the soda. When we looked around, compared to other groups' balloons, ours had not been filled up much at all. It may have been because we were only able to use half the packet of the Pop Rocks, or maybe because we did not stretch our balloon very long. Then we got the idea to shake our bottle from one of the other groups, it maybe released the carbonation from the coke because the balloon started inflating a lot more. Soon there was only two inches of balloon not inflated. It looked somewhat like this, but the balloon was much smaller:

Then we did the baking soda and vinegar test. We went through pretty much the same procedures, except we used the empty bottle and filled it with 50mL of vinegar. Then instead of Pop Rocks, we filled the balloon with baking soda. Then we attached the balloon onto the bottle and poured in the baking soda. The second the baking soda touched the vinegar it started bubbling and fizzing. In less than three seconds the vinegar-baking soda had bubbled up to the top of the bottle and the balloon had fully inflated. But, the reaction soon ended, just as quickly as it happened. The vinegar mixture bubbled back down to the bottom of the bottle, and the balloon deflated slightly.

My hypothesis was supported, because it was pretty much what happened. I did not know all the details of how the balloon would be inflated, but I knew carbon dioxide was inside of the Pop Rocks, and figured it would end up inflating the balloon. Now I know exactly how it worked. When being made, Pop Rocks are boiled at a very high pressure with carbon dioxide, and the end result is tiny bubbles of carbon dioxide compressed at 600 PSI inside the candies. So when they are opened up or dissolved, the carbon dioxide is freed. So when put in the bottle of soda, the Pop Rocks were dissolved and the carbon dioxide went up into the balloon. Something else that I left out in the hypothesis was that the soda also contributed to the inflation of the balloon. But after some research, I found that the Pop Rocks actually released carbon dioxide from the soda. So the soda also helped inflate the balloon.

Something I thought was interesting was that the Pop Rocks and soda test did not show a chemical reaction, but a physical reaction. The reason is being that the soda is just dissolving the Pop Rocks which releases its carbon dioxide, and there is no real reaction.

Tuesday, March 15, 2011

Chemical Reactions and Temperature Investigation

Today we had a Chemical Reaction and Heat Lab Investigation where we investigated how temperature varies chemical reactions. The materials needed for this lab investigation were a 600mL beaker, a stirring rod, metal tongs/clamps, Vernier software, temperature probe, ring stand, graduated cylinder, 3 alka-seltzer tablets, stopwatch, hot plate, ice cubes, laptop, and 665mL of water.

My hypothesis was: If increased temperature increases the reaction rate, then the Hot Test will have the quickest dissolve time because it has the highest temperature. In order to find out if this hypothesis would be supported or not, I had to complete the three tests: Hot, Room Temperature, and Cold. Each test involved filling the beaker up with water, getting it to a certain temperature, and dissolving the tablets in the water. The difference was that the Hot test used a hot plate and needed to go up to 50 degrees Celsius, the Room Temp. test just needed to be regular water, and the Cold test needed ice cubes.

Our results are shown in the chart below:

The proved our hypothesis to be true because the Hot test ended up having the shortest dissolve time (23 seconds). Room Temperature was only 16 seconds behind, and Cold was 97 seconds behind. Basically, hotter temperatures will tend to quicken the rates of chemical reactions (especially when concerning the dissolving of something).

Below are diagrams of how the beaker looked for each test.
This was my diagram for the Room Temperature test. Bubbles were flying from the alka-seltzer tablet (as shown in diagram). In fact, the bubbles were coming so rapidly that the tablet was spinning round and round until it settled back at the top to dissovle into foam.

Then there was the Hot test, immediately after the tablet was dropped into the heated water it started to fizz. All around the tablet was bubbly foam, unlike the Room Temp. test, bubbles did not start spurting out until a little later. It mainly just fizzed.

Last was the Cold test. There were bubbles during the Cold test, but they were rather large and came very slowly. After about a minut the tablet started to really fizz and then it started looking like the Room Temperature beaker.

Friday, March 11, 2011

Chem Think; Chemical Reactions

1. Starting materials in a chemical reaction are called:
1A. Reactants

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

3. The arrow indicates a __________ has taken place.
3A. A chemical change
4. All reactions have one thing in common: there is a ______ of chem. bonds

5. Chemical reactions always involve ______ old bonds, ______ new bonds, or both.
5A. breaking, forming

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

7. In every reaction there can never be any __________atoms or ________
7A. missing, new

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

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 two atoms of O as reactants. This would make one molecule of H2O, but we’d have one atom of O leftover. However, this reaction only makes H2O.

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:

____ H2 + _____O2 ---> _____ H2O

Which is the same as:

11. This idea is called the _____________
11A. Law of Conservation of Masses

12. There must be the same _____________ and the same number of _____________
before the reaction (in the reactants) and after the reaction (in the products).
12A. elements, atoms

13. What is the balanced equation for this reaction? 2Cu + 1O2 → 2CuO

14. In the unbalanced equation there are:
15. To balance this equation, we have to add ______ molecules to the products, because this reaction doesn’t make lone _____ atoms.
15A. CuO, oxygen

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

17. The balanced equation for this reaction is

2 Cu + 2 O2 ---> 2 CuO

This is the same thing as saying:

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 H2O + 1 CO2

19. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.)
2 N2 + 3 H2 → 2 NH3

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

2KClO3 → 2 KCl + 3 O2

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


1. Chemical reactions always involve:
1A. breaking and/or making bonds

2.The Law of Conservation of Mass says that the same atoms must be:
2A. present prior and after the chemical reaction

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

Wednesday, March 9, 2011

Polymer Lab Group Investigation

Polyvinyl Lab Group Investigation: Polyvinyl Acetate and Borax Investigation

After the first polymer lab, my group was inspired to further investigate the properties of borax for our next investigation. We wanted to know if borax was truly responsible for the flexibility and rebound of the polymer. In this investigation, we completed three trials: Trial 1 would be the control (nothing would change), Trial 2 would be our variable (35 mL of borax solution), and Trial 3 would be another variable (15mL of solution). The control is used to compare the other Trials with. Trial 2 will allow us to see if more borax solution will allow more “cross-linking” thus leading to tighter bonds and more flexibility/higher rebound. By completing Trial 3, we can back up our theory of Trial 2, because if our theory is correct, then the polymer in Trial 3 will not have much flexibility or very high rebounds. Our hypothesis was If the polymer is most flexible and achieves the highest rebound tests in Trial 2 (the trial using more borax solution), then the borax is responsible because more borax solution was used in it, thus proving that more borax=more flexibility. If our hypothesis was correct, the results should have shown the polymer in Trial 3 to be less flexible or have not very high rebounds. Also, Trial 2 should have shown to be very flexible and fairly high rebounds (in comparison to Trial 1).

As it turned out, Trial 2 did have the highest average (14 cm) for the rebound tests, Trial 3 had the shortest (5.3), and Trial 1 was right in between (10.3). Trial 3 was incredibly mushy, wet, and sticky. It was so wet and sticky that it did not really bounce at all when dropped, and it was very difficult to drop due to it sticking to our hands. Below is a picture of what the Trial 3 Polymer looked like:

Here is what all three Trials looked like side by side:
Trial 1 was soft and moldable. Trial 2 was very firm, it was also stickier than Trial 1, but not squishier. It was also a lot denser. Trial 3 was watery and loose and shapeless. Something that I noticed was that after the removal of Trial 1 polymer, there was a little bit of water and some glue bits left over in the beaker. After the removal of Trial 2, there was at least 30mL of water in the beaker along with glue bits. After the removal of Trial 3, there was no water left, but there was some glue left. I think this is partially because we may have taken out Trial 2's polymer too early, and we may have taken out Trial 3's polymer too late. Thus the polymer soaked up all the water which may have resulted in it's watery-ness.

Then there were the flexibility tests. Below is the chart containing information for all of the tests.

To sum up all the information, at 54 cm, Trial 3 had the most flexibility, at 37 cm, Trial 1 had the second most, and at 26 cm, Trial 2 had the least. There are many explanations for this, but I think that perhaps our information is not completely correct. For one thing, different group members stretched the polymers, which would mean some of them may have been stretched harder and faster or slower. This could speed up the breaking of the polymer, or slow it down. Another thing is that with Trial 3, as mentioned previously, it had been left in the beaker the longest, resulting in it sucking up all the water and being very flexible. Although, Trial 2 was definitely not very flexible, despite the variables. It snapped easily, and was not all that flexible.

In conclusion, our hypothesis was partially correct because Trial 2's results did show that more borax provides more rebound, but it does not necessarily provide more flexibility.

Thursday, March 3, 2011

Sodium Silicate Polymer Lab Investigation

How do you make a sodium silicate polymer? That is the question we answered in our latest lab investigation. This is my hypothesis (what I thought was going to happen): If you mix ethyl alcohol with a sodium silicate solution, then you will make a polymer because when sodium silicate is added to ethyl alcohol, silicate chains form and the oxygen atoms of the silicate are replaced by ethyl. In order to find out if this hypothesis was supported, we mixed 12mL of sodium silicate with 3mL of ethyl alcohol. A polymer was formed, thus proving our hypothesis to be correct. We then rolled up the polymer into a ball, and went through some rebound tests. Then we froze the polymer ball, and went through the rebound tests once again. Below is a graph showing our results:

As with our first lab, once the polymer was frozen, it bounced slightly lower. When we compared our results with the group behind us, we discovered that our ball bounced slightly higher, and was smaller in diameter. Our ball turned out pretty good, but not very easily. At first we thought we might even have to start over because the polymer would not form. We had to put it under a lot of water because it got squished when we were rolling it. The polymer was squishy and moldable, but only if you touched it. Otherwise it stayed firm and held it's shape. It was sort of white, and also see through. It looked very similar to an ice cube or frozen water.

Sort of like this: After we froze the ball it became almost completely white and opaque.

We had originally done a lab about polymers that involved borax and glue, where we also made a polymer. Below is a diagram that I created to compare and contrast the two polymers:
Carbon is the basis of much life on Earth, the next best thing, as many believe, would be silicon. Silicon has an equal number of electrons in it's outer shell as carbon. This means that silicon can also create four bonds just like carbon. Certain types of carbon molecules (like carbon dioxide) derive from silcon.

Silicone polymer is a synthetic polymer created with silicon. It is a plastic polymer as well. It is similar to plastics, since it is a plastics polymer.

I know that a chemical reaction has taken place between two mixed liquids when they change their state of matter. For example, when borax solution is mixed with glue solution, a chemical reaction occurs and the mixture becomes solid instead of liquid. Same with ethyl alchol and sodium silcate.

I could find out what liquid was pressed out of the mass of a crumbled solid as I formed the ball by looking at it, and studying it. Also by smelling it, and if I knew what had been used to create the ball, I could probably make a hypothesis as to what it was.

When I compared my group's polymer ball with another group's, I discovered that the other group's "super ball" was a lot larger in diameter, and it also bounced a lot lower. After the other group's ball was frozen, it's highest bounce was 10cm, and ours was 14cm.

Tuesday, February 22, 2011

The Science of Addiction

Natural Reward Pathways (Section 1)

Neurons are in charge of transmitting neurotransmitters through the brain. They have specific functions such as holding memories and muscle control. The brain has many sections, in the middle of the brain is a section known as the reward pathway. This region is in charge of the emotions motivation, reward, and behavior. It's main role is to "reward" us by making us feel content when we commit an act or behavior beneficial to our life such as eating, drinking, and sex. The reward pathway has connections that let it know what is going on outside the body. The connections also makes the brain circuits that regulate desirable behavior stronger. Our senses of taste, touch, smell, sight, and hearing allow us to obtain knowledge of our environment/surroundings and let our brain know through signals that there may be something desirable near us. There is another section in our brain that contains a memory that tells us once you eat you are not hungry any more and you are feeling pleasant. Our senses notify the brain that you are eating tasty food and filling up your appetite. Special neurons release dopamine and give you a jolt of happiness. Thus you are rewarded for eating food. Not only do you feel pleasure, but you are encouraged to do this behavior again whenever you can by the reward pathway through connections to memory and behavior regions. The wiring for behaviors that aid you in your rewarding are strengthened when the reward pathway notifies the motor center of the brain. Thus the feeling of happiness makes us want to repeat our behaviors, and keeps us alive.

The synapse is what sends neurotransmitters from neuron to neuron. Scientists previously thought that neurons were the most valuable brain cells. Now it is known that there are other cells that have important contributions to brain functions.

Drugs Alter the Brain's Reward Pathway (Section 2)

Any drug that is addictive always alter the brain's reward pathway. Some examples of some drugs of abuse are: alcohol, steroids, cocaine, GHB & Rohypnol, hallucinogens, heroin, inhalants, marijuana, methamphetamine, ecstasy, and nicotine. All of these drugs have addictive qualities and terrible side effects. The synapses in the brain undergo immense changes seconds after the drug enters your system. (The faster the drug enters you, the more addictive it is.) The drug activates the reward system and makes you feel a sudden happiness or pleasure. This happens because the drug is able to trick cells into transmitting lots of dopamine in the synapse, which brings that jolt of pleasure. The brain is stimulated so immensely that it tries to develop a coping mechanism. The brain tries to lessen the amount of dopamine receptors so that the person using the drugs "comes down" and will need more of the drug to get high. This action by the brain is known as tolerance. As the brain changes and alters to adapt, other parts of the brain besides the reward system begin to get affected. Some examples of sections of the brain that are affected when the brain adapts are the judgement, memory, and learning sections. They become hard-wired, meaning getting drugs becomes a reflexive habit. The drug user becomes a drug addict. In brains addicted to meth, neurons on the exterior of the brain reward system have especially long and thick dendrites compared to a normal brain dendrite. Some other pathways affected besides the reward system are the dopamine and serotonin pathways. Serotonin controls happiness, so it is commonly used in antidepressants. Then there is glutamate and gamma-aminobutyric acid (GABA). They are both neurotransmitters that work together to regulate multiple processes in the body. Glutamate begins action potential and GABA ends it. Many addictive drugs affect glutamate and GABA resulting in stimulating effects. Drugs are so overwhelming to the brain and body that even a slight overdose will overload the body and kill you. Glutamate and GABA control many of the important processes in the body, as aforementioned, and one of them is the regulation of breathing. Drugs will decrease/increase the glutamate or GABA and make you stop breathing. Which results in death.

Wednesday, January 19, 2011

Great Discoveries in Chemistry

Great Discoveries in Chemistry

It was first suggested by Leonardo Da Vinci that the air was made up of two gases. Later on in 1774, Joseph Priestley did an experiment with mercury to find out if Da Vinci was correct. Priestley came across a gas with an unusual property. This gas would come to be known as oxygen. Basically Priestley literally discovered oxygen, but it was Antoine Lavoisier who really discovered it. Lavoisier was notified of Priestley's discovery by Priestly himself. Lavoisier redid Priestley's experiments and named the gas oxygen. Then John Dalton made a tremendous discovery. He came up with an atomic theory. Dalton proclaimed that atoms of a certain element are unlike any other atom of another element, atoms of the same element are alike, chemical compounds can be created when atoms from different elements combine, atoms cannot be created, divided, or destroyed, and that atoms make up elements. Dalton also discovered atomic weights which he called ultimate particles, and weight of elements. Also in the early 1800s Joseph Louis combined equal volumes of gases to find out that they had equal reactions. It was discovered that gases were not made out of single atoms, but multiple ones which were molecules. Then in the 19th century urea was discovered. A scientist noticed that something had crystallized in one of his tubes with two organic chemicals. The theory of organic chemical reactions had been stumbled upon! It was the underlying base and building block of organic compounds. Then August Kekule created a device for chemical molecules, using symbols resembling chain links. But there was one compound that would not fit his equation. Kekule was puzzling over it when he dreamt of a snake that bit its tail to form a ring. The six carbon atoms of benzine were discovered, they form a ring, like the snake. One or more carbon atom is inside every organic compound. This meant a new recipe for medicine and wonderful possibilities. Then in 1869, a German teacher named Demetri Mendelev created the periodic table of elements. He needed a way to teach them all to his students so he wrote out 63 elements on cards and sorted them and wrote their atomic weight, typical properties, and similarities. When he was complete, he realized he had created a map showing exact relationships between elements. Mendelev had forever changed the way of learning and comprehending the elements. There is an element named after him, Mendelevium. Then Humphrey Davie in 1807 conducted a battery experiment with melted pot ash. Pure potassium emerged, this brought about aluminium, solar panels, LED, and lithium batteries. Next was Robert Bunsen and Kierkoff in the 1850s. They conducted an experiment with a prism and pieces of a telescope. The end result? A spectroscope. With this new instrument they saw a spectrum of colors and dark lines that indicated what atoms were present. Cesium was discovered using this. Then a professor at Cambridge, Joseph Thompson, discovered he could extract a small piece from an atom while trying to find the ratio of charge in mass. Thompson discovered a subatomic particle. Later on Earnest Russerford showed positive sides of atoms located in the nuclei. A mechanism to combine atoms and create new substances was discovered by Gilbert Lewis. Separately sodium and chloride can be dangerous, but it was discovered that when sodium gives an electron from its outer shell to chlorine's outer shell, it forms sodium-chloride: table salt. Then there were the X-Rays . Investigation on special radiation/mysterious radioactive rays French Physicist, Ambre Beckrow tested uranium put objects on top of photographic plate develop plate, ghostly image would appear. He
discovered it was uranium. Marie Curie/husband boiled and sifted uranium, isolated two of them, radium and polonium. In a way, Marie Curie discovered radiation poisoning. Earnest Rutherford discovered radioactive material goes through natural decaying process emits unstable rays. Came across alpha and beta particles and gamma rays. Radioactivity has given us a method for earth's age calculation, spacecraft power source, cancer treatment, smoke alarms
Then there was the discovery of plastics in the 1860s, John Hyatt had discovered a way to exploit cellulose by creating plastic. Leo Bakeland came up with Bakelite, a polymer which are long chain molecules that are extended chains of carbon atoms, sometimes other objects. Plastic is moldable and strong and can mimic/surpass natural fibers. Making polyethlane, plexiglass, etc. polymers are example of human creativity in chemistry. Nanotubes are 1 billionth of a meter, thinner than DNA strands. Richard Smalley studied chemical conditions in space
searching for chemical nature of interstellar matter. A cluster of carbon atoms (60 approx. named buckyballs. Formally known as fullerenes. Most symmetry than any other molecule discovered. Then new fullerenes were discovered, pure carbon forming nanotubes, buckytubes. Have 12 pentagons, buckytubes are stiffer than steel/diamond. They are very stretchy, the strongest fiber ever. We can convert coal/tires/etc. into buckytubes. It is thought that carbon nanotubes are the modern day Industrial Revolution. Nanotechnology is, technically speaking, chemistry.