Ping Pong and Golf Ball Velocity

The velocity of a golf ball or a ping pong, or any type of object, you must do either of the equations. The two equations are, D=VxT or V=D/T, each letter is a different measurement of some type. The letters are as follows, D is distance, V is velocity, and T is time. In the lab we did were were given the distances and were were supposed to find the velocity of a falling golf ball and ping pong from 1, 2 and 3 meters. The time from which the ball was dropped to the time it hit the ground was T, time. Once we obtained an average amount for the time, we plugged each one into the equation. 1(D)=Vx.30(T) that was our first equation, each of them being different. After we got our averages and calculated the results for each we found that As the height went up with each the velocity increased, the golf ball increased faster than the ping pong though. We had a few issues with this lab because when we used the vernier motion sensor we picked up many random, stray lines that didn't match up to our math. When we held it at 1 meter, it showed it as somewhere around a half of a meter. Also when we went to 3 meters it showed it as less than two. Other than having issues with the sensor the lab ran fairly smoothly, even though it required quite a bit of math. Our results were, for the golfball velocity at 1 meter was .96m/s/s, 2 meters was .90m/s/s, and for 3 meters, .90 m/s/s. For our ping pong results we got, for 1 meter, .69 m/s/s, for 2 meters, .88 m/s/s, and finally for 3 meters we got 1.13 m/s/s. The final law we investigated was force, F=MxA. In this case the M(mass) was 45.66g for the golfball and 2.5g for the ping pong. The acceleration was just gravity, 9.8m/s/s. So for each we multiplied the mass times the acceleration to receive the force. For the golfball we got 447.468N and for the ping pong, 24.5N. I'm not surprised by the results, it seemed to be pretty close to what I was expecting, if anything the low was lower and the high was higher than I was expecting.

Yeast Beats in Action Investigation

First we took some hydrogen peroxide, poured 3 ml of it into 3 different test tubes. Then we put 3 different mixtures into 3 different test tubes. We put soda, the acidic mixture, into the left, milk, the neutral mix, into the middle and the antacid, the basic mixture, into the right one. For each test, we put 2 drops of yeast into each test tube and measured the pressure for 2 minutes. Our results were, for each test the pressure constantly increased, some faster than others. The soda mixture rose the least, starting at 97.05 and ending at 97.48. The in between mixture was the neutral, milk, which went from 97.03 to 98.46. The highest ending result was, the antacid mixture, starting at 98.36 and ended at 100.53. The results surprised me as to the order they went in. I was expecting to have the acidic mixture be the highest and the base, the lowest. I think that the bases rose the most because they were the steadiest and the yeast "rises" so therefore the pressure in the tubes what increase. But I think that the bases rose the most because they were the steadiest and the acids were unstable.

Conservation of Mass Lab Investigation

In this lab we investigated whether baking soda and vinegar or pop rocks and soda were able to cause a larger chemical reaction. My hypothesis for the lab was that the baking soda would expand about 4 inches and the pop rocks only 3 in.The way we were able to see which was more effective, we took 2 bottles, 1 full of soda the other with about 50 ml of vinegar. Then we poured a half of a teaspoon of baking soda into the vinegar and about a half bag of pop rocks into the soda. Next, we placed 2 balloons on each of the tops of the soda bottles and as each reacted with the other they created gases which floated up and began to blow the balloon up. The baking soda and vinegar only took about 15 seconds compared to the soda and pop rocks which took almost 3 minutes to fully dissolve. Our results were what I expected, the baking soda and vinegar expanded about 1 inch or so larger than the soda and pop rocks which expanded about 3 inches.

Something I realized about the reactions was, the baking soda and vinegar was a chemical reaction which means that ALL the vinegar and baking soda reacts with each other and creates gases. The pop rocks have air trapped inside them so the gases released are limited to how many pop rocks you have. This could have dramatically changed the outcome of the experiment because if you were to take the same amounts of baking soda and pop rocks and mix it with the other ingredient the baking soda would be about 10 times bigger than the pop rocks. The results defiantly differed from table to table because some people may have stretched their balloons more or less and some people may have moved or shook their bottle creating more gases, and increasing the size of their balloon. On average I think the vinegar and baking soda balloons got about 5 in whereas the soda and pop rocks only got about 3-4 in. My hypothesis was correct as far as our tests went, I said the pop rocks would only be about 3 inches and the baking soda about 4. Overall the lab went as expected and there weren't to many errors or mix-ups throughout. The only thing I would have changed was to have gotten 2 of the same size and shape bottles. Instead we just used the same bottle twice rinsing it out in between.

Chemical Reactions Temperature Investigations

For this experiment, chemical reactions, we investigated how chemical reactions change with temperature. We took hot, room temperature, and cold water and dropped an alka seltzer pill into each. My hypothesis for the experiment was that the warmer the water got the faster the the pill would dissolve. We the waters one at a time, room temperature first. The pill dissolved for about 30 seconds and the temperature changed from 23.1 degrees C to 22.7 degrees C. Next we did hot water. It took about 3 minutes to warm up on the hot plate up to 50 degrees C. Once we got it to that, we dropped another alka seltzer pill into the beaker it only took about 22 seconds for it to dissolve and the temperature went from 50 degrees C to 48 degrees C. Finally we used water that was filled with ice. After a minute of stirring we started at .6 degrees C. When we dropped the pill in after about 2 minutes the temperature went from .6 degrees C to .3 degrees C. In the end my hypothesis was correct, as the temperature of the starting water increased, the time of which the alka seltzer pill dissolved was decreased. Also with each test the end result was cooler than the start.

ChemThink Chemical Reactions

1. Reactants

2. Products

3. chemical change

4. rearrangement

5. breaking, forming

6. same atoms

7. missing, new atoms

8. rearrange the bonds

9. 2, 1, 1, 1

A. Cu, O2, CuO

B. 1 Cu and 2 O, 1 Cu and 1 O

10. 2, 1, 2

Number of atoms in reactants- 4, 2

Element- H, O

number of atoms in product- 4, 2

11. The Law of Conservation of Mass

12. mass, atoms

13. 2, 1, 2

14. 1, 2, 1 , 1

15. Cuo, Cu

16. O, Cu, Cu

17. 2, 2, 2

18. 1, 2, 2, 3

19. 2, 3, 2

20. 2, 2, 3

21. 2, 3, 1

SUMMARY:

1. The breaking or joining of different atoms.

2. the same mass

3. number of atoms, atom

Polymer Lab Group Investigation

In the borax-polymer lab today we combined glue, water, and borax. We also added another ingredient, corn starch which caused the result to become stickier and softer. As well as adding corn starch we adjusted the glue and water amounts a little to have less water so that it would be more of a solid. My hypothesis for this lab was, adding cornstarch would make the ball more solid and less of a soft liquid that when set down for a minute would spread into a puddle. When they were mixed together in the right amounts they formed a white sticky substance that we related to marshmallow fluff. We then picked up the fluff and started to knead it into a ball. Halfway through the process we decided to split it in half and put one in the fridge and continue to knead the first ball. We tested it for three things, density, elasticity, and rebound. Our results were, density- soft, elasticity- at least 2 feet, rebound- less than 2 cm. Some of the results were expected but for the rebound of only 2 cm. I was surprised at how little it bounced, for how soft and move able it was I expected at least 6 or 7 cm. About 10 minutes later, we pulled out the chilled ball and tested it for the same things. Our results were, density- soft (softer than the other), Elasticity- 1 foot or more, rebound- 2 cm. Once again I was surprised about the rebound, the others were expected. Considering the ball had been chilled, to me it seemed like it should have bounced a lot more because of it becoming more of a whole and it should stay together more, but it just didn't bounce like I thought it would. In conclusion, the changes in our tests aloud the ball to become softer and stretchier but dramatically dropped in bounce. Maybe next time we could use more water and less cornstarch, but thats just another hypothesis.

Sodium Silicate Polymer Lab

My hypothesis for the lab was that the two liquids would come together to make a solid and when it was tested it would bounce higher than the borax polymer. When forming the borax polymer the combination acted like Play-doh and formed together easily, but the silicone polymer took much more pressing and kneading to form. When the two liquids, silicone and ethanol, mixed together they became like a gel and with more mixing became a crumbly clear-white mess. When I squeezed it into a ball some liquid was squeezed out too, which i believed to be the ethanol. Compared to the borax polymer, the sodium polymer bounced up 15 cm at room temperature compared to 9. When the sodium polymer was chilled and bounced it only went 10 cm and the borax went 6 cm up. My hypothesis was correct but the way the liquids formed a solid was unique and very different than i thought it would be.