Yeast Beasts in Action Lab Investigation

Problem: What material tested will have the greatest amount of gas pressure?

Hypothesis: The acid solution will produce the most gas pressure.

The acid substance (which was made of 3 mL of Diet Coke™ and 3 mL of hydrogen peroxide) was put into a test tube and two drops of the yeast solution (1/2 teaspoon of yeast and 50 mL of water) was added. The gas pressure of this mixture is in the table below.

Overall, the acid solution had a gas pressure of about 98 kPa (kilopascals).

Next, we tested the neutral solution. This was made of 3 mL of hydrogen peroxide and 3 mL of skim milk. The same amount of the yeast mixture was added and mixed. The results of this test is below.

Overall, the kPa of this test was about 97.3.

Lastly, we tested a basic solution made up of 3 mL of hydrogen peroxide and 3 mL of stomach antacid. The yeast was added and the results of this test are below.

The pressure in this test increased by just over 2 kPa.

The graph above shows the results of all three tests. The acid test is in red, the neutral is in blue, and the base is in green. The base had the highest gas pressure and the neutral solution had the least. I think that the reason for this is because it has hydroxide ions in it while the acid had hydrogen atoms. Hydrogen is the lightest element known to man and that lack of mass might have something to do with the amount of pressure. The hydroxide is made of hydrogen and oxygen atom stuck together and it can create an acid when the oxygen atom is released. I think that the hydroxide and hydrogen are pretty much the same, except for that extra oxygen atom and that's what makes the difference in the gas pressure.

Conservation of Mass Investigation

Conservation of Mass

Problem: How much gas will be released when pop rocks are dropped into a 20 oz bottle of soda and how much gas will be released when baking soda is dropped into vinegar?
Hypothesis: The balloon over the pop rocks and soda will be 3 inches tall when it is full of gas and the gas from the baking soda and vinegar will fill the balloon to be 6 inches.

Results:

This picture is of the soda and pop rocks. The balloon was filled with about three inches of carbon dioxide.

This picture is of the baking soda and vinegar and this balloon was filled with about 4 inches of carbon dioxide.

Conclusion:
My hypothesis was partially correct because the pop rocks and soda balloon was 3 inches long and the baking soda and vinegar was longer than the pop rocks and soda lab, but it wasn’t quite as long as I had expected. It may have been as long as I had thought, but some air was let out of the balloon when we were trying to find a way to block it. It may have been longer if this had not occurred. Other problems we ran into, were with the balloon because it was not very sturdy and this may have changed the results. If I were to repeat this lab, I would try using a different type of soda to see if it made any difference. With the soda and pop rocks, the reaction took about 2 minutes and 30 seconds. With the baking soda and vinegar, however, the reaction lasted for about 15 seconds. The pop rocks test demonstrated a physical change because the acidity in the soda melted the candy of the pop rocks to release the carbon dioxide trapped inside the pop rocks into the balloon. The baking soda and vinegar demonstrated a chemical change and all of the atoms reacted together to release the carbon dioxide. Even though it appeared that some of the material was lost when the baking soda and vinegar were combined, all of the mass was still there, just in a different form. It had a different weight because some of the liquid became carbon dioxide. It was the same process with the pop rocks and soda because there was less weight when the carbon dioxide was released, but none of the atoms disappeared, just changed forms.

Chemical Reactions and Temperature Lab Investigation

Problem: How does temperature affect the chemical reaction time?

Hypothesis: When tests are conducted at room temperature, cooled temperature, and heated temperature, the heated water will dissolve the tablet the fastest and the coolest test will be completed the slowest.

Observations and Conclusions:

As I expected, the heated water caused the Alka-Seltzer tablet to dissolve faster than the cooled or room temperature water. The results from each of the tests is in the table below.

In each test, bubbles rose to the top directly after the Alka-Seltzer tablet was dropped in. Even after the chemical reaction stopped taking place, the bubble continued to rise. The element that makes water hot is the amount of energy being conducted. The energy at use also makes the Alka-Seltzer tablet dissolve faster than the cold or room temperature water would because there is more energy in use. Although there is energy in all water, in the cold and room temperature water has potential energy while the hot water has kinetic energy. The bubbles also rose faster in the hot water.

Cool water sinks and the ice cubes in the water floated. All of this contributed to the slow pace of the dissolving Alka-Seltzer tablet. The cold water kept the tablet at the bottom of the beaker which meant that the dissolving tablet had a much more difficult task of rising to the top of the beaker. The ice also blocked the path of the bubbles traveling upwards.

In the room temperature water, the Alka-Seltzer tablet was not being dissolved by the quick paced energy flowing through, but it was not being forced down by the lack of energy either. It was right in the middle. As you can observe from the table above, the time that this test took was shorter than the cold test and longer than the hot test.

The temperature (which is also the flow of energy or the lack of energy) is very important when dissolving a solvent into a solute. The time is very much impacted by the pull downward of the cold temperature or the pull upwards of the heated temperature.

ChemThink; Chemical Reactions

All chemical reactions involve either breaking bonds, forming bonds, or breaking and forming bonds.

When conducting a chemical reaction, the compound composition is used (example: Fe+S= FeS)

In the final product, all of the same molecules are used as what we started with.

The same amount of molecules is not necessary for all of the molecules. They do not have to be balanced because if they are, they would make completely different compounds that what were needed. (example H2+O2 H2O. H4+O2=H2O This is now considered to be balanced because it shows us how many product and reactant will be present. Each atom in the reactant side will be present in the product side.)

The Law of Conservation of Mass: There can never be more or less atoms before the reaction as compared to after the reaction. This also means that it will have the same mass before and after the reaction.

Chemical reactions rearrange the atoms present.



Chemistry is the basis of almost all science and benefits thereof, without chemistry we would not have many of the wonderful things we have access to today, like normal milk, its pasteurized by a process that requires basic knowledge of chemistry.





CHEMICAL REACTIONS TUTORIAL QUESTIONS:
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 change has taken place.

4. All reactions have one thing in common: there is a breaking, bonding, or both of chemical bonds.

5. Chemical reactions always involve broken old bonds, forming of new bonds, or both.

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

7. In every reaction there can never be any more atoms or less atoms on one side than there are on the other.

8. Chemical reactions only balance 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 + O2H2O

If we use only the atoms shown, we’d have 4 atoms of H and 3 atoms of O as reactants. This would make 2 molecule of H2O, but we’d have 1 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:
___4_ H2 + ___2__ O2 ___=__ H2O Which is the same as: 2H2O


11. This idea is called the Law of Conservation of Mass
12. There must be the same coefficients and the same number of atoms before the reaction (in the reactants) and after the reaction (in the products).

Element	# of atoms in Reactants	# of atoms in Products
H	4	4
O	2	2

13. What is the balanced equation for this reaction?
__2__ Cu + ___1__ O2 =___2_ CuO

14. In the unbalanced equation there are:
Reactants Products
# Cu atoms __2___ = # Cu atoms ___2__
# O atoms ___2__= # O atoms ___2__


15. To balance this equation, we have to add __1____ 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 __Cu___ atoms is balanced but the number of _O___ atoms don’t match. Now we have to add more __O___ atoms to the reactants.

17. The balanced equation for this reaction is __2__ Cu + ___1__ O2 =__2__ CuO

This is the same thing as saying:
Reactants # Cu atoms __2___ = # O atoms ____2_ =
Products # Cu 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__ H2O + __1___ CO2


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

20. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) ___2__ KClO3 = ____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.) ___4__ Al + __3___ O2 =__2___ Al2O3

SUMMARY

1) Chemical reactions always involve the breaking of bonds, the forming of bonds, or both.

2)The Law of Conservation of Mass says that the same atoms must be the same before the chemical reaction and after the chemical reaction. They must also have the same mass.

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

When conducting a chemical reaction, the compound composition is used (example: Fe+S= FeS)

In the final product, all of the same molecules are used as what we started with.

The same amount of molecules is not necessary for all of the molecules. They do not have to be balanced because if they are, they would make completely different compounds that what were needed. (example H2+O2 H2O. H4+O2=H2O This is now considered to be balanced because it shows us how many product and reactant will be present. Each atom in the reactant side will be present in the product side.)

The Law of Conservation of Mass: There can never be more or less atoms before the reaction as compared to after the reaction. This also means that it will have the same mass before and after the reaction.

Chemical reactions rearrange the atoms present.



Chemistry is the basis of almost all science and benefits thereof, without chemistry we would not have many of the wonderful things we have access to today, like normal milk, its pasteurized by a process that requires basic knowledge of chemistry.





CHEMICAL REACTIONS TUTORIAL QUESTIONS:
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 change has taken place.

4. All reactions have one thing in common: there is a breaking, bonding, or both of chemical bonds.

5. Chemical reactions always involve broken old bonds, forming of new bonds, or both.

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

7. In every reaction there can never be any more atoms or less atoms on one side than there are on the other.

8. Chemical reactions only balance 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 + O2H2O

If we use only the atoms shown, we’d have 4 atoms of H and 3 atoms of O as reactants. This would make 2 molecule of H2O, but we’d have 1 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:
___4_ H2 + ___2__ O2 ___=__ H2O Which is the same as: 2H2O


11. This idea is called the Law of Conservation of Mass
12. There must be the same coefficients and the same number of atoms before the reaction (in the reactants) and after the reaction (in the products).

Element	# of atoms in Reactants	# of atoms in Products
H	4	4
O	2	2

13. What is the balanced equation for this reaction?
__2__ Cu + ___1__ O2 =___2_ CuO

14. In the unbalanced equation there are:
Reactants Products
# Cu atoms __2___ = # Cu atoms ___2__
# O atoms ___2__= # O atoms ___2__


15. To balance this equation, we have to add __1____ 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 __Cu___ atoms is balanced but the number of _O___ atoms don’t match. Now we have to add more __O___ atoms to the reactants.

17. The balanced equation for this reaction is __2__ Cu + ___1__ O2 =__2__ CuO

This is the same thing as saying:
Reactants # Cu atoms __2___ = # O atoms ____2_ =
Products # Cu 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__ H2O + __1___ CO2


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

20. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) ___2__ KClO3 = ____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.) ___4__ Al + __3___ O2 =__2___ Al2O3

SUMMARY

1) Chemical reactions always involve the breaking of bonds, the forming of bonds, or both.

2)The Law of Conservation of Mass says that the same atoms must be the same before the chemical reaction and after the chemical reaction. They must also have the same mass.

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