Our research goal was to determine the enthalpy of magnesium and hydrochloric acid mixed together.

We achieved this goal by measuring out 50ml of hydrochloric acid in a cholorimeter, then adding 1.6g of magnesium ribbon to the hydrochhloric acid. We determined that the hydrochloric acid absorbed 3kj, after doing multiple calculations to help support it. Overall, the hydrochloric acid absorbed quite a bit of energy from the magnesium.

Hydrochloric acid is an acid, therefore CAN harm people in high enough quantities. Along with the hydrogen gas being given off could cause harm if inhailed.

Materials

• 100ml graduated cylinder
• 50ml of hydrochloric acid
• 1.6g of magnesium strip
• chloromiter
• Sparks machine /w temp prob
• scale

1. Collect all equipment and put on your safety glasses.
2. Measure out 50.0mL of 1.0M HCl and pour into a pre-weighed calorimeter.
3. Record the mass of the calorimeter + HCl.
4. Record the starting temperature of the HCl.
5. Measure out no more than 0.2g of magnesium ribbon. Record the actual mass.
6. Roll up the Mg ribbon into a loose ball. When ready, place the Mg into the HCl. Quickly place BOTH lids on the calorimeter and slide the thermometer probe into the reaction mixture.
7. Record the temperature every 15 seconds, until the reaction is complete (you'll be able to hear the gas being given off when it's reacting).
8. When the reaction is complete, record the final temperature.
9. Rinse off the thermometer probe and pour the reaction mixture into the waste container, with an equal volume of tap water to "neutralize" any remaining acid.
10. Clean off your lab table and return to your seat

Evidence

•  50ml of hydrochloric acid
• 1.6g of magnesium ribbon
• 29.48g choloromiter
• Hydrochloric acid is 24.3C
• Initial temp of acid /w Mg = 25.2
• Final temp = 39.4
• Hydrochloric acid absorbed 3kj
• Enthalpy of Mg was 455.71875
• The theoretical heat of reaction was 466.75kj
• Our percent error is 2.36%

The enthalpy of the Mg and HCL was 466.75kj.

What I learned from this expierment was that you can find the enthalpy of reactions by finding out the mass, change in temperature, and specific heat of the inital, and final substances of the reactants. Thus, we were able to deduce the enthalpy by using various formulas Including, finding the moles of a substance, finding the heat absorbed by a substance, and finding the enthalpy. This type of expierment can be used for a lot of reactions, and therefore able to be used on various substances, enabling us to find the enthalpy easily.

The feeedback I recieved was mostly negative, with a very small amount of positive. However, the negative comments were not too harsh. It was mostly about being more descriptive, backing up my evidence, and a few grammatical mistakes. That is really what was in the feedback.

A few of the changes I am going to make is adding a well done title page, a better description of my comments, and having a much better cite page. Along with having more descriptive cites, and rewording and rephrasing some of the actual paragraphs. Those five are the major ones I am going to focus on.

The only question I really have left is what would be a good source or a few of them? I could not really find much about silly putty, and just had to go with what I could get. That, and what would be a better set-up for my paper? I can not really think of any more questions I have about my essay.

Question:

Our investigation was that of the amount of red absorbance in different concentrations of a stock fluid.

Abstract:

This experiment was conducted for the purpose of trying to prove Beer's law through coloration. How my group and I did this, was making a stock concaction and diluting it to test the different amounts of reb absorbance. What we found, was that the higher concentration of the final stock, the red absorbance increased.

Safety considerations:

1. Liquid in eyes
2. Glass, possible breaking
3. Solution on hands

Materials:

1. CuSO4
2. Distilled water
3. SPARKS machine
4. Test tubes
5. Pippets
6. Flask
7. Cork

Procedure:

1. Find the amount of grams needed to reach a .5M concentration per 25mL
2. Put 3.121 (per 25mL) grams of CuSO4 into the flask
3. Fill to the white line with distilled water
4. Put the cork on, and shake thourghly
5. Fill each test tube with 0mL to 5mL of stock, increasing by 1mL each time
6. Fill each test tube with distilled water 5mL to 0mL, decreasing by one and corresponding with the stock to always have a final volume of 5mL.
7. Measure each tube for its' red absorbance using the SPARK machine.

Evidence: Normal 0 false false false EN-US X-NONE X-NONE MicrosoftInternetExplorer4

Claim:

We have proved Beer's law, as the concentration went up, so did the red absorbance. Therefore, they have a direct correlation

Scinetific Explanation:

Therefore, the correlation of the concentration of the dilluted liquid and red absorbance is apparent. As, the more stock that was in the final mixture, the more red light it absorbed.

The Standard Model is very important to scientists because it helps classify the sub atomic particles by their use or where they are located. Which, really helps to speed things up when you're talking about a large sum of them

The force ones are grouped together because they each have to do with some kind of force, and are classified because they help regulate the force. Just as all the Quarks are found within Protons and Neutrons, and make up those two particles. Not to mention they decay into each other and are used for the same things. As for Leptons, they all are like Electrons. They are small, and carry a negative charge. 

The model could have rows and collums added as we go smaller and smaller, and more indepth into what we currently have. Otherwise, we can't add much more until we find the base partical for everything.

The Desnity test