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Submitted By Zach-Kieszkowski
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Conservation of Matter Lab
Background and Purpose:
“Antoine Lavoisier’s discovery of the Law of Conservation of Mass led to many new findings in the 19th century” (Conservation of Mass). The Law of the Conservation of Mass/Matter states that the mass of the system must remain constant over time. This is most clearly shown through chemical reactions and changes. “When large energy transfers between systems are involved, the difference between thermodynamically closed and isolated systems becomes important, since conservation of mass is strictly and perfectly upheld only for so-called isolated systems, i.e. those completely isolated from all exchanges with the environment.” (Conservation of Mass).
Matter cannot be destroyed or created by a chemical change. (Mess)
This very important principle is known as the Law of the Conservation of Matter. This law applies to ordinary chemical reactions unless it’s a nuclear reaction where matter may be changed to energy. During a chemical change, the atoms of one or more substances go under some rearrangements. The result of these rearrangements is the formation of new different substances. (Davis)
Works Cited
Conservation of Mass. Wikipedia, October 1, 2013.
Mess, B.A. “Law of Conservation of Matter.” Honors Chemistry. BHS, Lake Geneva, WI. 25 Oct. 2013. Notes.
Davis, Raymond E., et al. Modern Chemistry. Austin, TX: Holt, Rhinehart, and Winston, 2002. Print.

Safety glasses
Test tubes
Graduated cylinders
Marking pen
Solutions of: Na2CO3
Using a graduated cylinder, measure exactly 10.0ml of sodium carbonate (Na2CO3) solution and pour it into a test tube. Stopper the test tube and mark it. Make sure to rinse and dry the cylinder. Then measure 3.0ml of calcium chloride (CaCl2) solution and pour into a clean, dry test tube. Then stopper and label the test tube. Rinse this cylinder also.
Repeat step 2 with 3.0ml of sulfuric acid (H2S04) solution. CAUTION: Handle this substance with care.
Put all the test tubes in the beaker and measure them on the balance.
Remove the test tubes containing the CaCl2 solution and the Na2CO3 solution. Pour the CaCl2 solution into the Na2CO3 solution (be careful not to spill. Mix and record observations. Then measure all tubes in the