StableinK

Our 8.0 KNO3 solution has begun to solidify once again.

Our KNO3 has dissolved we are stirring and waiting for it to become crystal again, we will record at what temp it happens.

To dissolve our solid KNO3 we have submerged our test tube in the 90 degree water bath,we have stirred to KNO3 and we are waiting for it to dissolve.

In this picture we are taking the temp.of our water we want it to be at 90 degrees c. Once we reach 90 degrees we will lower test tubes with the solid KNO3 into the water bath to allow it to dissolve.

Here we have added 2.0,4.0, 6.0, and 8.0 grams of KNO3 to our test tubes

Here we labeled the 4 test tubes and added the 5 mL of water to it.



In this picture we began to add Fe into our solutions, the iron rusted when it was placed in CuSo4. Then we added Zinc, which reacted by dissolving solution in Pb(No3)2, CuSo4 and AgNo3. We also found that Cu reacted with AgNo3 and was coated with a solution, and Al did not react with any of the solutions. As a result we found Zinc was the strongest, then Pb, then Cu, then Ag, and finally Fe.

We have added copper wire to each solution, the copper reacted with the AgNo3, forming a layer or silver fuzz around it, but we see no other reactions.

For this lab we are adding Copper, Zinc, Aluminum, and iron to our liquid solutions. Based on each reaction that occurs we want to be able to see which metals are the strongest. we will do this by watching the reactions to see which metals replaced others.

\ These are some of the solutions we used for the reactions in each solution we will add different metals.

\ Chase has begun to set up the lab with Pb(NO3)2, FeCl2, CuSo4, and AgNo3, this is before any reactions, no metals have been added.

mendeleev: Predicting the Future? Purpose: Predict the density of the element Germanium by determining the density of the other metals found in the same column of the periodic table. Data:

Conclude: by taking the average density and the period the element occupied we can find the denisty of Germanium.

Lavoisier a Liar? Purpose: The purpose of this lab is to find out whether or not Lavoisier was correct in his statement that matter is the same before a reaction as it is after a reaction. Data:
 * Reactants || Mass (grams) ||
 * Mass of empty beaker A || 66.5 ||
 * Mass of compound placed in beaker A || .7509 ||
 * Mass of empty beaker B || 67.7 ||
 * Mass of compound in beaker B || 1.2040 ||
 * Total mass of compounds placed in beaker A&B || 1.9549 ||
 * Mass of clean filter paper || .9 ||


 * Products || Mass (grams) ||
 * Mass of beaker A & filter with compound || 86.46 ||
 * Mass of compound recovered in beaker A || 1.1 ||
 * Mass of beaker B+ compound || 98.16 ||
 * Mass of recovered compound in beaker B || 2 ||
 * Total mass of both A&B compounds || 3.1 ||

When we measured the mass of our first empty beaker we got 66.5 grams we reset the scale to 0 then we carefully put in our compound and got .7509 grams. After that we set the scale back to 0 and measured beaker B's mass and that was 67.7 grams we zeroed it again and measured the mass of the compound added to beaker B and got 1.2040. We then added those masses together from both beaker A&B and its sum was 1.9549 grams. Finally we zeroed it and measured the clean filter paper its mass was .9 grams. Those were all of our reactants measurements. Then we measured our products in grams. First we measured the mass of Beaker A and its filter with the compound and its sum was 86.46 grams. Then we measured the mass of beaker B and the compound which resulted in 98.16 grams. The mass we of the compound we recovered in beaker A was 1.1 grams and the mass of compounds recovered from beaker B was 2.0 grams. Once we got all of the masses all we had to do was compare them. We did this by subtracting the total mass before the reaction from the total mass after the reaction. Some experimental errors may have been our starting measurements of empty beakers and or bad rounding. We had to compare the compounds mass from before the reaction in both beakers to the beakers after the reactions occurred taking into account the filter paper. We had to do careful math adding all totals up to make sure we were accurate. But we must have been off because our compounds before the reaction were a much different mass than it was after the reaction. The class average was 2.7 grams and our percent error was 61.63.
 * Total mass of compounds before the reaction || 1.95g ||
 * Total mass of compounds after the reaction || 3.1g ||

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