Procedure: Fill a small test tube halfway with copper (II) sulfate solution. Add a 2. 0 gram iron rod to the solution and observe the reaction. Observations: When I put the Iron (Ill) and cooper (II) in the test tube I notice that the color change to a darker gray at the beginning. Regarding to the sulfate solution I also notice that its color change in to a clear blue. When they are mixt together the blue solution vanished slowly while its color change in toa reddish brown in the test tube. 2. Lead (II) nitrate and potassium iodide solutions pour about 2. L of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. Observations: the two solutions the lead (II) nitrate and potassium are transparent. But, when the two solutions are combine its color change to a yellow color. While the top of the test tube is like a light yellow but on the bottom of the test tube the yellow is darker. 3. Magnesium metal and hydrochloric acid solution Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid lowly and observe the reaction.
Next, place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas. Observations when its put the magnesium metal and the hydrochloric acid solution it look like many bubbles Observacion: cuando se pone el metal de magnesio ala solucion de acido clorhidrico se ve como muchas burbuJas en la surpeficie del tubo de ensayo como si fuera humo. Observation: when you put the metal wing magnesium hydrochloric acid solution looks like surpeficie many bubbles in the test tube as if it were smoke. 4. Electrolysis of water Use a U-tube with electrodes at each end, connected to a battery.
Fill the U-tube with water. Turning on the battery, observe the results at each electrode. Next, test for hydrogen and oxygen gas produced at each end of the tube. 5. Burning magnesium Place magnesium ribbon in a clean crucible (on a clay triangle above a Bunsen burner). Heat until the magnesium begins to burn. Complete a data table that includes a prediction of reaction type (single replacement, double replacement, synthesis, decomposition, or combustion), observations, and dentification of reaction type for each reaction in the lab.
Reactants Prediction of Reaction Type Observations Reaction Type Conclusion: 1 . Write a balanced equation for each reaction observed in this lab. 2. If you were to measure the mass of magnesium and hydrochloric acid before combining them in the test tube, how would that mass compare to the mass of reactants left in the test tube after the reaction? Explain your answer and how it corresponds to the law of conservation of mass. types of reactions. Which reaction is this, and what are the two types of reactions?