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Cuco3 Reaction Lab Report

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Overall, the experiment was a success. Fewer mistakes were made and everything went smoothly. The first reaction was Magnesium ribbon in which we were able to examine it reacts when we put it under the flame. It is important to remember to use the tongs that are not prone to melt like the rubber pair I started to use. I quickly paused the experiment once I noticed the rubber tongs were gluing together. This minor mistake is avoidable and easy to fix. Our first conclusion was that magnesium burns to form new compounds. It reacts with oxygen to form oxides of each metal. This was an example of combustion and combination/synthesis reactions. Next, was the CuCO3 reaction, where we used a wood splint to discover that CO2 gas was present. After we …show more content…

It began to fizz instantly and the metal turnings began to dissolve. The bubbles continuously moved up and down while there was also a formation of a gas. We then placed a second test tube over the reaction test tube, and in order to see if it was Hydrogen gas that was present, we had to insert a burning wood splint into the tube and wait to hear the pop noise. This abrupt pop scared me and Julia so much we screamed and flew back. At least we discovered the presence of Hydrogen gas! This is an example of single replacement reaction. Next, is the AgNO3 reaction where we placed a small coil of copper wire into the solution. In approximately 8 minutes we got our reaction. The copper is covered with what looks like white crystals and the AgNO3 solution turned clear light blue. This is an example of single replacement reaction. Here comes another reaction, and this time it involves copper (II) sulfate solution and sodium hydroxide solution. When the two aqueous solutions mixed with each other, a pale blue precipitate of basic copper hydroxide and a solution of sodium sulfate is formed. Lastly, is the reaction between sodium carbonate and

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Once the material was acquired, 1.0094 grams of Aluminum were weighed and then transferred to a 250mL beaker. The 250mL beaker continued to remain in use for the next few steps. 1.4M KOH solution was added to the Aluminum sample that was previously obtained. For gas to escape the lab, there was a fume

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When we placed the aluminum foil in copper chloride, a chemical reaction occurred. Before the reaction took place we had aluminum foil and copper chloride as our reactants. After the reaction happened, the products were aluminum chloride and copper. After the foil was placed in the copper chloride, the color of the aluminum foil had changed from a shiny silver, to a deep red. Also, the color of the copper chloride changed from a light blue to a murky green.

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Introduction In the late 1700’s, Jeremias Benjamin Richter defined stoichiometry as the "art of chemical measurements, which has to deal with the laws according to which substances unite to form chemical compounds." In this exercise, we combined copper(II) sulfate pentahydrate with two moles of sodium hydroxide which produced copper(II) hydroxide and sodium sulfate (CuSO4 + 5H2O +2NaOH  Cu(OH)2 + Na2SO4). We then dissociated copper(II) hydroxide to produce copper(II) oxide and water (Cu(OH)2  CuO + H2O). The objective of this exercise is to perform a simple chemical reaction where the concept of stoichiometry is put into practice (2).

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The products were aluminum chloride and copper. A change in properties demonstrates that a chemical reaction occurred. One property that changed was the colors. Initially the aluminum foil was a shiny silver, and the copper chloride was a green-blue liquid. After we placed the aluminum into the copper chloride solution, the liquid clouded up a lot and turned to a light grayish hue.

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Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and

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As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear.

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The bag expands and there are visible bubbles forming. Next the reaction releases carbon dioxide and creates-a small amount of- water. These are new substances because the original substances involved were baking soda and vinegar. Finally the temperature change is noted with a thermometer after the

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Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of

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Tiny black-brown particles that looked like dirt eventually appeared throughout the course of the reaction. Once the liquid surrounding the particles became clear, the beaker was removed from the hotplate and the particles settled at the bottom of the beaker where the water was decanted. The particles looked airy and light. The Cu(OH)2 reacted because the of the heat added to the solution which caused the solution to be broken down. Therefore, this was caused by a decomposition reaction.

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Double Displacement: If the reaction that occurs is double displacement then an increase in reactants will reesult in creating two or more compounds/reactants. Experimental Design Part A: A large well plate was placed on the lab station, each well was filled with either copper (II) nitrate, magnesium nitrate, or zinc nitrate. Added to each of the wells was three strips of copper wire, magnesium ribbon, and zinc metal (powder form). Using a toothpick, you submerged the metals in the liquid and ensured they did not touch.

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But the difference was no bigger than 0.08, and after the values were rounded the same empirical formula was deduced. So the experiment can be concluded as successful. Evaluation: The method used was simple and easy to follow; however, it did not include how much oxygen was needed to react completely. Also it didn 't mention what magnesium oxide looked like after it finished reacting, so it was a guesswork of determining whether the reaction was finished or not.

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It is hypothesised that the total mass of the three compounds will be the same number as if you were to add them up. The conservation of mass states that no mass is lost when two substances are combined, none is created either. The only thing that may happen is that these chemicals will be rearranged. No mass will be lost at all, so in the practical one adds 50 mL of Sodium Hydroxide and 50 mL of Copper Sulfate, these two combined will give a total of 100 mL, since no mass will be created or lost. The chemicals may react but no mass will be lost due to the conservation of mass.

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In this lab, the hypothesis, if a chemical reaction occurs, there will be signs of a chemical change such as a change in temperature, color, and/or smell, was accepted. In each experiment, clear signs of a chemical reaction were observed. In chemical reaction #1, we put drops of vinegar onto a small pile of baking soda. The baking soda and vinegar produced bubbles of gas right as the first drop hit the baking soda, which is a clear sign that there was a chemical change occurring. This can be classified as a double replacement chemical reaction.

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