Chemical Change Lab Report

The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as

When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.

Copper wire turned white when submerged in distilled water, little crystal-like substances forming on copper

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

|1. Copper metal (penny) at the start |Tarnished, worn out, brownish, copper-colored, fine solid. |

The experiment was performed to show the many chemical reactions and states of copper, a very common yet important element that can is found in many useful compounds throughout the world. Copper was combined with many different compounds and elements to cause chemical changes in the state of copper. These reactions were conducted to display the several different states of copper throughout the cycle, ultimately restoring the copper after the metal seemingly disappeared.

A physical change includes a change in the material without affecting its composition, such as the physical state change. However, a chemical change includes the change in the composition of the substance. The change in color, formation of a gas or a solid product, and the production of energy are the evidences of a chemical reaction, thus, of a chemical change.

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

In this experiment you will observe some physical and some chemical changes. You will observe that energy must be used to start some chemical reactions, and that it is produced in others.

Purpose/Introduction: The objective of this lab was to recognize and differentiate between physical and chemical changes in matter. Physical change can be defined as a usually reversible change from one state (solid, liquid, or gas) to another without a change in chemical composition. The physical properties of a substance--such as size, shape, density, or state--are altered. An example of a physical change is ripping paper.

The main goal of this experiment was to observe series of reactions that convert a piece of copper metal, via several different copper-containing compounds, back into its original elemental form. The data collected was the striking color changes along with their relevant chemical equations. The data was collected while keeping a close eye on the experiment the whole time. The data recorded was used to see the different changes involved with a piece of copper metal. The copper was weighed and heated multiple times throughout the experiment

When the Acetic acid and Sodium Bicarbonate mixed together, it was clear that a chemical change took place because gas was produced. The chemical reaction occurred in two steps. First, a double displacement reaction occurred in which the Acetic acid reacted with Sodium Bicarbonate to form Sodium Acetate and Carbonic acid. Since the Carbonic acid was unstable and underwent a decomposition reaction, it produced water and Carbon Dioxide instead. The mass of the products in the chemical reaction was the same compared to the mass of the reactants.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

The purpose of this lab is to test substances and to determine the physical and chemical properties of substances.

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the