Ammonium Chloride And Sodium Hydrochloric Acid

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

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

During the heating period, a noticeable change took place in the sugar test tube – it began to caramelize, melting into a golden brown color, then finally a dark brownish/black hue; it remained constant at that color. The copper sulfate began losing color when applied to the heat, turning from a bright blue to white and remained white after heating. Once cooled, 2-3 drops of water were added to each tube; the sugar remained the same, while the copper sulfate immediately bubbled and transformed from white back to its original blue hue. Next 1-3 grams of the hydrated copper sulfate were added to a crucible, which was weighed prior to adding the sample, then heated gently with a Bunsen burner. Once the salt stopped changing color, it was heated for an additional 5 minutes, then the total mass was measured. Finally, a pea-sized amount of Epsom Salt was added to a test tube and heated for 1 minute without the tube becoming red

Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper.

In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

The main objective of this experiment is to differentiate between a physical change and a chemical change.

Steel wool was used since it is virtually pure iron. In this reaction single displacement had occurred.

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows:

In the third chemical reaction copper hydroxide reacted was heated resulting in this equation: Cu(OH)₂(s) → CuO(s) +

The Rorschach test is a projective psychological test created in 1921 by Hermann Rorschach. The test consists of ten symmetrical inkblots printed on cards which are divided into five black and white and five in color. The Rorschach test is used to inspect the emotional functioning and personality characteristics of the person taking it. It is often employed in diagnosing underlying thought disorders. Also in differentiating psychotic from non-psychotic thinking in cases where the patient is averse to openly admit to psychotic thinking."

To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution.

As the temperature of water increases, the particles of solid Potassium chloride, KCl, which are absorbing energy from its surrounding, start moving more easily between the solution and its solid state because. According to the second law of thermodynamics, the particles will shift to the more disordered, more highly dispersed solution state. I predict that as the temperature of a KCl and water mixture increases, then the solubility of the KCl will also increase.

This experiment was performed to determine the heat of neutralization between Hydrogen chloride (HCl) and Sodium hydroxide (NaOH). A temperature probe was used to measure the temperature of the reaction when the base (NaOH) was poured into the acid (HCl). The data was collected on logged on LoggerPro.