Copper Cycle Lab Report

The goal of the experiment is to synthesize a bromohexane compound from 1-hexene and HBr(aq) under reflux conditions and use the silver nitrate and sodium iodide tests to determine if the product is a primary or secondary hydrocarbon. The heterogeneous reaction mixture contains 1-hexene, 48% HBr(aq), and tetrabutylammonium bromide and was heated to under reflux conditions. Heating under reflux means that the reaction mixture is heated at its boiling point so that the reaction can proceed at a faster rate. The attached reflux condenser allows volatile substances to return to the reaction flask so that no material is lost. Since alkenes are immiscible with concentrated HBr, tetrabutylammonium bromide is used as a phase-transfer catalyst.

If I had a household product labeled sodium bicarbonate, I would add an acidic substance and expect bubble to be created. As we know acid reacts with bubbles when combined with sodium bicarbonate. 2. Write the chemical equation for the reaction in well A6. B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript3 Words NaOh + AgNO3>>>>NaNO3 + AgOH 3.

Copper is an element and a mineral important to our everyday lives. Because copper is stable, it can be used in jewelry, coins, wiring, and statues. It’s one of the well-known metals due to its reddish brown metallic color. Because copper has high ductility, malleability, thermal and electrical conductivity, and resistance to corrosion, it is a major industrial metal. Copper is one of the oldest metals, dating back more than 10,000 years ago.

The reactions that form the basis for the iodine clock reaction are shown below. Equation 1: H2O2 + 3 I- + 2 H+ → I3- + 2 H2O • H2O2 = Hydrogen peroxide • I- = Iodide ion (from potassium iodide) • H+

Purpose: To recognize the evidence of a chemical change and to prove the law of conservation of mass by observing a series of chemical reactions involving copper. A specific quantity of copper will be transformed through a series of chemical reactions to form new substances and then recovered as solid copper. A percent yield will be calculated to determine the amount of copper recovered from the chemical reactions.

For an example (the reaction of tert-butyl chloride with water.) The SN2

First,the aspirin dissolves in water. Second, sodium and citrate ions combine to form sodium citrate which is soluble in the water. Third and finally, the bicarbonate ions from sodium bicarbonate react with hydrogen ions from citric acid to produce water and carbon dioxide gas which is released in bubbles. The result is a fizzy, or effervescent, solution. Bubbles are produced continuously from the time the tablet enters the water until the time when the reaction between sodium bicarbonate and citric acid ceases.

Aluminum (s) + Sulfuric acid (aq) > Hydrogen (g) + Aluminum sulfate (aq) 2 Al (s) + 3 H2SO4 (aq) > 3 H2 (g) + Al2(SO4)3 (aq) This reaction undergoes physical and chemical changes, there is a chemical change as there are new products formed and a physical change as there are changes in state. 3.

But first, the ore has to react with a weak acid, for example dilute sulphuric acid to make a thin copper (II) sulphate solution. Then, the copper ions are removed from the solution by adding sulphuric acid to the reaction. This produces a more concentrated copper (II) sulphate solution. Then the copper is purified further using electrolysis. An impure copper rod serving as a anode and pure copper serving as a cathode are placed in an electrolytic cell.

persulfate variation. This is the third of the four main forms of the iodine clock reactions where iodide ions is reacted with persulfate in 2 main reactions. The total reaction is the reaction of sodium and iodide ions, as well as sodium thiosulfate, which is then reacted with the starch to form the bluish color. As seen in figure 6, the first reaction consists of peroxydisulfate (), and iodide ions which form iodine and sulfate (SO42-).

The reaction between Hydrochloric Acid and Sodium Carbonate led to the formation of gaseous Carbon Dioxide, aqueous water, and aqueous solution of Sodium Chloride as a result of all compounds containing alkali metals solubility. Lastly, Copper Sulfate and Sodium Carbonate reaction produced an aqueous sodium sulfate solution and a solid precipitate of Copper (II) Sulfite because of all alkali metals and sulfates ability to be soluble and the rule that any compound containing CO₃ is insoluble. In the end, the hypothesis that if we react mystery chemicals with one another, we will be able to identify the reactants and products, create balanced equations, and observe properties because of our prior knowledge learned throughout the course of the unit and using the known chemical reaction was accepted by the data

A double-replacement reaction also involves the transfer of anions. However, unlike a single-replacement reaction, a double-replacement reaction has two anions being intrechanged. An example of this type of reaction would be the combination of hydrochloric acid and sodium hydroxide to form water and sodium chloride: HCl + NaOH --> H2O +

Hydrophobic & Hydrophilic Molecules 1. Hydrocarbons made up of solely of hydrogen and carbon atoms 2. Hydrophilic is water loving and are compounds that will interact with water 3. Hydrophobic is water fearing and compounds that do not interact with water 2.7 Acids and Bases 1. Acid is any substance that yields hydrogen ions when put in water solutions 2.

ZnS(s) +2NaCl(aq). The ionic and net ionic equations are: Ionic: 2Na(aq) + S2(aq) + Zn2(aq) + 2Cl(aq) ZnS(s) +2Na(aq) + 2Cl(aq), and net ionic: Zn2(aq) + S2 (aq)+ ZnS(s). Chemical reaction occurred from the ammonium dichromate(Decomposition) was exothermic reactions. In a double displacement reaction two compounds exchange bonds or ions in order to form different compounds. An example of a double displacement reaction occurred between zinc chloride and sodium sulfide to form zinc sulfide and sodium chloride.

For example, if lead (II) nitrate (Pb(NO3)2) were to react with potassium iodide (KI2), the products would each have the metal from their original reactant bonded with the