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    Copper to Silver to Gold—A Comparison of Physical and Chemical Changes (Adapted from Abra-Ka-Dabra by C. M. Bires.) Introduction Hundreds of years ago‚ noblemen and women would pay large sums of money to alchemists. These early chemists were similar to modern-day illusionists in that they used a little science‚ a few tricks‚ and some acting to convince their clients that they had the ability to transform base metals into pure gold. Although these alchemists were eventually revealed as charlatans

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    In order to find the formula of the copper chloride hydrate‚ we had to separate the compound to find the mass of water and copper. To begin this process‚ we evaporated the water and created an anhydrous compound‚ meaning we were left with only CuxCly. By calculating the weight of both the anhydrous and the hydrated compounds‚ we could conclude that the difference in the weights was the weight of the H2O. From this we were able to calculate the percent composition of CuxCly and H2O (see Calculations:

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    Temperature and Cofactors on Enzymatic Reactions “I pledge that no unauthorized assistance has been given or received in the completion of this work. Experiments described were performed by me and/or my lab group and this write-up is entirely my own creative work.” X________________________________________ Introduction Enzymes are protein molecules that speed up the rate of reactions by reducing the activation energy of a reaction. They act as catalysts in reactions‚ increasing the rate at which

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    From this lab we can learn to observe physical properties of varying substances as well as to use chemical reactions to observe chemical observe the chemical properties of varying substances. In experiment #1‚ we were able to detect physical properties of the aluminum and copper sulfate simply by looking at the substances. We then combined the two substances to see if they would create a chemical reaction and test the chemical properties. After being combined‚ bubbles and gas were created and the

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    aluminum powder and a metal oxide [usually iron oxide (Fe2O3‚ known as rust)]. The thermite reaction is a redox reaction‚ where Aluminum reduces the oxide of another metal. For example‚ when using iron oxide (as I did) the equation would be Fe2O3(s) + 2 Al(s) -> Al2O3(s) + 2 Fe(l). Black or blue iron oxide (Fe3O4) could also be used. Other examples of possible oxides are manganese thermite (MnO2)‚ Cr2O3‚ and copper thermite (CuO). Aluminum can also be replaced by any reactive metal. Aluminum‚ however

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    Writing Practical Reports Aim: To observe what happens during and after a chemical reaction. Equipment: • Concentrated nitric acid in a glass dropping bottle • Small pieces of Copper • 250ml Beaker • 2 M Lead nitrate in a dropping bottle • 2 M Potassium iodide in a dropping bottle • 2 M Copper sulfate in a dropping bottle • 2 M Sodium hydroxide in a dropping bottle • 2 M Hydrochloric acid in a dropping bottle • 4 Pyrex test tubes • Test tube rack • Spatula • Bunsen burner‚ gauze

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    Oxidation and Reduction Reactions: The Reactions of Copper Data: Part I: Preparing a solution of copper (II) nitrate Initial mass of copper wire: .520g Mass of copper wire after vigorously scouring: .518g Observations of Copper (II) ribbon mixed with HNO3: Solution turned green. Thick brown gas formed. Copper (II) bubbled vigorously. Cu (II) dissolved‚ solution appeared green/blue. After the addition of H2O a blue crusty precipitate formed. Part II: Synthesis of solid copper (II) hydroxide

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    Redox Reaction Lab Report

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    Purpose Determine which kinds of reactions involve electron transfer as the driving force. Background Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed. So‚ when a metal and a nonmetal react‚ there is an ionic bond formed‚ which means one of them loses electrons while the other gains them. Since this reaction involves the exchange of electrons it is termed as a redox reaction. The oxidation states in a metal- nonmetal are simple

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    EXPERIMENT # 14: Exothermic and endothermic reactions Date: 25/06/2012 Name: Meagen Reyes Year 11 PARTS A‚ B and C * For the procedures and equipment needed in these experiments‚ refer to page 73-74 in the STAWA Exploring chemistry stage 2 book Part A: solution process (dissociation) Solutions and their chemical equations | Initial temperature (in Celsius) | Final temperature (in Celsius) | Classification(exothermic or endothermic) | Sodium hydroxide NaOH(s) Na+(aq) + OH-(aq) + Energy

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    H2 Reaction Lab Report

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    which complexes with the sulfide radical to create an H2S2•- species.2 This type of reaction can continue to create polysulfide chains.2 Lastly‚ type III reactions

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