Classes of Chemical Reactions :: essays research papers

Classes of Chemical ReactionsWhenever a reaction takes place, vitality is varyd as well when the substances react chemically. Scientists have taken these changes in energy and infer them. Scientists can take these generalizations and discover more about the nature and tendencies of matter. In this lab, the purpose was to perform seven reactions, write down their equations, and identify the lawsuit of reaction. In this lab report, several methods of displaying this information will be applied. discount1.A piece of Magnesium was obtained at about two centimeters in length. The divest was thin and easily bent or twisted. It had a gilded surface and was brittle. It was silver in color. A flame from a bunsen burner was held to the Mg, and it ignited, giving off a brilliant white light. Looking like a shot into the light resulted in temporary blindness, which would explain the warning on the procedures that strongly suggested not looking directly into the light. After the flame had extinguished itself repayable to lack of fuel, the Mg had turned from a metallic strip to an achromatic powder, which go badd at the slightest irritation. The magnesium had bonded with the oxygen gas in the air from the energy that was applied to it and formed magnesium oxide. The type of reaction was a implication reaction, as is shown by this equation.2Mg(s) + O2(g) = 2MgO(s) 2.A piece of copper was obtained. It was a small, go wire that could be bent, although with a greater difficulty than the Mg strip from the previous account. It was copper in color (never saw that one coming, didja) and had a metallic luster. The copper was put in the flame of a bunsen burner and after several seconds, it began to unappeasableen. The flame was applied to it for about a sharp and a half, and the copper appeared silvery under intense heat, but when it was withdraw from the flame, the silver color quickly faded. The copper strip was now dimmed all over, and the change in color sugg ested that a chemical change had occurred. The Cu had reacted with the oxygen in the air and formed copper oxide. The black color could be scraped off, but only in small slivers. It would crumble when it was irritated with a great deal of pressure, respectively. It was a synthesis reaction as displayed by the equation here.Cu(s) + O2(o) = CuO2