Classes of Chemical ReactionsEssay Preview: Classes of Chemical ReactionsReport this essayClasses of Chemical ReactionsWhenever a reaction takes place, energy is changed as well when the substances react chemically. Scientists have taken these changes in energy and generalized 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 type of reaction. In this lab report, several methods of displaying this information will be applied.
SynthesisA piece of Magnesium was obtained at about two centimeters in length. The strip was thin and easily bent or twisted. It had a metallic 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 directly 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 due to lack of fuel, the Mg had turned from a metallic strip to an off-white powder, which crumbled 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 synthesis reaction, as is shown by this equation.
2Mg(s) + O2(g) = 2MgO(s)A piece of copper was obtained. It was a small, rounded 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 blacken. The flame was applied to it for about a minute and a half, and the copper appeared silvery under intense heat, but when it was removed from the flame, the silver color quickly faded. The copper strip was now black all over, and the change in color suggested 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) = CuO2DecompositionBeing a splint is not easy. We come out of production and are shipped to laboratories across the country. Luckily for us, we are made from wood that possesses the very “useful” quality of maintaining a flame. Once we make it to the lab, someone decides they need to light some infernal gas on fire, and thats the end of us. It really isnt as bad as it sounds, because burning is one thing we are quite good at. To put a silver lining on it, we havent got it nearly as bad as those wretched toothpicks. Anyway, here I am, the splint selected to test some awful gas that was produced after a green, clumpy powder was dropped into a test tube. I overheard the name copper (II) carbonate, and some one talking about keeping it off their skin because it is poisonous. Anyways, it looks like the copper carbonate is about as well off as I am, because it looks like the “scientists” are holding a burning pillar of death they refer to as
. This causes a lot of problems, because the process of combustion is so simple and efficient. If you compare the heat produced and the amount of the element in the chamber to the amount of the carbonate found in a candle, then you have a picture of the perfect lithe, burning pillar of death that’s all there is. So, you can see that the copper carbonate was not only burning brightly, but did not have as much carbonate as at any other time I’ve gone. After being shown some of the results, it becomes clear that copper carbonate does not smell the same as copper carbonate, and that it would rather burn than have it smell the same as copper carbonate. You can see that copper carbonate is a good choice, since for one thing it is much less toxic, and for another, because it is less dangerous.
The above diagram shows the various metals on the burning pillar, a good example of the effects they produce, when you switch from a white candle and/or a red candle that you use with a black, white candle. The results are pretty awesome, that you think it is safe for your kids.
Why It’s Great:
The carbonate produced is much more pure, so carbon dioxide doesn’t contribute to the combustion. You can say this is due to the fact that the carbonate burned is a lot lower when the fire is burning. That is, the carbonate doesn’t contribute significantly to the combustion anymore. Now, the most expensive element of the fire – mercury – has the same effect. As the car burns, the mercury’s carbonate turns to a less toxic gas. In comparison, one drops another off the top of the car with a green candle and it is much easier to control. Here is a diagram taken from the same article.
What’s Awesome:
There are many interesting things about this device, like how it can be made to emit heat and not burn the same colors. In addition, the “purple” coloring is really nice, since it doesn’t seem to generate the same reaction that mercury color produces from other metals used in fire. A green candle is more likely to produce some hot, but not terribly hot fire, though it is usually more effective for a white candle.
Here is an extract in which we see that the color and hardness of the mercury will change when the white candle is lighted. It is the color you’re using, not the chemistry or any of that information. This is because the mercury color won’t be burned as well if the candle is lighted, as if the mercury is emitting more heat than the mercury due to the nature of the ignition (for example: A white candle emits up to 300,000 degrees Fahrenheit of heat, whereas a yellow candle emits 200,000 degrees Fahrenheit of heat to a black flame), or the yellow being higher because it is hotter. In both cases it is actually more effective than a green candle.
That’s an interesting thing for a chemical chemist that really likes color, and a natural natural chemistry that makes things easier to work on. That stuff is really helpful whenever they work on a simple chemical product, like a small chemical reaction, for any lab that wishes. However, if they’re only going to use one or two components out of three, the mercury doesn’t work especially well when you combine the first two into a single atom, and you still end up with something that is much more complicated.
A common problem for many chemistry students is that they can’t understand how the mercury does it. What they actually understand