Observing Chemical Reactions

For reaction a2sodium sulfite when combined with a

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For reaction A2—Sodium sulfite when combined with a strong acid such as HCl produces a toxic gas therefor, as green chemistry principle #1 states reaction A1 would prevent toxic waste and generates a safer chemical as listed in principle #4. Also since sodium sulfite poses a moderate health risk, principle #3 can be applied.
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For reaction B1—Sodium oxalate is toxic to humans therefore principle #3 is applicable because B2 produces safer chemical products. For reaction C2—magnesium metal is highly flammable and would be difficult to extinguish thus principle 12 is applied here and it is safer to preform reaction C1 for there is no way it could emit UV light For reaction D2—Copper (II) carbonate is an unsafe chemical thus principle #3 is applied. Also this experiment requires fire where D1 does not so less energy is used in D1, thus principle #6 is applied. In D2 none of the chemicals could be used again where in D1 a potato is used as a catalyst, which enacts principles #7 and #9. E2 For reaction E2—Sodium hydroxide is extremely corrosive and with strong acids released heat. The release of heat is toxic to the environment thus principle #12 is a reason for doing reaction E1 instead. Also since it is a harmful compound it is better to prevent the rapid reaction so principle #1 can be applied as well as principle #3. For reaction F1—Calcium oxide vigorously reacts with water and causes irritation when inhaled. So here we can say principles #3 and #12 apply for reasons for not conducting the reaction. Because we were not required to accurately measure out substances, we just measured based off of approximation, if we measured too much of a reactant, or not enough the reaction might not work. This is determinate error could be adjusted with a better approximation or measurement technique. Since we were not accurately measuring any of the substances there were no indeterminate errors. After learning the structure for categorizing reactions it was fairly simple to write the molecular equations and determine what products were formed. Seeing the experiments also helped to determine the states of each of the compounds so that I could accurately write the net ionic equation and determine that a reaction actually took place. This qualitative analysis is important in the world of chemistry because if chemist’s conducted experiments without knowing what products they were forming then they could conduct a potentially hazardous experiment.
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