: The chemical formula of a compound will be determined using the mass of each individual element that is present in a weighed sample of that compound. The chemical formula shows the proportions of elements in a specific compound. This proportion is uniform to all samples of the same compound. Using the mass of each element, the moles of the element in the compound can be found and then compared to that of the other elements. This will create our atom ratio which will lead to our mole ratio. The mole ratio is discovered in chemical analysis and from this, the chemical formula of the compound.
Procedure: From the laboratory textbook Chemical Principles by Slowinski, Wolsey, and Rossi (p. 23-28, chapter 4), our experiment began. First, a crucible without its cover was weighed. About one gram of the unknown hydrated copper chloride was added to the crucible, broken up, then accurately weighed and recorded. …show more content…
The unknown hydrated copper chloride was burned enough so that the sample’s green crystals turn to their anhydrous brown form. After the color change, the sample was heated for an additional two minutes. Precaution was taken so as not to overheat the sample. The crucible was then covered and allowed to cool for fifteen minutes. The anhydrous sample in the uncovered crucible was weighed and recorded. Third, an empty 100mL beaker was weighed and recorded. The brown crystals were transferred to the beaker. About 5-7mL of distilled water was added to the crucible, swirled, and then poured on the brown crystals in the beaker. The beaker was swirled to dissolve the crystals. The green color was restored. Next, two aluminum wire pieces about an inch long were obtained and weighed. The aluminum wire was then fully immersed in the solution. The color of the solution faded, and within 30 minutes, the solution was completely
Procedure: From the laboratory textbook Chemical Principles by Slowinski, Wolsey, and Rossi (p. 23-28, chapter 4), our experiment began. First, a crucible without its cover was weighed. About one gram of the unknown hydrated copper chloride was added to the crucible, broken up, then accurately weighed and recorded. …show more content…
The unknown hydrated copper chloride was burned enough so that the sample’s green crystals turn to their anhydrous brown form. After the color change, the sample was heated for an additional two minutes. Precaution was taken so as not to overheat the sample. The crucible was then covered and allowed to cool for fifteen minutes. The anhydrous sample in the uncovered crucible was weighed and recorded. Third, an empty 100mL beaker was weighed and recorded. The brown crystals were transferred to the beaker. About 5-7mL of distilled water was added to the crucible, swirled, and then poured on the brown crystals in the beaker. The beaker was swirled to dissolve the crystals. The green color was restored. Next, two aluminum wire pieces about an inch long were obtained and weighed. The aluminum wire was then fully immersed in the solution. The color of the solution faded, and within 30 minutes, the solution was completely