joooselinn9688

27.06.2019 • 

Chemistry

Data trial 1 trial 2 mass of empty crucible with lid 26.688 26.681 mass of mg metal, crucible, and lid 26.994 26.985 mass of mgo, crucible, and lid 27.188 27.180 calculations: show your calculations for each of the following. remember, calculations should follow rules for significant figures. 1. write the balanced chemical equation for the reaction you are performing. 2. calculate the mass of magnesium metal used in each trial. o trial 1: o trial 2: 3. calculate the actual yield of magnesium oxide for each trial. o trial 1: o trial 2: 4. magnesium is the limiting reactant in this experiment. calculate the theoretical yield of mgo for each trial. o trial 1: o trial 2: 5. determine the percent yield of mgo for your experiment for each trial. o trial 1: o trial 2: 6. determine the average percent yield of mgo for the two trials. questions and conclusions: 1. describe the process that was used in this lab to create magnesium oxide, specifically identifying the type of chemical reaction. explain why the product had a higher mass than the reactant, and how this relates to conservation of matter. 2. what sources of error may have contributed to the percent yield not being 100 percent? think about things that may have led to inaccurate measurements or where mass of the product could have been lost if this experiment was conducted in a physical laboratory.

Ответ:

kaitlyn4576

09.06.2023

Chemistry

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  B. Solution

Explanation:  According to the question statement, Susan wrote in her notebook that it was a blue liquid. Therefore, from a chemistry point of view, it was a solution and not a heterogeneous mixture. Then, the solvent was evaporated after leaving the solution for 72 hours at the windowsill. The solute (blue color most likely) however was not able to evaporate with solvent and left behind.

Example: if you leave the KMnO4+water solution for a few days, water will evaporate thus leaving behind purple crystals of KMnO4.

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