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CHM2045Lab1 - An Analysis Of Production Methods And Costs...

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An Analysis Of Production Methods And Costs Of The Synthesis Zinc Iodide Frank Selb – Lab #3 Introduction. In the synthesis of zinc iodide lab, the objective was to analyze the costs of producing zinc iodide based on the percent yield generated from using a multi-step production method. The lab tested the experimenter’s ability to make an acid dilution which would catalyze the reaction between zinc and iodide, decompose a solution of zinc iodide by electrolysis, and determine and calculate the limiting reactant in the reaction and percent yield of product. The experimenter was then able to see the effects a limiting reactant has on the reaction. From the percent yield, the experimenter would be able to determine the effectiveness of this zinc iodide production method and examine where possible loss of zinc iodide (or miss-measurement) occurred within the experiment. This then aided the experimenter in determining alternative methods that would be more time or cost effective thus producing a greater percent yield. Experimental Procedure. A dilute solution of acetic acid was first created to drive the reaction of zinc and iodide, in which the experimenter calculated using the amount of milliliters needed to make 1.000 M acetic acid diluted to 10.00 milliliters of 0.200 M acetic acid solution, which was then determined to be 2.00 ml. The next step involved the experimenter to perform a series of mass measurements which were used to accurately determine the amount of zinc iodide that formed during the reaction. The weight of test tube #2 with three boiling chip was weighed at 22.060 g, while the initial mass of zinc was recorded as 0.573 g and the initial mass of iodide was recorded as 0.530 g. The catalyst was then added to test tube #1 with the zinc and iodide. During a constant agitation of the solution, a series of color changes lasting for a period of 5 minutes
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occurred along with noticeable warmth emitted from the bottom of the test tube, identifying an exothermic reaction. The experimenter saw the solution change from a yellowish brown color to a much darker solution of dark red. Then after three minutes the solution colors reversed and returned to its original yellow color then finally a clear solution. At the bottom of the solution remained excess zinc solid which was a silver metallic color. The evidence of the remaining zinc allowed the experimenter to correctly identify the limiting reactant as iodide. The experimenter then decanted the solution into test tube #2 keeping the solid in test tube #1. This decanting
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CHM2045Lab1 - An Analysis Of Production Methods And Costs...

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