Before Reaction Massof empty Erlenmeyer flask 85.35g Mass of Zn and Erlenmeyer flask 86.90g Mass of iodine 1.65g After Reaction Mass of Erlenmeyer flask and unreacted zinc 86.56g Calculate the following: (a). moles of Zn - (b). moles of I -
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Change in mass of Zn = Mass of Zn and Erlenmeyer flask - Mass of empty Erlenmeyer flask Change in mass of Zn = 86.90g - 85.35g Change in mass of Zn = 1.55g Now, we can calculate the moles of Zn using its molar mass. Molar mass of Zn = 65.38 g/mol Moles of Zn Show more…
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Chemistry 110 Laboratory Empirical Formula of Zinc Iodide Report Sheet Trial 1 Trial 2 Mass of zinc at start: 2.025 g 2.090 g Mass of iodine at start: 2.082 g 2.057 g Mass of dry zinc left over: 1.477 g 1.562 g Mass of zinc reacted: 0.548 g 0.528 g Moles of zinc reacted: 0.00838 mol 0.00807 mol Moles of iodine* reacted: 0.01641 mol 0.01621 mol * as iodine atoms Show calculations below for determining empirical formula:
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If at the end of the reaction some of the unreacted zinc escaped from the Erlenmeyer flask, the mass of the flask plus the unreacted zinc would be lower than it should be. Would this cause the calculated mole ratio (mol I/mol Zn) to be higher or lower than the actual value (Iodine is the limiting reactant in this reaction)? Explain
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Zinc (Zn) and Iodine (I2) react to form Zinc Iodide (ZnI2) at room temperature (Given 50.0g of Zinc and 50.0g of Iodine). What is Moles Zn in 50.0g, Mole I2 in 50.0 grams. Identify limiting reactant and excess element and Grams of excess element.
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