For every mole of copper chloride used, how many moles of copper are formed? 3.

Question

For every mole of copper chloride used, how many moles of copper are formed? 3. In an experiment, a student isolated 6.356 g of pure copper from an initial sample of 9.902 g of copper chloride. Determine the empirical formula of this copper chloride compound. Show your work. 4. In an experiment, 3.264 g of zinc chloride, ZnCI_2, yielded 1.468 g of zinc metal. Assuming that the original sample was pure, how much zinc should be obtained? Was all zinc possible from the sample recovered? Calculate the percentage recovery. (Express your answer to the proper number of significant figures.)

Explanation / Answer

2. For every moles of CuCl2, we would get 1 mole of Cu formed.

3. Cu isolated = 6.356 g

moles of Cu = 6.356 g/63.546 g/mol = 0.1 mol

mass of Cl in sample = 9.902 - 6.356 = 3.546 g

moles of Cl = 3.546 g/35.453 g/mol = 0.1 mol

Molar ratio of Cu to Cl is 1 : 1

So empirical formula of the compound is CuCl

4. 1.468 g Zn formed starting with 3.264 g ZnCl2

theoretical yield of zinc = (3.264 g/136.315 g/mol) x 65.409 g/mol = 1.566 g

So not all zinc from sample has been isolated.

percent recovery = 1.468 x 100/1.566 = 93.74%

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