Looking for the answer to question number 6 on this post lab sheet Include Rf va

Question

Looking for the answer to question number 6 on this post lab sheet

Include Rf values (along with your math) for each spot Which was the optimal solvent system for separating the different organic compounds? Why? Both the 100% ethyl acetate and the 1:1 EtOAc:Hex provided similar results but I feel the 1:1 EtOAc.Hex worked best in that our compound rose all the way up the plate meaning the solvent was polar enough. With the 100% EtOAc there was just not enough polarity to move the compound well, and lots of spotting of the compound was left behind. Give your unknown number and say which of the 3 compounds you think your unknown is. Explain your rationale. We had unknown #6 and believe that it is Triphenylmethanol. We found this to be true based on our run in part D. We noticed that on the 1:1 EtOAC:Hex solvent plate and on the 1:9 EtOAc:Hex solvent plate tiphenylmethanol was the exact same Rf value or close to our unknown, while the other compounds were more distant and separated from it. If you used 10 mL of a 1:1 (v/v) HexrEtOAc solution, how many moles of Hexane would be in that solution, and how many moles of Ethyl Acetate would be in that solution? Show your work for full credit.

Explanation / Answer

1:1 hexane and ethyl acetoacetate have 5ml hexane and 5 ml ethyl acetoacetate.

mole caculation of hexane:

density of hexane is .6548 g/ml

so 5 ml hexane means .6548*5 = 3.274 g hexane

now molecular wt. of hexane is 86 g/mol

so mole of hexane is 3.274/86 = .038

mole calculation of ethyl acetoacetate

density of ethyl acetoacetate is 1.021 g/ ml

so 5ml ethyl acetoacetate means 1.021*5 = 5.105 g ethyl acetoacetate

molecular wt. of ethyl acetoacetate = 130 g/ mol

mole of ethyl acetoacetate = 5.105/130 = .0392

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