create a balanced chemical equation and theoretical yield

In this experiment, you will be given an impure sample of fluorene. Your goal will be to find a good solvent for crystallizing the sample. You should try water, methyl alcohol, and toluene. After you have determined which is the best solvent, crystallize the remaining material. Finally, determine the melting point of the purified compound and of the impure sample. Salectling a Solvent. Perform the procedure given in Technique 11, Section 11.6 with three sepe: rate samples of impure fluorene. Use the following solvents: methyl alcohol, water, and toluene. Crystalibing the Sample. After you have found a good solvent, crystallize 0.75g of impure fluorene using the procedure given in Experiment 2A. Weigh the impure sample carefully and be sure to keep a little of it for loter determination of the meiting point. After filtering the crystals on the Bochner funnel, transfer the crystals to a preweighed watch glass and allow them to airdry. If water was used as the solvent, you may need to let the crystals sit out overnight to dry, because water is less volatile than most organic solvents. Weigh the dried sample and calculate the percentege recovery. Determine the melting point of both the pure sample and the original impure meterial. The literature melting point for pure fluorene is 116C117C. At the option of the instructor, turn in your crystalized material in a properly labeled container. 3 The impure fluorene contains 5% fluorenane, a yellow compound