Preparation od synthetic banana oil (Post-lab) 1. calculate the amount isopenyl
ID: 894270 • Letter: P
Question
Preparation od synthetic banana oil (Post-lab) 1. calculate the amount isopenyl acetate should be present in the reaction mixture at equilibrium, based on the of start materials you used a the be used the quadratic equation because volumes cancel moles in place of molar concentra (b) e the mass of sopenty was lost as a result of incomplete reaction. (2) during (see oP-30a). Assume that the washings, and (3) during the distillation the ester's solubility in aqueous NaHCO, is about the same as in water Compare the sum of these estimated losses with your actual product loss and try to account for any significant differences. washing? Write b 2. What gas escaped during the sodium bic nced equations for two reactions that took place during this operation 3. (a) Calculate the atom economy and reaction efficiency of your synthe sis of isopentyl ace (b)Tell how the procedure for the preparation of isopentyl acetate might be modified to increase the reaction efficiency (c) Describe some green features of your synthesis, and any that a so green 5. (a) In the "Understanding the Experiment" section, it was stated that the reaction of an equimolar mixture of isopentyl alcohol and acetic acid will produce, at most, 67% of the theoretical amount of isopentyl acetate. Verify this with an equilibrium constant calculation, using K 4.2. (b) Compare this with the corresponding percentage for th conditions used in this experiment (see Exercise 1 Are your results consistent with Le Chatelier's principle? Explain 6. Based on the procedure that you used in this experiment and using the same molar quantities of reactants, develop a procedure that would be suitable for the preparation of isobutyl propionate. Specify the amounts of all materials required and a distillation range for the prod uct. Obtain the necessary physical properties from one of the reference books listed in the Bibliography
Explanation / Answer
1)
I took my original expected yield (which was calculated assuming the reaction was irreversible and there was 100% yield) and multiplied it by (4.2/5.2), as I assumed an equlibrium constant of 4.2 means there are 4.2 moles of products for every 1 mole of reactants at equilibrium. I came up with this:
19.53 grams expected yield * 4.2/5.2 = 15.77 grams true expected yield
2) Acetic acid and sulfuric acid each react with sodium bicarbonate to produce carbon dioxide gas.
CH3COOH + NaHCO3 CH3COONa + CO2 + H2O
H2SO4 + 2 NaHCO3 Na2SO4 + 2 CO2 + 2 H2O
Roger the Mole · 2 years ago