Question

1.2 pts.) Complete the following (assume that mass and weight are equivalents), a) The weight of your alcohol that you started with = 1. 9 b) The molecular weight of your alcohol = 102.17 gimo ne number of moles of your alcohol in your sample that you used to start the reaction = 0.01297 more d) The number of molecules of your alcohol in your sample that you used to start the reaction = (6.023 x 10 molecules 0.01297 moles) = 2. (2 pts) Complete the following (assume that mass and weight are equivalents), a) The weight of acetic acid that you started with = 2.5804 b) The molecular weight of acetic acid = 60.052 Simol c) The number of moles of acetic acid in your sample that you used to start the reaction = 0.04103 mores d) The number of molecules of acetic acid in your sample that you used to start the reaction (6.023X1023 molecules) (0.4036 moles): 3. (1 pt.) Which is the limiting reagent/reactant? The limiting is the alcohol, l-hexanol, 4. (1 pt.) What is the maximum possible yield of ester in moles, based on the limiting reactant/reagent given above? (this is the theoretical yield, in moles) 1.3259 102,17glmul. 297 moles / 5. (2 pts.) Give the number of moles of your ester product (or use borrowed data and indicate so) (assume that mass and weight are equivalent), show the equation you used and all units. 6. (2 pts.) Give the percent yield of your ester product based on the theoretical yield. Show all equations and units.

Answer 1

си , но Madars to gange 144.22g/mol I max: 1.325g 2.586g No. of moles of ester- observed yield molar massester (144.22) yield- obserund gield xloo Theoretical gield Theoretical yield = 0.01297 x 48:22g mo = 18703 g

you did not mention how much observed yield you got. please put the value in the formula and do calculate accordingly.

for the last question experimental procedure is required to know where Amberlyst is used.