Consider the following reaction between cyclohexene and hydrogen bromide: Cycloh
ID: 1065635 • Letter: C
Question
Consider the following reaction between cyclohexene and hydrogen bromide: Cyclohexene (C_6H_12): molecular weight = 82.14 g/mol; density = 0.811 g/mL HBr acid: 30% by weight solution (30 grams/100 mL) How many grams of cyclohexene are involved in this reaction? How many grams of hydrobromic acid are involved in this reaction? How many moles of cyclohexene are involved? How many moles of hydrobromic acid are involved? Which compound is the limiting reagent? What is the maximum number of moles of product that can form? What is the maximum number of grams of products that can form? What would be the percent yield if 25 grams of product are isolated?Explanation / Answer
how many grams of cyclohexene involved in this reaction : mass = D x V = 0.811 x 40 = 32.44 gms
how many grams of hydrogen bromide involved in this reaction : mass = D x V = 1.49 x 30 = 44.7 gms
how many moles of cyclohexene is involved : mass/molar mass = 32.44/82.14 = 0.39 moles
how many moles of hydrogen bromide is involved : mass/molar mass = 44.7/80.91 = 0.55 moles
which compound is the limiting reagent = cyclohexene is the limiting reagent
what is the maximum no. of moles product can be formed :
for 1 mole of cyclohexene 100 % yield = 162 g
then for 0.39 mole = 32.44 x 162/82.14 = 64 g
64/162 = 0.39 moles
what is the maximum number of grams of product can be formed : 64 gms
what would be the yield if 25 gms of product is isolated : 25/64 x 100 = 39.06 %