Question

Using the following atomic weights and that the density of cyclohexanol is 0.96, what is the % yield of a reaction that starts with 5.8 mL of cyclohexanol and ends with 4.2 g of cyclohexene?

Answer 1

D cyclohexanol = 0.96 g/mL

%yield of reaction if...

mass of cyclohexanol = D*V = 5.8*0.96 = 5.568 g of cyclohexanol

MW of cyclohexanol = 100.158 g/mol

mol of cyclohexanol = mass/MW = 5.568 /100.158 = 0.05559 mol of cyclohexanol   

at the end...

mass of cyclohexene= 4.2 g

MW of cyclohexene =82.143

mol of cyclohexene = 4.2/82.143 = 0.051130 mol

in theory...

theoretical yield expected =0.05559 mol

actual yield = 0.051130 mol

so..

%yield = actual/theoretical * 100 = 0.051130 /0.05559 *100 = 91.97%