2. The above equation is balanced. What is the percent yield of isoamyl acetate,

Question

2. The above equation is balanced. What is the percent yield of isoamyl acetate, if 1.28g of isoamyl alcohol was added to 2.01g acetic acid, and 0.61 g of isoamyl acetate was extracted from the Hickman Head during distillation? (The isoamyl alcohol was the limiting reagent, so molecular weight can be used to move between mass and moles)

Isoamyl alcohol molecular weight: 88.148 g/mol

Isoamyl acetate molecular weight: 130.19 g/mol

Acetic Acid: 60.05 g/mol

Water: 18.0 g/mol

Percent/yield = Actual Yield/ Theoretical Yield x 100% 2. The above equation is balanced. What is the percent yield of isoamyl acetate, if 1.28g of isoamyl alcohol was added to 2.01g acetic acid, and 0.61 g of isoamyl acetate was extracted from the Hickman Head during distillation? (The isoamyl alcohol was the limiting reagent, so molecular weight can be used to move between mass and moles) Isoamyl alcohol molecular weight: 88.148 g/mol Isoamyl acetate molecular weight: 130.19 g/mol Acetic Acid: 60.05 g/mol Water: 18.0 g/mol

Explanation / Answer

The general mechanism for finding percentage yield is as follows:
1. Balance the chemical equation
2. Find the limiting reagent
3. Find the theoretical yield
4. Find the actual yield

5. Find the percentage yield

Percentage Yield = (mass of Actual Yield/mass of Theoretical Yield) x   100%

1. The given Equation is already balanced.

2. Limiting reagent: is the reactant which the product yield depends on, as it is not in excess. The isoamyl alcohol is the limiting reagent.

moles of isoamyl alcohol = mass/molar mass

                                  = 1.28g/(88.148 g/mol)

                                  = 0.0145 mol

moles of acetic acid = mass/molar mass

                                         = 2.01g/(130.19 g/mol)

                                         = 0.0154 mol

Hence  isoamyl alcohol is limiting reagent.

3. Theoretical Yield: is how much product will be synthesized in ideal conditions. To determine theoretical yield, multiply the amount of moles of the limiting reagent by the ratio of the limiting reagent and the synthesized product and by the molecular weight of the product.

Theoretical Yield = moles of isoamyl acetate x molar mass of isoamyl acetate

Finding the Theoretical Yield

From the balanced chemical equation we know that for every mole of isoamyl alcohol and acetic acid one mole of isoamyl acetate is produced. Since there are more moles of acetic acid than isoamyl alcohol, isoamyl alcohol is used up first as the reaction proceeds. We can conclude that acetic acid is in excess and isoamyl alcohol is the limiting reagent.

Therefore # moles of isoamyl alcohol = # of isoamyl acetate produced

Theoretical Yield = moles of isoamyl acetate x molar mass of isoamyl acetate

                         = 0.0145 mol x 130.19 g/mol

                         = 1.8904g

Percent Yield =  (Actual Yield/Theoretical Yield) x 100% = (0.61 g/1.89g) x 100 % = 32.27%

ANSWER: 32.27%

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