Ethyl butyrate is an artificial fruit flavor commonly used in the food industry for such flavors as orange and pineapple. It can be produced by the reaction of butanoic acid with ethanol in the presence of an acid catalyst.
i) Given 8.45g of butanoic acid and excess ethanol, how many grams of ethyl butyrate would be synthesized, assuming a complete 100 yield?
ii) A chemist ran the reaction and obtained 5.25 of ethyl butyrate. What was the percent yield?
iii) The chemist discovers a more efficient catalyst that can produce ethyl butyrate with a 78.0 yield. How many grams would be produced from 8.45 of butanoic acid and excess ethanol?
To answer these questions, we will need to calculate the amount of ethyl butyrate produced in each scenario. Let's proceed step-by-step:
i) Given 8.45g of butanoic acid, we need to determine how many grams of ethyl butyrate would be synthesized assuming a complete 100% yield.
The balanced equation for the reaction is:
Butanoic acid + ethanol -> ethyl butyrate + water
The molar mass of butanoic acid is 88.11 g/mol, and the molar mass of ethyl butyrate is 116.16 g/mol.
To calculate the theoretical yield, we need to convert 8.45g of butanoic acid to moles using its molar mass:
8.45g butanoic acid * (1 mol butanoic acid / 88.11 g) = 0.0959 mol butanoic acid
According to the balanced equation, the ratio between butanoic acid and ethyl butyrate is 1:1. Therefore, the moles of ethyl butyrate produced would be the same as the moles of butanoic acid:
0.0959 mol ethyl butyrate
Finally, we can convert this back to grams by multiplying by the molar mass of ethyl butyrate:
0.0959 mol ethyl butyrate * (116.16 g / 1 mol ethyl butyrate) = 11.2g ethyl butyrate
Therefore, if the reaction had a complete 100% yield, 11.2 grams of ethyl butyrate would be synthesized.
ii) If the chemist obtained 5.25g of ethyl butyrate, we need to calculate the percent yield.
To calculate the percent yield, we divide the actual yield by the theoretical yield and multiply by 100:
Percent yield = (actual yield / theoretical yield) * 100
Percent yield = (5.25g / 11.2g) * 100 = 46.9%
Therefore, the percent yield of ethyl butyrate in this case is 46.9%.
iii) If a more efficient catalyst is discovered that can produce ethyl butyrate with a 78.0% yield, we can use the same approach to calculate the amount of ethyl butyrate produced.
Using the percent yield of 78.0%, we can calculate the theoretical yield as follows:
Theoretical yield = (percent yield / 100) * actual yield
Theoretical yield = (78.0 / 100) * 8.45g = 6.59g
Therefore, if the reaction had a 78.0% yield, 6.59 grams of ethyl butyrate would be produced.
i) To calculate the number of grams of ethyl butyrate synthesized, we need to use the stoichiometry of the reaction and the masses of the reactants.
The balanced equation for the reaction is:
Butanoic acid + Ethanol → Ethyl butyrate + Water
From the balanced equation, we can see that 1 mole of butanoic acid reacts with 1 mole of ethanol to produce 1 mole of ethyl butyrate.
First, calculate the number of moles of butanoic acid:
Molar mass of butanoic acid (C4H8O2) = 88 g/mol
Number of moles of butanoic acid = Mass of butanoic acid / Molar mass of butanoic acid
Number of moles of butanoic acid = 8.45 g / 88 g/mol
Next, since the reaction has a 1:1 stoichiometric ratio between butanoic acid and ethyl butyrate, the number of moles of ethyl butyrate produced will be the same as the number of moles of butanoic acid.
Finally, calculate the mass of ethyl butyrate produced:
Mass of ethyl butyrate = Number of moles of ethyl butyrate × Molar mass of ethyl butyrate
ii) To calculate the percent yield, we need to compare the actual yield (5.25 g) to the theoretical yield (calculated in part i)).
Percent yield = (Actual yield / Theoretical yield) × 100
iii) To calculate the number of grams of ethyl butyrate produced with a 78.0% yield, we follow the same steps as in part i), but consider the given percent yield in the calculation.
First, calculate the theoretical yield:
Theoretical yield = Mass of butanoic acid × Percent yield
Finally, calculate the mass of ethyl butyrate produced:
Mass of ethyl butyrate = Theoretical yield × Molar mass of ethyl butyrate
i)
Write and balance the reaction. I think the compounds are 1:1 ratio of mols.
Convert 8.45 g butanoic acid to mols. mol = grams/molar mass.
Use the coefficients in the balanced equation to convert mols butanoic acid to mols of the product. I believe mols butanoic acid = mols or the product.
Convert mols of the product to grams. g = mols x molar mass. This is the theoretical yield (TY)
ii)
Actual yield (AY) is 5.25 g from the problem.
%yield = (AY/TY)*100 = ?
iii)
Use the equation in ii to do this. Substitute and solve for AY.