Yes...another calculation problem.
Rxn:
1ml isopentyl alcohol + 1.5ml glacial acetic acid + 3 drops sulfuric acid=> isopentyl acetate
to calculate the theoretical yield..
I know that the acetic acid is in excess but how would I calculate the theoretical yield?
is it just find moles acetic acid (know excess) and then since I do know that the ratio is 1:1 then I can just find theoretical yield directly?
Another question is...
1) What catalyst is used in the experiment?
I say it's the sulfuric acid.
2) since one method of formation of ester is to add excess acetic acid. What is another way to form the ester which will favor the formation fo ester
I said that you could add excess isopentyl alcohol
3) Why is it easier to remove excess acetic acid from products than excess isopentyl alcohol?
No idea about this question.
Thank you
Is the last question with the "why is it easier to remove excess acetic acid from products than excess isopentyl alcohol?"
because I can just use sodium bicarbonate to remove the acid?
Is there a method to remove the isopentyl alcohol though?
To calculate the theoretical yield of isopentyl acetate in this reaction, you first need to find the limiting reactant. From the given information, it is clear that glacial acetic acid is in excess, so it is not the limiting reactant.
To determine the limiting reactant, you can start by calculating the number of moles of isopentyl alcohol and glacial acetic acid used. You can convert the given volumes of each reactant to moles using their respective molar masses and the formulas:
Molar mass of isopentyl alcohol = 88.15 g/mol
Molar mass of glacial acetic acid = 60.05 g/mol
Next, you need to compare the moles of isopentyl alcohol and glacial acetic acid to find which one is the limiting reactant. Since the reaction ratio is 1:1 between isopentyl alcohol and isopentyl acetate, the limiting reactant will be the one with fewer moles.
Once you determine the limiting reactant, you can use its mole ratio with the product, which is 1:1, to calculate the theoretical yield of isopentyl acetate. This value represents the maximum amount of isopentyl acetate that can be obtained under ideal conditions.
Regarding the catalyst used in the experiment, you are correct that sulfuric acid acts as a catalyst. It helps the reaction proceed at a faster rate by lowering the activation energy. The role of the catalyst is to increase the rate of reaction without being consumed or taking part in the reaction itself.
To answer the question about another method to favor the formation of ester, you suggested adding excess isopentyl alcohol. This is a valid approach. By increasing the concentration of isopentyl alcohol, the reaction equilibrium will shift to favor the formation of more isopentyl acetate.
Regarding the question about why it is easier to remove excess acetic acid from products than excess isopentyl alcohol, we need to consider the properties of these compounds. Acetic acid is a volatile liquid, meaning it has a high vapor pressure and tends to evaporate easily. This property makes it easier to remove excess acetic acid by evaporation or by distillation. On the other hand, isopentyl alcohol has a higher boiling point and is less volatile, making it more difficult to remove by simple evaporation or distillation.