For the reaction:
acetic acid (2g) + Isopentyl alcohol (0.9g) =>
Isopently acetate(1.15g)+ H2O
I'm suposed to determine the limiting reagent, theoretical yield and percent yield from this reaction but the reaction was given as a picture...
I'm not sure about the mole ratio though.
It only shows one molecule for each, however I was wondering if it was a 1:1 ratio of 1mol acetic acid and one mol Isopentyl alcohol that results in 1 mol of Isopentyl acetate and 1mol water.
And If it is a one to one ratio, how would a 2:1 or any other ratio besides a 1:1 ratio look in a drawing of the molecule for the reaction?
would there be a 2 and the molecule would be in brackets or something?
Thank You=)
I have no idea how it would look in a drawing but I presume it would show two molecules if it was a 2:1 ratio. However, you need not worry about that because it is a 1:1 reaction. 1 mol alcohol + 1 mol acid produces 1 mol of the ester.
Thank you very much Dr.Bob =D
To determine the limiting reagent, theoretical yield, and percent yield of the reaction, you need to first determine the mole ratio between the reactants. From the balanced chemical equation, the reaction appears to be a 1:1 ratio, where 1 mol of acetic acid reacts with 1 mol of Isopentyl alcohol to produce 1 mol of Isopentyl acetate and 1 mol of water.
However, you mentioned that the reaction was given as a picture, and you are unsure if other ratios are involved. In that case, it would be best to consult the picture or the original source for more information on the specific reaction conditions and stoichiometry.
Regarding how different ratios would appear in a drawing of the molecule, it is not common to represent the stoichiometric ratios through the molecular structure itself. The molecular structure represents the arrangement of atoms in a molecule and does not explicitly show the stoichiometric ratios. The ratios are typically indicated using coefficients in the balanced chemical equation.
Once you have the mole ratio between the reactants (if different from 1:1), you can compare the actual ratio of the given amounts of reactants to the stoichiometric ratio to determine the limiting reagent. The limiting reagent is the reactant that is completely consumed and determines how much product is formed.
The theoretical yield is the maximum amount of product that can be obtained based on the limiting reagent. It is calculated by converting the limiting reagent's mass (given or determined) to moles, using the molar mass, and then converting it to the mass of the desired product using the stoichiometry of the reaction.
Finally, the percent yield is calculated by dividing the actual yield (given or determined) by the theoretical yield, and then multiplying by 100.
Overall, to fully determine the limiting reagent, theoretical yield, and percent yield of the reaction, you need to have additional information about the reaction conditions, stoichiometry, and actual yield.