Pentyl Ethanoate, CH3COOC5H11, which smells like bananas, is produced from the esterification reaction: CH3COOH(aq) +C5H11OH(aq) → CH3COOC5H11(aq) + H2O(l)

A reaction uses 3.58g of CH3COOH and 4.75g of C5H11OH and has a yield of 45.00%. Determine the mass of ester that foorms.

3.16g of the ester are produced

Explanation:

First, we need to determine the limiting reactant of the reaction converting each reactant to moles:

Moles CH3COOH (Molar mass: 60g/mol):

3.58g *  (1mol / 60g) = 0.05967moles

Moles C5H11OH (Molar mass: 88.15g/mol):

4.75g * (1mol / 88.15g) = 0.05389 moles

As the reaction is 1:1, limiting reactant is C5H11OH.

Theoretical moles of the ester CH3COOC5H11 is 0.05389 moles.

As only the 45.00% is produced:

0.05389 moles * 45.00% =

0.02425 moles of CH3COOC5H11 are produced.

In mass (Molar mass CH3COOC5H11: 130.1849g/mol):

0.02425 moles * (130.1849g / mol) =

0.88m hope i am correct : )