Respuesta :
Answer: The percent yield of the reaction is 87.24 %.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
- For acetic acid:
Given mass of acetic acid = 6.289 g
Molar mass of acetic acid = 60 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of acetic acid}=\frac{6.289g}{60g/mol}=0.105mol[/tex]
- For isoamyl alcohol:
Given mass of isoamyl alcohol = 3.75 g
Molar mass of isoamyl alcohol = 88.15 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of isoamyl alcohol}=\frac{3.75g}{88.15g/mol}=0.0425mol[/tex]
The chemical equation for the reaction of acetic acid and isoamyl alcohol follows:
[tex]\text{Acetic acid + Isoamyl alcohol}\rightarrow \text{Isoamyl acetate}[/tex]
By Stoichiometry of the reaction:
1 mole of isoamyl alcohol reacts with 1 mole of acetic acid
So, 0.0425 moles of isoamyl alcohol will react with = [tex]\frac{1}{1}\times 0.0425=0.0425mol[/tex] of acetic acid
As, given amount of acetic acid is more than the required amount. So, it is considered as an excess reagent.
Thus, isoamyl alcohol is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of isoamyl alcohol produces 1 mole of isoamyl acetate
So, 0.0425 moles of isoamyl alcohol will produce = [tex]\frac{1}{1}\times 0.0425=0.0425moles[/tex] of isoamyl acetate
Now, calculating the mass of isoamyl acetate from equation 1, we get:
Molar mass of isoamyl acetate = 130.2 g/mol
Moles of isoamyl acetate = 0.0425 moles
Putting values in equation 1, we get:
[tex]0.0425mol=\frac{\text{Mass of isoamyl acetate}}{130.2g/mol}\\\\\text{Mass of isoamyl acetate}=(0.0425mol\times 130.2g/mol)=5.534g[/tex]
- To calculate the percentage yield of isoamyl acetate, we use the equation:
[tex]\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100[/tex]
Experimental yield of isoamyl acetate = 4.828 g
Theoretical yield of isoamyl acetate = 5.534 g
Putting values in above equation, we get:
[tex]\%\text{ yield of isoamyl acetate}=\frac{4.828g}{5.534g}\times 100\\\\\% \text{yield of isoamyl acetate}=87.24\%[/tex]
Hence, the percent yield of the reaction is 87.24 %.
