While performing the assays for the LDH kinetics experiment, you will pipet 25ul of 250 ug/ml LDH into 975 ul of assay buffer (T
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<u>Answer:</u> The percent yield of the aspirin is 77.5 %.
<u>Explanation:</u>
To calculate the mass of acetic anhydride, we use the equation:
Density of acetic anhydride = 1.08 g/mL
Volume of acetic anhydride = 2.80 mL
Putting values in above equation, we get:
To calculate the number of moles, we use the equation:
.....(1)
- <u>For acetic anhydride:</u>
Given mass of acetic anhydride = 3.024 g
Molar mass of acetic anhydride = 102.1 g/mol
Putting values in equation 1, we get:
- <u>For salicylic acid:</u>
Given mass of salicylic acid = 1.24 g
Molar mass of salicylic acid = 138.12 g/mol
Putting values in equation 1, we get:
The chemical equation for the combustion of hexane follows:
By Stoichiometry of the reaction:
1 mole of salicylic acid reacts with 1 mole of acetic anhydride
So, 0.0089 moles of salicylic acid will react with = of acetic anhydride
As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.
Thus, salicylic acid is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of salicylic acid produces 1 mole of aspirin
So, 0.0089 moles of salicylic acid will produce = of aspirin
Now, calculating the mass of aspirin from equation 1, we get:
Molar mass of aspirin = 180.16 g/mol
Moles of aspirin = 0.0089 moles
Putting values in equation 1, we get:
- To calculate the percentage yield of aspirin, we use the equation:
Experimental yield of aspirin = 1.24 g
Theoretical yield of aspirin = 1.60 g
Putting values in above equation, we get:
Hence, the percent yield of the aspirin is 77.5 %.