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You are watching: What is the theoretical yield of aspirin

The post-lab inquiries provided are SIMILAR to concerns you may encounter in your lab hand-operated. These questions will certainly provide you with a step-by-action guide on how we approached the trouble. You deserve to usage this overview and the data you videotaped to help answer the inquiries. Any given examples with worths will be via mock worths. Use of these worths will certainly almost assuredly give you nonsensical calculations. They are just expected to illustrate the logic.


question 1

You are asked to calculate the percent yield of aspirin, offer what the value must be (theoretical yield), and describe why your value (actual yield) might vary from this

From the above reaction we understand the amount of salicylic acid is a 1 to 1 (1:1) ratio through the amount of aspirin. This implies eincredibly mole of salicylic acid provided will yield the same variety of moles of aspirin. Thus, the first action is to calculate the variety of moles of salicylic acid provided. Note: you are told that acetic anyhydride is in excess and salicylic acid is the limiting reagent

Mass of Salicylic Acid Used (mock value) = 276.24 g

Molar Mass of Salicylic Acid = 138.12 g

Moles of Salicylic Acid = (1)/(2) = 276.24/138.12 = 2.000 moles

To then convert the number moles of Aspirin to the intended yield in grams, we multiply the moles by the molar mass of asprin

Moles of Salicylic Acid = Moles of Aspirin —> 2 moles of Salicylic Acid provides 2 moles of Asprin

Molar Mass of Aspirin = 180.16 g

Theoretical yield of Aspirin (g) = (2 moles)(molar mass of aspirin) = 2.000(180.16) = 360.3 grams

Percent Yield Calculation (remember significant figures)

Your actual yield will certainly be the amount aspirin you weighed after it was filtered and dried in lab. Using the theoretical and also actual you can calculate percent yield.

Actual Yield of Aspirin in lab after filtered/dried (mock value) = 370 g

Mass of Theoretical Yield of Aspirin (mock value) = 360.3 g

Percent Yield = (Actual ÷ Theoretical) x 100 = (370 ÷ 360.3) x 100 = 103 %

Your worth might differ from the theoretical value for a number of factors. If it is over 100%, it may be because your aspirin was not totally dried. If it is below 100%, it might be bereason of sample loss once carrying to the weigh paper.

Inquiry 2

Asks you between aspirin and salicylic acid, which reacts via FeCl3FeCl3 just reacts via copounds that have phenols. Determine whether aspirin or salicylic acid has a phenol and also that should be the one that reacts via FeCl3

View fulldimension

Phenols (click to enlarge)

Concern 3

Asks you to discover 3 prevalent esters and also attract the structures.

Just google it.


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