Calculate the theoretical yield of acetylsalicylic acid from 2.01 g of salicylic acid assuming excess acetic anhydride.
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First, we need to know the molecular weight of salicylic acid. The molecular weight of salicylic acid is approximately 138.12 g/mol. Show more…
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Calculate the theoretical yield of aspirin (FW = 180.158 g/mol) for a reaction where 2.734 g of salicylic acid (FW = 138.121 g/mol) is reacted with excess acetic anhydride?
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If 3.5 g of salicylic acid is heated with an excess of acetic anhydride, what is the theoretical yield of acetylsalicylic acid?
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Aspirin or acetyl salicylic acid is synthesized by reacting salicylic acid with acetic anhydride: $$ \mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3} \quad \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2} $$ $\begin{array}{lll}\text { salicylic acid } & \text { acetic anhydride } & \text { aspirin } & \text { acetic acid }\end{array}$ (a) How much salicylic acid is required to produce $0.400 \mathrm{~g}$ of aspirin (about the content in a tablet), assuming acetic anhydride is present in excess? (b) Calculate the amount of salicylic acid needed if only $74.9$ percent of salicylic acid is converted to aspirin. (c) In one experiment, $9.26 \mathrm{~g}$ of salicylic acid is reacted with $8.54 \mathrm{~g}$ of acetic anhydride. Calculate the theoretical yield of aspirin and the percent yield if only $10.9 \mathrm{~g}$ of aspirin is produced.
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