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What is the theoretical yield of aspirin (180.2 g/mol) in the reaction of 2.94 grams of salicylic acid (138.1 g/mol) with excess acetic anhydride (102.1 g/mol)? Show your work. Include UNITS and round your final answer appropriately.

Respuesta :

Answer:

Theoretical Yield of Aspirin = 3.84 g

Explanation:

The reaction between salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) to form aspirin(C9H8O4) and acetic acid (HC2H3O2) is:

[tex]C7H6O3 + C4H6O3 \rightarrow  C9H8O4 + HC2H3O2[/tex]

Mass of salicylic acid present = 2.94 g

Molar Mass of salicylic acid = 138.1 g/mol

[tex]Mole\ salicylic\ acid = \frac{2.94}{138.1g/mol} =0.0213\ moles[/tex]

Since acetic anhydride is in excess, salicylic acid will be the limiting reagent and will determine the amount of product formed.

Based on the reaction stoichiometry:

1 mole of salicylic acid yields 1 mole of aspirin

Therefore, Moles of aspirin = 0.0213

Molar mass of aspirin = 180.2 g/mol

[tex]Mass (aspirin) = moles*mol mass = 0.0213 * 180.2 =3.84 g[/tex]

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