Aspirin (c9h8o4) is synthesized by reacting salicylic acid (c7h6o3) with acetic anhydride (c4h6o3). the balanced equation isc7h6o3 + c4h6o3 → c9h8o4 + hc2h3o2(a) what mass of acetic anhydride is needed to completely consume 1.00 x 10^2 g salicylic acid? (b) what is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?

For a: The mass of acetic anhydride needed is 73.91 grams.

For b: The theoretical yield of aspirin is 130.43 grams.

Explanation:

To calculate the number of moles, we use the equation:

  .....(1)

Given mass of salicylic acid =

Molar mass of salicylic acid = 138.121 g/mol

Putting values in equation 1, we get:

For the given chemical reaction:

By stoichiometry of the reaction:

1 mole of salicylic acid reacts with 1 mole of acetic anhydride.

So, 0.724 moles of salicylic acid will react with = of acetic anhydride.

Now, to calculate the mass of acetic anhydride, we use equation 1:

Moles of acetic anhydride = 0.724 moles

Molar mass of acetic anhydride = 102.09 g/mol

Putting values in equation 1, we get:

Hence, the mass of acetic anhydride needed is 73.91 grams.

By stoichiometry of the reaction:

1 mole of salicylic acid is producing 1 mole of aspirin.

So, 0.724 moles of salicylic acid will produce = of aspirin.

Now, to calculate the mass of aspirin, we use equation 1:

Moles of aspirin = 0.724 moles

Molar mass of aspirin = 180.158 g/mol

Putting values in equation 1, we get:

Hence, the theoretical yield of aspirin is 130.43 grams.

it would be a gas formation